Carboxylic acids are more acidic than phenols | vedclass

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(D) Step $1$: The acidity of a compound depends on the stability of its conjugate base.Step $2$: The conjugate base of a carboxylic acid is the carbox

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More resonance stabilization of their conjugate base

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(D) Step $1$: The acidity of a compound depends on the stability of its conjugate base.Step $2$: The conjugate base of a carboxylic acid is the carboxylate ion $(RCOO^-)$, where the negative charge is delocalized over two highly electronegative oxygen atoms.Step $3$: The conjugate base of a phenol is the phenoxide ion $(C_6H_5O^-)$, where the negative charge is delocalized over the carbon atoms of the benzene ring and one oxygen atom.Step $4$: Since oxygen is more electronegative than carbon, the negative charge is more effectively stabilized in the carboxylate ion than in the phenoxide ion. Therefore, carboxylic acids are more acidic.

Carboxylic acids are more acidic than phenols because:

Similar Questions

The $pK_a$ values of four carboxylic acids are $4.76, 4.19, 0.23$ and $3.41$ respectively. The $pK_a$ value of the strongest carboxylic acid among them is

Correct order of $pK_{a}$ of given compounds is $:-$
$(P) \ CH_{3}COOH$
$(Q) \ FCH_{2}COOH$
$(R) \ ClCH_{2}COOH$
$(S) \ C_{2}H_{5}COOH$

What are $X$ and $Y$ respectively in the following reaction sequence?
Styrene $\xrightarrow[(ii) H_3O^+]{(i) KMnO_4 / KOH} X$ $\xrightarrow{Br_2 / FeBr_3} Y$

Identify the reason for the highest boiling point of $R-COOH$ as compared to alkanes, ethers, alcohols and aldehydes.

The preferred reagent for the following conversion is $CH_3CH_2COOH \rightarrow CH_3CH_2COCl$.

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