The values of K_{sp} for CuS,Ag_2S and HgS ar | vedclass

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(D) The solubility $(S)$ of a salt depends on its $K_{sp}$ and stoichiometry.For $CuS$ ($AB$ type): $K_{sp} = S^2 \implies S = \sqrt{10^{-31}} \approx

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$Ag_2S > CuS > HgS$

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(D) The solubility $(S)$ of a salt depends on its $K_{sp}$ and stoichiometry.For $CuS$ ($AB$ type): $K_{sp} = S^2 \implies S = \sqrt{10^{-31}} \approx 3.16 	imes 10^{-16} \, mol/L$.For $Ag_2S$ ($A_2B$ type): $K_{sp} = 4S^3 \implies S = \sqrt[3]{\frac{10^{-42}}{4}} \approx 6.3 	imes 10^{-15} \, mol/L$.For $HgS$ ($AB$ type): $K_{sp} = S^2 \implies S = \sqrt{10^{-54}} = 10^{-27} \, mol/L$.Comparing the values: $6.3 	imes 10^{-15} > 3.16 	imes 10^{-16} > 10^{-27}$.Thus,the correct order is $Ag_2S > CuS > HgS$.

Product	Sulphide Solubility $(K_{sp})$
$I$	$1.74 \times 10^{-16}$
$II$	$1.2 \times 10^{-22}$
$III$	$8.2 \times 10^{-46}$
$IV$	$5.0 \times 10^{-34}$

The values of $K_{sp}$ for $CuS$,$Ag_2S$ and $HgS$ are $10^{-31}$,$10^{-42}$ and $10^{-54}$ respectively. The correct order of their solubility in water is

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