The most acidic carboxylic acid is

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(C) The acidity of carboxylic acids depends on the stability of the carboxylate anion formed after the loss of a proton. Electron-withdrawing groups i

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$HCOOH$

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(C) The acidity of carboxylic acids depends on the stability of the carboxylate anion formed after the loss of a proton. Electron-withdrawing groups increase acidity by stabilizing the negative charge,while electron-donating groups decrease acidity.$1$. $HCOOH$ (Formic acid): The $H$ atom has no inductive effect.$2$. $CH_3COOH$ (Acetic acid): The $CH_3$ group is electron-donating ($+I$ effect),which destabilizes the carboxylate anion,making it less acidic than formic acid.$3$. $C_6H_5COOH$ (Benzoic acid): The phenyl group is electron-withdrawing due to its $sp^2$ hybridized carbon atom ($-I$ effect),making it more acidic than acetic acid.$4$. $C_6H_5CH_2COOH$ (Phenylacetic acid): The $CH_2$ group separates the phenyl ring from the carboxyl group,reducing the electron-withdrawing effect of the phenyl ring compared to benzoic acid.Comparing the $pK_a$ values: $HCOOH$ $(pK_a \approx 3.75)$ > $C_6H_5COOH$ $(pK_a \approx 4.20)$ > $C_6H_5CH_2COOH$ $(pK_a \approx 4.31)$ > $CH_3COOH$ $(pK_a \approx 4.76)$.Therefore,$HCOOH$ is the most acidic among the given options.

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