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	<id>https://teaching.ncl.ac.uk/bms/wiki//api.php?action=feedcontributions&amp;feedformat=atom&amp;user=090012763</id>
	<title>The School of Biomedical Sciences Wiki - User contributions [en]</title>
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	<updated>2026-04-14T23:53:07Z</updated>
	<subtitle>User contributions</subtitle>
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	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=1253</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=1253"/>
		<updated>2010-11-17T18:32:39Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Blood Pressure]] &lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Blood group systems]] &lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System. &lt;br /&gt;
&lt;br /&gt;
== See also ==&lt;br /&gt;
&lt;br /&gt;
#[[Haemoglobin]]&lt;br /&gt;
#[[Hypertension]]&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems.]&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1017</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1017"/>
		<updated>2010-11-15T18:15:53Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&#039;&#039;&#039;&amp;lt;br&amp;gt;&#039;&#039;&#039; &lt;br /&gt;
&lt;br /&gt;
{| cellspacing=&amp;quot;1&amp;quot; cellpadding=&amp;quot;1&amp;quot; border=&amp;quot;1&amp;quot; align=&amp;quot;center&amp;quot; style=&amp;quot;width: 451px; height: 140px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
| &#039;&#039;&#039;Blood group&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Antigen(s) present on erythrocytes&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Antibodies present in plasma&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Genotype(s)&#039;&#039;&#039;&lt;br /&gt;
|-&lt;br /&gt;
| A &lt;br /&gt;
| A antigen &lt;br /&gt;
| Anti-B &lt;br /&gt;
| AA or AO&lt;br /&gt;
|-&lt;br /&gt;
| B &lt;br /&gt;
| B antigen &lt;br /&gt;
| Anti-A &lt;br /&gt;
| BB or BO&lt;br /&gt;
|-&lt;br /&gt;
| AB &lt;br /&gt;
| A and B antigens &lt;br /&gt;
| none &lt;br /&gt;
| AB&lt;br /&gt;
|-&lt;br /&gt;
| O &lt;br /&gt;
| none &lt;br /&gt;
| Anti-A and B &lt;br /&gt;
| OO&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface. &lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt; &lt;br /&gt;
*[http://www.ncbi.nlm.nih.gov/bookshelf/br.fcgi?book=rbcantigen&amp;amp;part=ch05ABO The ABO blood group]&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1011</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1011"/>
		<updated>2010-11-15T18:08:07Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&#039;&#039;&#039;&amp;lt;br&amp;gt;&#039;&#039;&#039; &lt;br /&gt;
&lt;br /&gt;
{| cellspacing=&amp;quot;1&amp;quot; cellpadding=&amp;quot;1&amp;quot; border=&amp;quot;1&amp;quot; align=&amp;quot;center&amp;quot; style=&amp;quot;width: 451px; height: 140px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
| &#039;&#039;&#039;Blood group&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Antigen(s) present on erythrocytes&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Antibodies present in plasma&#039;&#039;&#039; &lt;br /&gt;
| &#039;&#039;&#039;Genotype(s)&#039;&#039;&#039;&lt;br /&gt;
|-&lt;br /&gt;
| A &lt;br /&gt;
| A antigen &lt;br /&gt;
| Anti-B &lt;br /&gt;
| AA or AO&lt;br /&gt;
|-&lt;br /&gt;
| B &lt;br /&gt;
| B antigen &lt;br /&gt;
| Anti-A &lt;br /&gt;
| BB or BO&lt;br /&gt;
|-&lt;br /&gt;
| AB &lt;br /&gt;
| A and B antigens &lt;br /&gt;
| none &lt;br /&gt;
| AB&lt;br /&gt;
|-&lt;br /&gt;
| O &lt;br /&gt;
| none &lt;br /&gt;
| Anti-A and B &lt;br /&gt;
| OO&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface. &lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1007</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1007"/>
		<updated>2010-11-15T18:06:49Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm, Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&#039;&#039;&#039;&amp;lt;br&amp;gt;&#039;&#039;&#039;&lt;br /&gt;
&lt;br /&gt;
{| cellspacing=&amp;quot;1&amp;quot; cellpadding=&amp;quot;1&amp;quot; border=&amp;quot;1&amp;quot; align=&amp;quot;center&amp;quot; style=&amp;quot;width: 451px; height: 140px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
| &#039;&#039;&#039;Blood group&#039;&#039;&#039;&lt;br /&gt;
| &#039;&#039;&#039;Antigen(s) present on erythrocytes&#039;&#039;&#039;&lt;br /&gt;
| &#039;&#039;&#039;Antibodies present in plasma&#039;&#039;&#039;&lt;br /&gt;
| &#039;&#039;&#039;Genotype(s)&#039;&#039;&#039;&lt;br /&gt;
|-&lt;br /&gt;
| A&lt;br /&gt;
| A antigen&lt;br /&gt;
| Anti-B&lt;br /&gt;
| AA or AO&lt;br /&gt;
|-&lt;br /&gt;
| B&lt;br /&gt;
| B antigen&lt;br /&gt;
| Anti-A&lt;br /&gt;
| BB or BO&lt;br /&gt;
|-&lt;br /&gt;
| AB&lt;br /&gt;
| A and B antigens&lt;br /&gt;
| none&lt;br /&gt;
| AB&lt;br /&gt;
|-&lt;br /&gt;
| O&lt;br /&gt;
| none&lt;br /&gt;
| Anti-A and B&lt;br /&gt;
| OO&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface.&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1002</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1002"/>
		<updated>2010-11-15T17:57:34Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm, Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
{| cellspacing=&amp;quot;1&amp;quot; cellpadding=&amp;quot;1&amp;quot; border=&amp;quot;1&amp;quot; style=&amp;quot;width: 295px; height: 61px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
| &#039;&#039;&#039;Phenotype&#039;&#039;&#039;&amp;lt;br&amp;gt; &lt;br /&gt;
| A&amp;lt;br&amp;gt; &lt;br /&gt;
| B&amp;lt;br&amp;gt; &lt;br /&gt;
| AB&amp;lt;br&amp;gt; &lt;br /&gt;
| O&amp;lt;br&amp;gt;&lt;br /&gt;
|-&lt;br /&gt;
| &#039;&#039;&#039;Genotype&#039;&#039;&#039;&amp;lt;br&amp;gt; &lt;br /&gt;
| AA or AO&amp;lt;br&amp;gt; &lt;br /&gt;
| BB or BO&amp;lt;br&amp;gt; &lt;br /&gt;
| AB&amp;lt;br&amp;gt; &lt;br /&gt;
| OO&amp;lt;br&amp;gt;&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface.&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1001</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1001"/>
		<updated>2010-11-15T17:57:09Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm, Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
{| cellspacing=&amp;quot;1&amp;quot; cellpadding=&amp;quot;1&amp;quot; border=&amp;quot;1&amp;quot; style=&amp;quot;width: 295px; height: 61px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
| [[&#039;&#039;&#039;Phenotype&#039;&#039;&#039;]]&amp;lt;br&amp;gt;&lt;br /&gt;
| A&amp;lt;br&amp;gt;&lt;br /&gt;
| B&amp;lt;br&amp;gt;&lt;br /&gt;
| AB&amp;lt;br&amp;gt;&lt;br /&gt;
| O&amp;lt;br&amp;gt;&lt;br /&gt;
|-&lt;br /&gt;
| [[&#039;&#039;&#039;Genotype&#039;&#039;&#039;]]&amp;lt;br&amp;gt;&lt;br /&gt;
| AA or AO&amp;lt;br&amp;gt;&lt;br /&gt;
| BB or BO&amp;lt;br&amp;gt;&lt;br /&gt;
| AB&amp;lt;br&amp;gt;&lt;br /&gt;
| OO&amp;lt;br&amp;gt;&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface.&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1000</id>
		<title>Blood group systems</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood_group_systems&amp;diff=1000"/>
		<updated>2010-11-15T17:47:43Z</updated>

		<summary type="html">&lt;p&gt;090012763: Created page with &amp;#039;&amp;#039;&amp;#039;&amp;#039;Blood group&amp;#039;&amp;#039;&amp;#039; (or &amp;#039;&amp;#039;&amp;#039;blood type&amp;#039;&amp;#039;&amp;#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the Intern…&amp;#039;&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Blood group&#039;&#039;&#039; (or &#039;&#039;&#039;blood type&#039;&#039;&#039;) is a term used to clasify blood based on the presence or absence of a specific antigen on red blood cells surface. According to the International Society of Blood Transfusion, there are about 30 human blood group systems recognized so far&amp;lt;ref&amp;gt;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm, Table of blood group systems, ISBT (August 2008). Retrieved on 15 November 2010.&amp;lt;/ref&amp;gt;.&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== ABO blood group system&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
The most common blood group system being used nowadays is ABO blood group system. In this system, there are 4 classification of blood types. They are group A, B, AB and O. These groups are classified according to the presence or absence of ABO antigen. &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Rh blood group system&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Rh blood group system is the second most important system in determining blood groups. It is based on the presence or absence of D antigen on the red blood cells surface.&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Blood]]&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== External links&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=974</id>
		<title>Goldman equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=974"/>
		<updated>2010-11-15T15:32:01Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Goldman equation&#039;&#039;&#039; is an equation used to calculate the electrical equilibium potential across the cell&#039;s membrane in the presence of more than one ions taking into account the selectivity of membrane&#039;s permeability. It is derived from the Nernst equation. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The Goldman equation can be expressed as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman eqn1.png|412x105px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman eqn2.png|520x124px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol-1 &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol-1 &lt;br /&gt;
&lt;br /&gt;
P&amp;lt;sub&amp;gt;A or B &amp;lt;/sub&amp;gt;is the permeability of the membrane to a particular ion (A or B) &lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;o&amp;lt;/sub&amp;gt; is the concentration of ion outside the membrane &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;i&amp;lt;/sub&amp;gt; is the concentration of ion inside the membrane&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
*[[Nernst equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=972</id>
		<title>Goldman equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=972"/>
		<updated>2010-11-15T15:30:29Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Goldman equation&#039;&#039;&#039; is an equation used to calculate the electrical equilibium potential across the cell&#039;s membrane in the presence of more than one ions taking into account the selectivity of membrane&#039;s permeability. It is derived from the Nernst equation. &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Equation&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
The Goldman equation can be expressed as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman eqn1.png|412x105px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman eqn2.png|520x124px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol-1 &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol-1 &lt;br /&gt;
&lt;br /&gt;
P&amp;lt;sub&amp;gt;A or B &amp;lt;/sub&amp;gt;is the permeability of the membrane to a particular ion (A or B) &lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;o&amp;lt;/sub&amp;gt; is the concentration of ion outside the membrane &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;i&amp;lt;/sub&amp;gt; is the concentration of ion inside the membrane&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Nernst equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=971</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=971"/>
		<updated>2010-11-15T15:29:06Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential|Membrane potential]] &lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;]&amp;lt;sub&amp;gt;o&amp;lt;/sub&amp;gt; is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;]&amp;lt;sub&amp;gt;i&amp;lt;/sub&amp;gt; is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing study of frog skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
=== Goldman equation  ===&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Goldman equation]] &lt;br /&gt;
&lt;br /&gt;
In presence of more than one ion, the Nernst equation can be modified into Hodgkin-Katz-Goldman equation or is commonly known as Goldman equation. Goldman equation is proposed by David E. Goldman of Columbia University together with Alan L. Hodgkin and Bernard Katz. &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
*[[Membrane potential]]&amp;lt;br&amp;gt; &lt;br /&gt;
*[[Goldman equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=969</id>
		<title>Goldman equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Goldman_equation&amp;diff=969"/>
		<updated>2010-11-15T15:27:50Z</updated>

		<summary type="html">&lt;p&gt;090012763: Created page with &amp;#039;&amp;#039;&amp;#039;&amp;#039;Goldman equation&amp;#039;&amp;#039;&amp;#039; is an equation used to calculate the electrical equilibium potential across the cell&amp;#039;s membrane in the presence of more than one ions taking into account t…&amp;#039;&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Goldman equation&#039;&#039;&#039; is an equation used to calculate the electrical equilibium potential across the cell&#039;s membrane in the presence of more than one ions taking into account the selectivity of membrane&#039;s permeability. It is derived from the Nernst equation. &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Equation&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
The Goldman equation can be expressed as follows:&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman_eqn1.png]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[[Image:Goldman_eqn2.png]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol-1&lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC&lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion)&lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol-1&lt;br /&gt;
&lt;br /&gt;
P&amp;lt;sub&amp;gt;A or B &amp;lt;/sub&amp;gt;is the permeability of the membrane to a particular ion (A or B)&lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;o&amp;lt;/sub&amp;gt; is the concentration of ion outside the membrane &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A or B]&amp;lt;sub&amp;gt;i&amp;lt;/sub&amp;gt; is the concentration of ion inside the membrane&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[[Nernst equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Goldman_eqn2.png&amp;diff=967</id>
		<title>File:Goldman eqn2.png</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Goldman_eqn2.png&amp;diff=967"/>
		<updated>2010-11-15T15:24:12Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Goldman_eqn1.png&amp;diff=965</id>
		<title>File:Goldman eqn1.png</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Goldman_eqn1.png&amp;diff=965"/>
		<updated>2010-11-15T15:23:58Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=963</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=963"/>
		<updated>2010-11-15T15:07:14Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential|Membrane potential]] &lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing study of frog skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
=== Goldman equation  ===&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Goldman equation]] &lt;br /&gt;
&lt;br /&gt;
In presence of more than one ion, the Nernst equation can be modified into Hodgkin-Katz-Goldman equation or is commonly known as Goldman equation. Goldman equation is proposed by David E. Goldman of Columbia University together with Alan L. Hodgkin and Bernard Katz. &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
*[[Membrane potential]]&amp;lt;br&amp;gt; &lt;br /&gt;
*[[Goldman equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=962</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=962"/>
		<updated>2010-11-15T15:06:11Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential|Membrane potential]] &lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing study of frog skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Goldman equation  ===&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Goldman equation]] &lt;br /&gt;
&lt;br /&gt;
In presence of more than one ion, the Nernst equation can be modified into Hodgkin-Katz-Goldman equation or is commonly known as Goldman equation. Goldman equation is proposed by David E. Goldman of Columbia University together with Alan L. Hodgkin and Bernard Katz. &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
*[[Membrane potential]]&amp;lt;br&amp;gt;&lt;br /&gt;
*[[Goldman equation]]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=961</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=961"/>
		<updated>2010-11-15T15:04:31Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential|Membrane potential]] &lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing study of frog skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Goldman equation  ===&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Goldman equation]] &lt;br /&gt;
&lt;br /&gt;
In presence of more than one ion, the Nernst equation can be modified into Hodgkin-Katz-Goldman equation or is commonly known as Goldman equation. Goldman equation is proposed by David E. Goldman of Columbia University together with Alan L. Hodgkin and Bernard Katz. &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=960</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=960"/>
		<updated>2010-11-15T15:03:35Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential]]&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Goldman Equation ===&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Goldman equation]]&lt;br /&gt;
&lt;br /&gt;
In presence of more than one ion, the Nernst equation can be modified into Hodgkin-Katz-Goldman equation or is commonly known as Goldman equation. Goldman equation is proposed by David E. Goldman of Columbia University together with Alan L. Hodgkin and Bernard Katz.&lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=959</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=959"/>
		<updated>2010-11-15T14:54:51Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article: &#039;&#039;[[Membrane Potential]]&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=957</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=957"/>
		<updated>2010-11-15T14:53:58Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=956</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=956"/>
		<updated>2010-11-15T14:52:21Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Blood Pressure]]&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Blood group systems]]&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems.]&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=955</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=955"/>
		<updated>2010-11-15T14:51:01Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;Main article:&#039;&#039; [[Blood Pressure]]&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems.]&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=953</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=953"/>
		<updated>2010-11-15T14:49:54Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems.]&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=952</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=952"/>
		<updated>2010-11-15T14:48:59Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm Table of blood group systems][http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm ].&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=951</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=951"/>
		<updated>2010-11-15T14:47:47Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion. &lt;br /&gt;
#Table of blood group systems.[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm]&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=950</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=950"/>
		<updated>2010-11-15T14:46:40Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=949</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=949"/>
		<updated>2010-11-15T14:44:09Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion[http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm &amp;lt;ref&amp;gt;Table of blood group systems&amp;lt;/ref&amp;gt;]. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=948</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=948"/>
		<updated>2010-11-15T14:42:17Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion&amp;lt;ref name=&amp;quot;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm&amp;quot;&amp;gt;Table of blood group systems&amp;lt;/ref&amp;gt;. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=946</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=946"/>
		<updated>2010-11-15T14:41:18Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems  ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion&amp;lt;ref name=&amp;quot;Table of blood group systems.&amp;quot;&amp;gt;http://ibgrl.blood.co.uk/isbt%20pages/isbt%20terminology%20pages/table%20of%20blood%20group%20systems.htm&amp;lt;/ref&amp;gt;. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=944</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=944"/>
		<updated>2010-11-15T14:38:34Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
== Composition&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
=== Plasma  ===&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Thrombocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]].&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Erythrocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== Leukocytes  ===&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Blood Pressure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Blood pressure is the pressure of the blood vessels exerted by circulating blood. It is normally measured at upper arm using a sphygmomanometer. During a heartbeat, there are two types of blood pressure is measured. One is &#039;upper&#039; systolic pressure (contraction) and another is &#039;lower&#039; diastolic (relaxation) pressure. Normal blood pressure for a healthy person is 120/80 mmHg (systolic/diastolic).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Blood Group Systems ==&lt;br /&gt;
&lt;br /&gt;
There are 30 blood groups systems recognised by International Society of Blood Transfusion&amp;lt;ref&amp;gt;Table of blood group systems.&amp;lt;/ref&amp;gt;. The major blood group systems are ABO Blood Group System and Rh Blood Group System.&lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.isbtweb.org/home/ ISBT]. International Society of Blood Transfusion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Protein&amp;diff=930</id>
		<title>Protein</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Protein&amp;diff=930"/>
		<updated>2010-11-15T14:19:18Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;A protein is a biological molecule which is made up of [[Amino acid|amino acids]].&amp;amp;nbsp; The [[Amino acids|amino acids]] join together with peptide bond to form a polypeptide chain. A protein can be made up of a single polypeptide chain or multiple [[Polypeptides|polypeptides]] linked together.&amp;amp;nbsp;Examples of proteins include [[Enzyme|enzymes]], [[Receptor|receptors]] and [[Hormone|hormones.]]&amp;amp;nbsp; They are found in every form of life from viruses to bacteria, yeasts to humans.&amp;amp;nbsp; &lt;br /&gt;
&lt;br /&gt;
== Structure&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
A protein has several &#039;layers&#039; of structure.&amp;amp;nbsp; &lt;br /&gt;
&lt;br /&gt;
=== Primary Structure ===&lt;br /&gt;
&lt;br /&gt;
The [[Primary structure|primary structure]] is the sequence of [[Amino acids|amino acids]].&amp;amp;nbsp; This is determined&amp;amp;nbsp;by the [[DNA|DNA]] sequence&amp;amp;nbsp;that encodes for&amp;amp;nbsp;that particular protein, called the [[Gene|gene]].&amp;amp;nbsp; &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
=== Secondary Structure&amp;lt;br&amp;gt; ===&lt;br /&gt;
&lt;br /&gt;
[[Secondary structure|Secondary structure]] is the first level of protein folding.&amp;amp;nbsp;A protein can fold in two different ways or not at all.&amp;amp;nbsp; It can either fold as an [[Alpha-helix|alpha-helix or]] a [[Beta-sheet|beta-sheet]]&amp;amp;nbsp;depending on the sequence of [[Amino acids|amino acids]].&amp;amp;nbsp; &amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
=== Tertiary Structure&amp;lt;br&amp;gt; ===&lt;br /&gt;
&lt;br /&gt;
[[Tertiary structure|Tertiary structure]] relates to the protein function.&amp;amp;nbsp; If the [[Tertiary structure|tertiary structure]] is wrong then the protein is unlikely to function properly.&amp;amp;nbsp; [[Tertiary structure|Tertiary structure]] is held together by either [[Hydrogen bonds|hydrogen bonds]] or [[Disulphide bridges|disulphide bridges]] depending o the [[Amino acids|amio acids]] present.&amp;amp;nbsp; Finally, if there are more than one peptide chains linked together to form a protein then you get a [[Quarternary structure|quarternary structure]].&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
=== Quarternary Structure&amp;lt;br&amp;gt; ===&lt;br /&gt;
&lt;br /&gt;
One or more tertiary stucture of protein build up a quarternary structure.&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== See also&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
*[http://bms.ncl.ac.uk/wiki/index.php/Amino_acids Amino acid]&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== References&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Renin-Angiotensin_System&amp;diff=922</id>
		<title>Renin-Angiotensin System</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Renin-Angiotensin_System&amp;diff=922"/>
		<updated>2010-11-15T13:56:14Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The Renin-Angiotensin system (RAS), also Renin-Angiotensin-Aldosterone system, is one of the mechanisms used by the body to regulate [[blood pressure|blood pressure]]. It comes into play when the [[blood pressure|blood pressure]] is too low, in disease it can&amp;amp;nbsp;happen when the [[blood pressure|blood pressure]] is not low&amp;amp;nbsp;which can lead to [[hypertension|hypertension]].&amp;amp;nbsp; &lt;br /&gt;
&lt;br /&gt;
== &amp;lt;u&amp;gt;&amp;lt;/u&amp;gt;Mechanism&amp;lt;u&amp;gt;&amp;lt;/u&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Low [[Blood pressure|blood pressure]] is detected by the juxtaglomerular apparatus&amp;amp;nbsp;which&amp;amp;nbsp;secretes&amp;amp;nbsp;renin. This&amp;amp;nbsp;[[Enzyme|enzyme]] hydrolyses&amp;amp;nbsp;angiotensinogen&amp;amp;nbsp;in the blood stream to [[Angiotensin I|angiotensin I]]. Angiotensin&amp;amp;nbsp;I is further processed; [[Angiotensin-converting-enzyme|angiotensin-converting-enzyme]] (ACE), released from the lungs, cleaves further [[Amino acids|amino acids]]&amp;amp;nbsp;from the protein resulting in [[Angiotensin II|angiotensin II]]. This [[Protein|protein]] help the body to raise the [[Blood pressure|blood pressure]] by many mechanisms including [[Vasoconstriction|vasoconstriction]], [[ADH|ADH]] secretion and [[Aldosterone|aldosterone]] secretion.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=921</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=921"/>
		<updated>2010-11-15T13:54:49Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Plasma ==&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Thrombocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]]. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Erythrocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Leukocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== References  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=920</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=920"/>
		<updated>2010-11-15T13:54:35Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Plasma ==&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Thrombocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]]. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Erythrocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Leukocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Reference  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=919</id>
		<title>Blood</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Blood&amp;diff=919"/>
		<updated>2010-11-15T13:54:02Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Blood is a major part of the human body. It is required for most functions of cells. Blood is comprised of 3 main sections: [[Plasma|Plasma]], [[Thrombocytes|Thrombocytes]], red blood cell ([[Erythrocytes|Erythrocytes]]), White Blood Cells&amp;amp;nbsp;([[Leukocytes|Leukocytes]]). &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Plasma ==&lt;br /&gt;
&lt;br /&gt;
[[Plasma|Plasma]] contains many molecules ranging from clotting factors, dissolved [[Proteins|proteins]] and even [[Carbon dioxide|carbon dioxide]] through respiration.&amp;amp;nbsp;Plasma is extremely important in the transport of metabolites&amp;amp;nbsp;such as ATP an&amp;amp;nbsp;glucose&amp;amp;nbsp;around the body.&amp;amp;nbsp;It also&amp;amp;nbsp;can contain waste&amp;amp;nbsp;molecules such&amp;amp;nbsp;as urea and lactic acid. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Thrombocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Thrombocytes|Thrombocytes]] are used in the clotting process and used to clog a broken seal with the aid of clotting factors via the [[Intrinsic Pathway|Intrinsic pathway]]. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Erythrocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Erythrocytes|Erythrocytes]] are used in gas exchange using the [[Proteins|protein]] [[Haemoglobin|Haemoglobin]] (Hb). The most distinct characteristic of the Erythrocytes is their unique biconcave shape. To be more specific, [[Erythrocytes|erythrocytes]] are flat and disc-shaped with indentations in the middle of both sides. This contribute to the ease of carrying and transporting [[Molecule|oxygen]] across the whole blood stream. [[Erythrocytes|Erythrocytes]] are also able to demonstrate their membrane flexibility by&amp;amp;nbsp; being able to squeeze through the very tiny and narrow blood capillaries&amp;lt;ref&amp;gt;Sherwood (2010) Human Physiology (From Cells to Systems), 7th edition, Canada : BROOKS/COLE CENGAGE Learning. page 392-4&amp;lt;/ref&amp;gt;. &amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Leukocytes ==&lt;br /&gt;
&lt;br /&gt;
[[Leukocytes|Leukocytes]] are used to defend the body against [[Pathogens|pathogens]] via [[Phagocytosis|phagocytosis]] or [[Antibody|antibody]] production.&amp;amp;nbsp;There are many leukocytes differing in their mechanisms and appearance&amp;amp;nbsp;(granular/agranular): l[[Lymphocyte|ymphocytes]], [[Monocyte|monocytes]], [[Basophil|basophils]] and&amp;amp;nbsp;[[Eosinophil|eosinophils]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
=== References:  ===&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=918</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=918"/>
		<updated>2010-11-15T13:09:50Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== External Links  ==&lt;br /&gt;
&lt;br /&gt;
#[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=894</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=894"/>
		<updated>2010-11-14T23:27:59Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;ref&amp;gt;http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst&amp;lt;/ref&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
== See also  ==&lt;br /&gt;
&lt;br /&gt;
== References &amp;amp;amp; Notes&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=893</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=893"/>
		<updated>2010-11-14T23:21:33Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]]&lt;br /&gt;
&lt;br /&gt;
== See also ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== References ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=892</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=892"/>
		<updated>2010-11-14T23:19:48Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]]&lt;br /&gt;
&lt;br /&gt;
== See also ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== References ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=891</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=891"/>
		<updated>2010-11-14T23:16:42Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Using Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]] &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== See also ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== References ==&lt;br /&gt;
&lt;br /&gt;
&amp;lt;references /&amp;gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=890</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=890"/>
		<updated>2010-11-14T23:13:36Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Using Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;ref&amp;gt;Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).&amp;lt;/ref&amp;gt;Ussing model of transepithelial ions absorption.&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=888</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=888"/>
		<updated>2010-11-14T23:10:06Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Using Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation4.png]]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=886</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=886"/>
		<updated>2010-11-14T23:05:58Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Using Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing_model.png|629x322px]]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst_equation4.png]]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=885</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=885"/>
		<updated>2010-11-14T23:02:14Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating [[Ion|ions]]. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;[[Kelvin|Kelvin]]&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the [[Faraday&#039;s constant|Faraday&#039;s constant]]; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]]&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt; &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion) &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane &lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane &lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Using Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber. &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Ussing_model.png|629x322px]]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
For example at the standard condition and temperature of 25&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C (298K), the above sodium ion membrane potential can be calculated as:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst_equation4.png]]&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Nernst_equation4.png&amp;diff=884</id>
		<title>File:Nernst equation4.png</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Nernst_equation4.png&amp;diff=884"/>
		<updated>2010-11-14T23:01:45Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Ussing_model.png&amp;diff=883</id>
		<title>File:Ussing model.png</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Ussing_model.png&amp;diff=883"/>
		<updated>2010-11-14T22:42:23Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=875</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=875"/>
		<updated>2010-11-14T21:48:30Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between cells (defined by the valency of ions)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of ion that gained electrons (reduction)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of ion that lost electrons (oxidation)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion)&lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Application  ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin  ===&lt;br /&gt;
&lt;br /&gt;
In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=874</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=874"/>
		<updated>2010-11-14T21:43:51Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between cells (defined by the valency of ions)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of ion that gained electrons (reduction)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of ion that lost electrons (oxidation)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|278x98px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|371x97px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;m&amp;lt;/sub&amp;gt; is the potential difference of an ion between membranes&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between membranes (defined by the valency of ion)&lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion outside the membrane&lt;br /&gt;
&lt;br /&gt;
[A&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;] is the concentration of ion inside the membrane&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== Application ==&lt;br /&gt;
&lt;br /&gt;
=== Ussing Study of Frog Skin ===&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=871</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=871"/>
		<updated>2010-11-14T21:38:08Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between cells (defined by the valency of ions)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of ion that gained electrons (reduction)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of ion that lost electrons (oxidation)&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt;  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation2.png|304x107px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
or &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation3.png|439x115px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=870</id>
		<title>Nernst Equation</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=Nernst_Equation&amp;diff=870"/>
		<updated>2010-11-14T21:37:05Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;= Nernst Equation&amp;lt;br&amp;gt;  =&lt;br /&gt;
&lt;br /&gt;
&#039;&#039;&#039;Nernst Equation&#039;&#039;&#039; is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
== Equation  ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation can be expressed as follows: &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst equation1.png|354x85px]] &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
where &lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt; &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the half-cell potential difference &lt;br /&gt;
&lt;br /&gt;
E&amp;lt;sup&amp;gt;θ&amp;lt;sub&amp;gt;&amp;lt;/sub&amp;gt;&amp;lt;/sup&amp;gt;&amp;lt;sub&amp;gt;cell &amp;lt;/sub&amp;gt;is the standard half-cell potential &lt;br /&gt;
&lt;br /&gt;
R is the universal gas constant; R = 8.314471 J K&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt; &lt;br /&gt;
&lt;br /&gt;
T is the thermodynamics temperature, in &#039;&#039;Kelvin&#039;&#039;; 0 K = -273.15&amp;lt;sup&amp;gt;o&amp;lt;/sup&amp;gt;C&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
z is the number of moles of electrons transferred between cells (defined by the valency of ions)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
F is the Faraday&#039;s constant; F = 96,485.3415 C mol&amp;lt;sup&amp;gt;-1&amp;lt;/sup&amp;gt;&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[red] is the concentration of ion that gained electrons (reduction)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[oxi] is the concentration of ion that lost electrons (oxidation)&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
== Membrane Potential&amp;lt;br&amp;gt; ==&lt;br /&gt;
&lt;br /&gt;
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:&amp;lt;br&amp;gt;&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst_equation2.png|304x107px]]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
or&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[Image:Nernst_equation3.png|439x115px]]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
where&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
	<entry>
		<id>https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Nernst_equation3.png&amp;diff=869</id>
		<title>File:Nernst equation3.png</title>
		<link rel="alternate" type="text/html" href="https://teaching.ncl.ac.uk/bms/wiki//index.php?title=File:Nernst_equation3.png&amp;diff=869"/>
		<updated>2010-11-14T21:35:57Z</updated>

		<summary type="html">&lt;p&gt;090012763: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;/div&gt;</summary>
		<author><name>090012763</name></author>
	</entry>
</feed>