Question:
Which of the following is the strongest acid?
Which of the following is the strongest acid?
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The greater the electron-withdrawing effect, the stronger the acid due to better conjugate base stabilization.
Updated On: Feb 27, 2025
- \( p\)-Cl – \( C_6H_4\text{COOH} \)
- \( p\)-OH – \( C_6H_4\text{COOH} \)
- \( C_6H_5\text{COOH} \)
- \( p\)-NO\(_2\) – \( C_6H_4\text{COOH} \)
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The Correct Option is D
Solution and Explanation
The acidity of benzoic acid derivatives depends on the electron-withdrawing or electron-donating nature of the substituent at the para position:
- Electron-withdrawing groups (like \( NO_2 \)) increase acidity by stabilizing the conjugate base through delocalization.
- Electron-donating groups (like \( OH \) or \( CH_3 \)) decrease acidity by increasing electron density on the carboxyl group.
Since \( p\)-NO\(_2\) is a strong electron-withdrawing group, it stabilizes the conjugate base, making benzoic acid more acidic.
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