# Nernst Equation

(3 intermediate revisions by 2 users not shown) | |||

Line 1: | Line 1: | ||

− | '''Nernst Equation''' 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).<ref>http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst</ref><br> | + | '''Nernst Equation''' 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|Walther H. Nernst]] (1864-1941).<ref>http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst</ref><br> |

== Equation == | == Equation == | ||

Line 5: | Line 5: | ||

Nernst equation can be expressed as follows: | Nernst equation can be expressed as follows: | ||

− | [[Image:Nernst equation1.png|354x85px]]<br> | + | [[Image:Nernst equation1.png|354x85px|Nernst equation1.png]]<br> |

− | where<br> | + | where<br> |

E<sub>cell </sub>is the half-cell potential difference | E<sub>cell </sub>is the half-cell potential difference | ||

Line 15: | Line 15: | ||

R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K<sup>-1</sup> mol<sup>-1</sup> | R is the [[Universal gas constant|universal gas constant]]; R = 8.314471 J K<sup>-1</sup> mol<sup>-1</sup> | ||

− | T is the thermodynamics temperature, in ''[[Kelvin|Kelvin]]''; 0 K = -273.15<sup>o</sup>C<br> | + | T is the thermodynamics temperature, in ''[[Kelvin|Kelvin]]''; 0 K = -273.15<sup>o</sup>C<br> |

− | z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])<br> | + | z is the number of [[Moles|moles]] of [[Electrons|electrons]] transferred between cells (defined by the valency of [[Ion|ions]])<br> |

− | F is the [[Faraday's constant|Faraday's constant]]; F = 96,485.3415 C mol<sup>-1</sup><br> | + | F is the [[Faraday's constant|Faraday's constant]]; F = 96,485.3415 C mol<sup>-1</sup><br> |

− | [red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])<br> | + | [red] is the concentration of [[Ion|ion]] that gained [[Electrons|electrons]] ([[Reduction|reduction]])<br> |

− | [oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])<br> | + | [oxi] is the concentration of [[Ion|ion]] that lost [[Electrons|electrons]] ([[Oxidation|oxidation]])<br> |

− | == Membrane potential<br> | + | == Membrane potential<br> == |

''Main article: ''[[Membrane Potential|Membrane potential]] | ''Main article: ''[[Membrane Potential|Membrane potential]] | ||

− | 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:<br> | + | 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:<br> |

− | [[Image:Nernst equation2.png|278x98px]]<br> | + | [[Image:Nernst equation2.png|278x98px|Nernst equation2.png]]<br> |

− | or<br> | + | or<br> |

− | [[Image:Nernst equation3.png|371x97px]]<br> | + | [[Image:Nernst equation3.png|371x97px|Nernst equation3.png]]<br> |

− | where<br> | + | where<br> |

E<sub>m</sub> is the potential difference of an ion between membranes<sub></sub> | E<sub>m</sub> is the potential difference of an ion between membranes<sub></sub> | ||

Line 49: | Line 49: | ||

F is the Faraday's constant; F = 96,485.3415 C mol<sup>-1</sup> | F is the Faraday's constant; F = 96,485.3415 C mol<sup>-1</sup> | ||

− | [A<sup>-</sup>]<sub>o</sub> is the concentration of ion outside the membrane (in this case is anion, negative charge ion)<br> | + | [A<sup>-</sup>]<sub>o</sub> is the concentration of ion outside the membrane (in this case is anion, negative charge ion)<br> |

− | [A<sup>-</sup>]<sub>i</sub> is the concentration of ion inside the membrane (in this case is anion, negative charge ion) | + | [A<sup>-</sup>]<sub>i</sub> is the concentration of ion inside the membrane (in this case is anion, negative charge ion) |

== Application == | == Application == | ||

− | === | + | === Using study of frog skin === |

− | 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.<br> | + | 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.<br> |

[[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] | [[Image:Ussing model.png|629x322px|Ussing model of transepithelial ions absorption.]] | ||

− | <ref>Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).</ref> | + | Using model of transepithelial ions absorption <ref>Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).</ref>.<br> |

− | For example at the standard condition and temperature of 25<sup>o</sup>C (298K), the above sodium ion membrane potential can be calculated as:<br> | + | For example at the standard condition and temperature of 25<sup>o</sup>C (298K), the above sodium ion membrane potential can be calculated as:<br> |

[[Image:Nernst equation4.png]] | [[Image:Nernst equation4.png]] | ||

Line 71: | Line 71: | ||

''Main article:'' [[Goldman equation]] | ''Main article:'' [[Goldman equation]] | ||

− | 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. | + | 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. It is used to determine the equilibrium potential across a cell's membrane using all of the ions taht can cross the membrane. The Hodgkin-Katz-Goldman equation is essentially a combined Nernst equation, taking into account the permeability's of the many ions present in real cells. |

== See also == | == See also == | ||

− | *[[Membrane potential]]<br> | + | *[[Membrane potential]]<br> |

*[[Goldman equation]]<br> | *[[Goldman equation]]<br> | ||

− | == References & Notes<br> | + | == References & Notes<br> == |

− | <references /><br> | + | <references /><br> |

== External Links == | == External Links == | ||

*[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator] | *[http://www.nernstgoldman.physiology.arizona.edu/ The Nernst/Goldman Equation Simulator] |

## Latest revision as of 14:30, 18 November 2016

**Nernst Equation** 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).^{[1]}

## Contents |

## Equation

Nernst equation can be expressed as follows:

where

E_{cell }is the half-cell potential difference

E^{θ}_{cell }is the standard half-cell potential

R is the universal gas constant; R = 8.314471 J K^{-1} mol^{-1}

T is the thermodynamics temperature, in *Kelvin*; 0 K = -273.15^{o}C

z is the number of moles of electrons transferred between cells (defined by the valency of ions)

F is the Faraday's constant; F = 96,485.3415 C mol^{-1}

[red] is the concentration of ion that gained electrons (reduction)

[oxi] is the concentration of ion that lost electrons (oxidation)

## Membrane potential

*Main article: *Membrane potential

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:

or

where

E_{m} is the potential difference of an ion between membranes_{}

R is the universal gas constant; R = 8.314471 J mol^{-1}

T is the thermodynamics temperature, in *Kelvin*; 0 K = -273.15^{o}C

z is the number of moles of electrons transferred between membranes (defined by the valency of ion)

F is the Faraday's constant; F = 96,485.3415 C mol^{-1}

[A^{-}]_{o} is the concentration of ion outside the membrane (in this case is anion, negative charge ion)

[A^{-}]_{i} is the concentration of ion inside the membrane (in this case is anion, negative charge ion)

## Application

### Using study of frog skin

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.

Using model of transepithelial ions absorption ^{[2]}.

For example at the standard condition and temperature of 25^{o}C (298K), the above sodium ion membrane potential can be calculated as:

### Goldman equation

*Main article:* Goldman equation

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. It is used to determine the equilibrium potential across a cell's membrane using all of the ions taht can cross the membrane. The Hodgkin-Katz-Goldman equation is essentially a combined Nernst equation, taking into account the permeability's of the many ions present in real cells.

## See also

## References & Notes

- ↑ http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst
- ↑ Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).