Which of the following is the strongest acid?

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Question

(A) The acidity of carboxylic acids is determined by the stability of the conjugate base (carboxylate ion). Electron-withdrawing groups $(EWG)$ stabil

Vedclass · Accepted Answer

$CF_3COOH$

Vedclass · Answer

(A) The acidity of carboxylic acids is determined by the stability of the conjugate base (carboxylate ion). Electron-withdrawing groups $(EWG)$ stabilize the carboxylate ion through the inductive effect ($-I$ effect),thereby increasing acidity. The strength of the $-I$ effect depends on the electronegativity of the substituent. Fluorine $(F)$ is more electronegative than Chlorine $(Cl)$ and Bromine $(Br)$. Therefore,the $-I$ effect follows the order: $CF_3 > CCl_3 > CBr_3 > CH_3$. Thus,$CF_3COOH$ is the strongest acid among the given options.

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