An acidified solution of $0.05 M Z n^{2 +}$ is saturated with 0.1 $M H_{2} S$ . What is the minimum molar concentration $(M)$ of $H^{+}$ required to prevent the precipitation of $Z n S$ ? Use $K_{s p} (Z n S) = 1.25 \times 10^{- 22}$ and Overall dissociation constant of $H_{2} S, K_{N E T} = K_{1} K_{2} = 1 \times 10^{- 21}$

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Detailed Solution

For ppt. $[Z n^{2 +}] [S^{2 -}] = K_{s p}$

$[S^{2 -}] = \frac{1.25 \times 10^{- 22}}{0.05} = 2.5 \times 10^{- 21} M$

$H_{2} S \underset{}{⇌} 2 H^{+} + S^{2 -}$

$K_{n e t} = 10^{- 21} = \frac{{[H^{+}]}^{2} \times 2.5 \times 10^{- 21}}{0.1}$

${[H^{+}]}^{2} = \frac{1}{25}$

$[H^{+}] = \frac{1}{5} M = 0.2 M$

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