The most acidic of the following is

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(A) The acidity of carboxylic acids depends on the stability of the conjugate base (carboxylate ion) formed after the loss of a proton.Electron-withdr

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$ClCH_2COOH$

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(A) The acidity of carboxylic acids depends on the stability of the conjugate base (carboxylate ion) formed after the loss of a proton.Electron-withdrawing groups ($-I$ effect) stabilize the carboxylate anion by dispersing the negative charge,thereby increasing the acidity of the parent acid.In $ClCH_2COOH$,the chlorine atom exerts a strong $-I$ effect,which significantly stabilizes the carboxylate ion.In $C_6H_5COOH$,the phenyl group has a weaker effect compared to the chlorine atom.In $CH_3CH_2COOH$ and $CD_3COOH$,the alkyl groups exert a $+I$ effect,which destabilizes the carboxylate ion and decreases acidity.Therefore,$ClCH_2COOH$ is the most acidic among the given options.

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Assertion $(A)$: Carboxylic acids are more acidic than Phenols.
Reason $(R)$: Resonance structures of carboxylate ion are equivalent,while resonance structures of phenoxide ion are not equivalent.

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