11.1 Acidity of Carboxylic Acids

Carboxylic acids are organic compounds that exhibit acidic properties, with a typical $p{K}_a$ value around 5. While acidic, they are considered weak acids when compared to strong mineral acids such as hydrochloric acid (HCl) or sulfuric acid ($H_{2}S{O}_4$).

A key principle is that a lower $p{K}_a$ value corresponds to a stronger acid.

Relative Strengths of Carboxylic Acids

The acidity of a carboxylic acid is significantly influenced by the nature of the substituent group attached to the carbon atom adjacent to the carboxyl group (-COOH).

The table below compares the $p{K}_a$ values of ethanoic acid with various substituted ethanoic acids.

Table 11.1: $p{K}_a$ Values of Various Organic Acids

Effect of Substituents on Acidity

1. Electron-Withdrawing Groups (EWGs)

An electron-withdrawing group (such as halogens or the nitro group) bonded to the carbon atom next to the carboxyl group increases the strength of the acid.

Mechanism: The EWG pulls electron density away from the carboxyl group. When the acid donates a proton ($H^{+}$) to form the carboxylate ion ($-CO{O}^{-}$), this electron-withdrawing effect helps disperse the negative charge over the ion.

Result: This stabilization of the conjugate base (the carboxylate ion) makes the proton less likely to re-bond, thus making the original acid stronger (it donates its proton more readily).

For example, the acidity order of chlorine-substituted ethanoic acids increases with the number of chlorine atoms:

${\text{CCl}}_3\text{COOH}>{\text{CHCl}}_2\text{COOH}>{\text{CH}}_2\text{ClCOOH}$

Chloroethanoic acid ($C{H}_{2}ClCOOH$) is approximately 100 times stronger than ethanoic acid ($C{H}_{3}COOH$).

2. Electron-Donating Groups (EDGs)

An electron-donating group (such as an alkyl group, e.g., $-C{H}_3$, $-C{H}_{2}C{H}_3$) bonded to the carboxyl group decreases the strength of the acid.

Mechanism: The EDG pushes electron density towards the carboxyl group. This intensifies the negative charge on the carboxylate ion after the proton has been donated.

Result: This destabilization of the conjugate base makes it more likely to attract and bond with an $H^{+}$ ion, thus making the original acid weaker.

For example, formic acid ($HCOOH$) is more acidic than acetic acid ($C{H}_{3}COOH$) because the methyl group ($-C{H}_3$) in acetic acid is electron-donating, which weakens the acid.

Comparison with Other Compounds

When comparing carboxylic acids to other organic compounds like phenols and alcohols, carboxylic acids are significantly more acidic. This is because the carboxylate ion is stabilized by resonance where the negative charge is delocalized over two electronegative oxygen atoms.

Possible Questions/Answers

Q: Why is trichloroethanoic acid ($CC{l}_{3}COOH$) a much stronger acid than ethanoic acid ($C{H}_{3}COOH$)?

A: Trichloroethanoic acid has three highly electronegative chlorine atoms, which are strong electron-withdrawing groups. They pull electron density away from the carboxylate ion, stabilizing the conjugate base and making the acid stronger. Ethanoic acid has an electron-donating methyl group, which destabilizes the conjugate base and makes the acid weaker.

Q: Arrange the following acids in order of increasing acidity: Propanoic acid, Chloroethanoic acid, Ethanoic acid.

A: Propanoic acid < Ethanoic acid < Chloroethanoic acid. (Based on their $p{K}_a$ values: 4.9, 4.7, and 2.9, respectively).

Significance: Understanding the acidity of carboxylic acids is crucial in organic synthesis, biochemistry (such as amino acids and fatty acids), and industrial processes where pH control is essential.