The pH of a buffer solution containing 25 mL | vedclass

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Question

(C) The $pH$ of a buffer solution is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.For the given buffer,$[Salt

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$5 \ M \ HCl$

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(C) The $pH$ of a buffer solution is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.For the given buffer,$[Salt] = [Acid] = 1 \ M$,so $pH = pK_a$.Adding a small amount of strong acid or base will change the ratio $\frac{[Salt]}{[Acid]}$,but the change is minimized by the buffer capacity.Option $C$ ($5 \ mL$ of $5 \ M \ HCl$) adds $25 \ mmol$ of $H^+$ ions,which is a significant amount compared to the $25 \ mmol$ of $CH_3COONa$ present,causing a drastic change in the $pH$ compared to the other options.Therefore,the $pH$ is most appreciably affected by $5 \ mL$ of $5 \ M \ HCl$.

The $pH$ of a buffer solution containing $25 \ mL$ of $1 \ M \ CH_3COONa$ and $25 \ mL$ of $1 \ M \ CH_3COOH$ will be appreciably affected by $5 \ mL$ of

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