Question:
An acidified solution of $0.05 \,M\, Zn ^{2+}$ is saturated with $0.1 \,M \,H _{2} S$. What is the minimum molar concentration $(M)$ of $H ^{+}$required to prevent the precipitation of $ZnS$ ?
Use $K_{s p}( ZnS )=1.25 \times 10^{-22}$ and overall dissociation constant of $H _{2} S. K _{ NET }=K_{1} K_{2}=1 \times 10^{-21}$
An acidified solution of $0.05 \,M\, Zn ^{2+}$ is saturated with $0.1 \,M \,H _{2} S$. What is the minimum molar concentration $(M)$ of $H ^{+}$required to prevent the precipitation of $ZnS$ ?
Use $K_{s p}( ZnS )=1.25 \times 10^{-22}$ and overall dissociation constant of $H _{2} S. K _{ NET }=K_{1} K_{2}=1 \times 10^{-21}$
Use $K_{s p}( ZnS )=1.25 \times 10^{-22}$ and overall dissociation constant of $H _{2} S. K _{ NET }=K_{1} K_{2}=1 \times 10^{-21}$
Updated On: May 21, 2024
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Correct Answer: 0.2
Solution and Explanation
Molar concentration = 0.2
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