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(C) The acidity of a compound depends on the stability of its conjugate base. Electron-withdrawing groups $(EWG)$ increase acidity by stabilizing the

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$4-$acetylphenol and phenol

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(C) The acidity of a compound depends on the stability of its conjugate base. Electron-withdrawing groups $(EWG)$ increase acidity by stabilizing the conjugate base,while electron-donating groups $(EDG)$ decrease acidity by destabilizing it.$(A)$ $Br-CH_2-NO_2$ is more acidic than $CH_3-CH_3$ because the $NO_2$ group is a strong $EWG$.$(B)$ $CH_3-C(=O)-CH_2-CN$ is more acidic than $CH_3-C(=O)-CH_3$ because the $CN$ group is a strong $EWG$.$(C)$ $4-$acetylphenol is more acidic than phenol because the acetyl group $(-COCH_3)$ is an $EWG$ ($-I$ and $-M$ effect).$(D)$ p-cresol is less acidic than phenol because the methyl group $(-CH_3)$ is an $EDG$ ($+I$ and $+H$ effect).Since the question asks for the pair where the second compound is more acidic than the first,options $(A)$,$(B)$,and $(C)$ satisfy this condition. However,in standard multiple-choice formats,if only one answer is expected,$(C)$ is a classic example of substituent effects on phenol acidity.

Among the given pairs,in which pair is the second compound more acidic than the first?

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