Calculate [H^{+}] of 0.2 M HCN in 1 M KCN s | vedclass

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Question

(A) The given solution is a buffer solution consisting of a weak acid $(HCN)$ and its salt with a strong base $(KCN)$.For an acidic buffer,the concent

Vedclass · Accepted Answer

$8 	imes 10^{-11} \ M$

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(A) The given solution is a buffer solution consisting of a weak acid $(HCN)$ and its salt with a strong base $(KCN)$.For an acidic buffer,the concentration of hydrogen ions is given by the Henderson-Hasselbalch equation:$[H^{+}] = K_{a} 	imes \frac{[Acid]}{[Salt]}$Given:$K_{a} = 4 	imes 10^{-10}$$[Acid] = [HCN] = 0.2 \ M$$[Salt] = [KCN] = 1 \ M$Substituting the values:$[H^{+}] = 4 	imes 10^{-10} 	imes \frac{0.2}{1}$$[H^{+}] = 4 	imes 10^{-10} 	imes 0.2 = 0.8 	imes 10^{-10} = 8 	imes 10^{-11} \ M$

Calculate $[H^{+}]$ of $0.2 \ M$ $HCN$ in $1 \ M$ $KCN$ solution. Given $K_{a(HCN)} = 4 \times 10^{-10}$.

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