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Why is chloroacetic acid stronger than acetic acid?

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oxidation of alcohols — carboxylic acid Alcohols may be oxidized to give aldehydes, ketones, and carboxylic acids. The oxidation of organic compounds generally increases the number of bonds from carbon to oxygen, and it may decrease the number of bonds to hydrogen.

Chloroacetic acid is stronger than acetic acid due to the inductive effect, which describes how substituents influence the distribution of electrons within a molecule.

In acetic acid ( $H — C H_{2} C O O H$ ), the methyl group is electron-donating, which destabilizes the resulting carboxylate ion. In contrast, chloroacetic acid ( $C l — C H_{2} C O O H$ ) contains a chlorine atom, which has a higher electronegativity than hydrogen. Because of this, the chlorine atom acts as an electron-withdrawing group, pulling electron density away from the carbon atom.

This electron-withdrawing effect stabilizes the negative charge of the carboxylate ion formed after the acid donates its proton. In general, electron-withdrawing groups increase the acidity of carboxylic acids by enhancing the stability of the conjugate base. Consequently, chloroacetic acid is approximately 100 times stronger than acetic acid.12