Carboxyllic acid: Difference between revisions

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&nbsp;Carboxylic acids are organic compounds which contain a carboxyl group (COOH)<ref name="1">Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref><span style="font-size: 13.28px;">.&nbsp;</span>  
&nbsp;Carboxylic acids are organic compounds which contain a carboxyl group (COOH)<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref><span style="font-size: 13.28px;">.&nbsp;</span>  


=== '''<u></u>'''<u>'''Naming'''</u>  ===
=== '''<u></u>'''<u>'''Naming'''</u>  ===


You always name carboxylic acids from the first carbon atom on the COOH group. This carbon atom is always counted as carbon number 1 regardless of how many other side chains there are on the compoun<span style="font-size: 13.28px;">d<ref name="1">Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref></span><span style="font-size: 13.28px;">.</span>  
You always name carboxylic acids from the first carbon atom on the COOH group. This carbon atom is always counted as carbon number 1 regardless of how many other side chains there are on the compoun<span style="font-size: 13.28px;">d<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref></span><span style="font-size: 13.28px;">.</span>  


=== <u>'''Examples of Carboxylic acids'''</u>  ===
=== <u>'''Examples of Carboxylic acids'''</u>  ===


The shortest carboxylic acid is methanoic acid and its chemical formula is CH3COOH. Other examples include ethanoic acid, 2 methyl butanoic acid etc<ref name="1">Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>.  
The shortest carboxylic acid is [[methanoic acid|methanoic acid]] and its chemical formula is CH3COOH<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>. Other examples include ethanoic acid, 2 methyl butanoic acid etc<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>.  


=== <u>'''Formation'''</u>  ===
=== <u>'''Formation'''</u>  ===


Primary alcohols can be oxidised through heating under reflux with potassium dichromate solution to produce carboxylic acids<ref name="2">LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids</ref>. Other ways of producing carboxylic acids include hydrolysing nitriles through acid or alkali hydrolysis<ref name="2">LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids</ref>.  
Primary alcohols can be [[oxidised|oxidised]] through heating under reflux with potassium dichromate solution to produce carboxylic acids<ref>LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids</ref>. Other ways of producing carboxylic acids include [[hydrolysing|hydrolysing]] nitriles through acid or alkali hydrolysis<ref>LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids</ref>.  


=== <u>'''Physical properties'''</u>  ===
=== <u>'''Physical properties'''</u>  ===


Carboxylic acids have slightly higher boiling points than alcohols due to stronger hydrogen bonding<ref name="1">Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>.  
Carboxylic acids have slightly higher boiling points than [[Alcohol|alcohols]] due to stronger[[hydrogen bonding|hydrogen bonding<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>]].  


Smaller chain carboxylic acids are relatively soluble in water. However the bigger acids tend to be less soluble due to the hydrocarbon tails breaking hydrogen bonds between water molecules and the carboxylic acid<ref name="1">Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>.  
Smaller chain carboxylic acids are relatively soluble in water. However the bigger acids tend to be less soluble due to the hydrocarbon tails breaking hydrogen bonds between water molecules and the carboxylic acid<ref>Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html</ref>.  


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= '''References'''<br>  =
= '''References'''<br>  =


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Revision as of 21:37, 3 December 2017

 Carboxylic acids are organic compounds which contain a carboxyl group (COOH)[1]. 

Naming

You always name carboxylic acids from the first carbon atom on the COOH group. This carbon atom is always counted as carbon number 1 regardless of how many other side chains there are on the compound[2].

Examples of Carboxylic acids

The shortest carboxylic acid is methanoic acid and its chemical formula is CH3COOH[3]. Other examples include ethanoic acid, 2 methyl butanoic acid etc[4].

Formation

Primary alcohols can be oxidised through heating under reflux with potassium dichromate solution to produce carboxylic acids[5]. Other ways of producing carboxylic acids include hydrolysing nitriles through acid or alkali hydrolysis[6].

Physical properties

Carboxylic acids have slightly higher boiling points than alcohols due to strongerhydrogen bonding[7].

Smaller chain carboxylic acids are relatively soluble in water. However the bigger acids tend to be less soluble due to the hydrocarbon tails breaking hydrogen bonds between water molecules and the carboxylic acid[8].


References

  1. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html
  2. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html
  3. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html
  4. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html
  5. ↑ LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids
  6. ↑ LibreTexts. Preparation of Carboxylic Acids. 2015. [cited 03/12/17]. Available from: https://chem.libretexts.org/Core/Organic_Chemistry/Carboxylic_Acids/Synthesis_of_Carboxylic_Acids/Preparation_of_carboxylic_acids
  7. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html
  8. ↑ Jim Clark. Introducing Carboxylic Acids. 2004. [cited 03/12/17]. Available from: https://www.chemguide.co.uk/organicprops/acids/background.html



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