The solubility of AgCN in a buffer solution o | vedclass

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(B) The dissolution reaction is $AgCN_{(s)} + H^{+}_{(aq)} \rightleftharpoons Ag^{+}_{(aq)} + HCN_{(aq)}$.The equilibrium constant $K_{eq} = \frac{K_{

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$1.9 	imes 10^{-5}$

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(B) The dissolution reaction is $AgCN_{(s)} + H^{+}_{(aq)} ightleftharpoons Ag^{+}_{(aq)} + HCN_{(aq)}$.The equilibrium constant $K_{eq} = \frac{K_{sp}(AgCN)}{K_a(HCN)} = \frac{2.2 	imes 10^{-16}}{6.2 	imes 10^{-10}} \approx 3.55 	imes 10^{-7}$.Since $s = [Ag^{+}] = [HCN]$ and $[H^{+}] = 10^{-pH} = 10^{-3}$,we have $K_{eq} = \frac{s^2}{[H^{+}]}$.$s^2 = K_{eq} 	imes [H^{+}] = 3.55 	imes 10^{-7} 	imes 10^{-3} = 3.55 	imes 10^{-10}$.$s = \sqrt{3.55 	imes 10^{-10}} \approx 1.88 	imes 10^{-5} \approx 1.9 	imes 10^{-5}$.

The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$. The value of $x$ is [Assume : No cyano complex is formed; $K_{sp}(AgCN) = 2.2 \times 10^{-16}$ and $K_{a}(HCN) = 6.2 \times 10^{-10}$]

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