Components of a buffer solution are 0.1 M H | vedclass

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Question

(A) The $pH$ of an acidic buffer is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log \left( \frac{[Salt]}{[Acid]} \right)$ Given

Vedclass · Accepted Answer

$9.60$

Vedclass · Answer

(A) The $pH$ of an acidic buffer is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log \left( \frac{[Salt]}{[Acid]} \right)$ Given: $[Acid] = [HCN] = 0.1 \ M$ $[Salt] = [NaCN] = 0.2 \ M$ $pK_a = 9.30$ Substituting the values: $pH = 9.30 + \log \left( \frac{0.2}{0.1} \right)$ $pH = 9.30 + \log(2)$ Since $\log(2) \approx 0.3010$: $pH = 9.30 + 0.3010 = 9.6010 \approx 9.60$ Therefore,the correct option is $A$.

Components of a buffer solution are $0.1 \ M \ HCN$ and $0.2 \ M \ NaCN$. What is the $pH$ of the solution? (Given: $pK_a$ of $HCN = 9.30$)

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