What is [H^{+}] of a solution that is 0.01 M | vedclass

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(D) The solution is a buffer containing a weak acid $(HCN)$ and its salt $(NaCN)$.Using the acid dissociation constant expression: $K_a = \frac{[H^{+}

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$3.1 	imes 10^{-10}$

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(D) The solution is a buffer containing a weak acid $(HCN)$ and its salt $(NaCN)$.Using the acid dissociation constant expression: $K_a = \frac{[H^{+}][CN^{-}]}{[HCN]}$Given: $K_a = 6.2 	imes 10^{-10}$,$[HCN] = 0.01 \ M$,and $[CN^{-}] = 0.02 \ M$.Substituting the values: $6.2 	imes 10^{-10} = \frac{[H^{+}](0.02)}{0.01}$$[H^{+}] = \frac{6.2 	imes 10^{-10} 	imes 0.01}{0.02}$$[H^{+}] = 3.1 	imes 10^{-10} \ M$.

What is $[H^{+}]$ of a solution that is $0.01 \ M$ in $HCN$ and $0.02 \ M$ in $NaCN$ ($K_a$ for $HCN = 6.2 \times 10^{-10}$)?

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