The hydrolysis of an ester is catalyzed by di | vedclass

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(B) The acid-catalyzed hydrolysis of an ester is a pseudo-first-order reaction where the rate of reaction is directly proportional to the concentratio

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Acid $A$ is a stronger acid than acid $B$.

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(B) The acid-catalyzed hydrolysis of an ester is a pseudo-first-order reaction where the rate of reaction is directly proportional to the concentration of $H^+$ ions.Since the reaction is catalyzed by $H^+$ ions,the rate constant $K$ is directly proportional to the concentration of $H^+$ ions produced by the acid.Therefore,$K \propto [H^+]$.Given $K_A > K_B$,it implies that $[H^+]_A > [H^+]_B$.Since a stronger acid dissociates more to provide a higher concentration of $H^+$ ions,acid $A$ must be a stronger acid than acid $B$.

Pressure $(mm \ Hg)$	$50, 100, 200$
Half-life period $(hrs)$	$3.52, 1.76, 0.88$

The hydrolysis of an ester is catalyzed by dilute acids $A$ and $B$. The rate constants for the two processes are $K_A$ and $K_B$ respectively. If $K_A > K_B$,which of the following statements is correct?

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