Chloroacetic acid is a stronger acid than acetic acid. Give reason

Chloroacetic acid is indeed a stronger acid than acetic acid, and this can be attributed to the presence of chlorine atoms in its molecular structure.

Influence of Chlorine

The chlorine atom is highly electronegative, meaning it attracts electrons more strongly than many other atoms. When chlorine is attached to the acetic acid molecule, it pulls electron density away from the carboxylic acid group (-COOH).

Effect on Ionization

This electron-withdrawing effect stabilizes the negative charge that forms when the acid donates a proton (H⁺). As a result, chloroacetic acid more readily releases its proton compared to acetic acid, making it a stronger acid.

Comparison of Structures

• Acetic Acid: Contains a methyl group (-CH₃) that does not significantly stabilize the negative charge.
• Chloroacetic Acid: Contains a chlorine atom that enhances the stability of the ion formed after deprotonation.

In summary, the presence of chlorine in chloroacetic acid increases its acidity by stabilizing the ion formed when it loses a proton, making it a stronger acid than acetic acid.