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Carboxylic acids are more acidic than phenol and alcohol because of
- a)intermolecular hydrogen bonding
- b)formation of dimers
- c)highly acidic hydrogen
- d)resonance stabilization of their conjugate base
Correct answer is option 'D'. Can you explain this answer?
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Carboxylic acids are more acidic than phenol and alcohol because ofa)i...
Resonance stabilization of the conjugate base:
Carboxylic acids are more acidic than phenols and alcohols because the carboxylate anion formed after deprotonation of the carboxylic acid can undergo resonance stabilization. The negative charge on the carboxylate ion can delocalize over two oxygen atoms, leading to the stabilization of the conjugate base.
Phenol and alcohol:
Phenol and alcohol do not show this resonance stabilization effect. In phenol, the negative charge is localized on the oxygen atom, whereas in alcohols, the negative charge is on the oxygen atom. This lack of resonance stabilization in phenol and alcohol makes them less acidic compared to carboxylic acids.
Electron-withdrawing effect:
The presence of the carbonyl group in carboxylic acids increases the acidity of the compound by withdrawing electron density from the O-H bond, making it easier to deprotonate. This electron-withdrawing effect further enhances the acidity of carboxylic acids compared to phenols and alcohols.
Conclusion:
In conclusion, the resonance stabilization of the conjugate base in carboxylic acids, along with the electron-withdrawing effect of the carbonyl group, makes carboxylic acids more acidic than phenols and alcohols.
Carboxylic acids are more acidic than phenols and alcohols because the carboxylate anion formed after deprotonation of the carboxylic acid can undergo resonance stabilization. The negative charge on the carboxylate ion can delocalize over two oxygen atoms, leading to the stabilization of the conjugate base.
Phenol and alcohol:
Phenol and alcohol do not show this resonance stabilization effect. In phenol, the negative charge is localized on the oxygen atom, whereas in alcohols, the negative charge is on the oxygen atom. This lack of resonance stabilization in phenol and alcohol makes them less acidic compared to carboxylic acids.
Electron-withdrawing effect:
The presence of the carbonyl group in carboxylic acids increases the acidity of the compound by withdrawing electron density from the O-H bond, making it easier to deprotonate. This electron-withdrawing effect further enhances the acidity of carboxylic acids compared to phenols and alcohols.
Conclusion:
In conclusion, the resonance stabilization of the conjugate base in carboxylic acids, along with the electron-withdrawing effect of the carbonyl group, makes carboxylic acids more acidic than phenols and alcohols.
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Carboxylic acids are more acidic than phenol and alcohol because ofa)intermolecular hydrogen bondingb)formation of dimersc)highly acidic hydrogend)resonance stabilization of their conjugate baseCorrect answer is option 'D'. Can you explain this answer?
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