(A) For $CuS$ ($1:1$ type salt): $K_{sp} = s^2 \implies s = \sqrt{K_{sp}} = \sqrt{10^{-31}} = 10^{-15.5}$.For $Ag_2S$ ($2:1$ type salt): $K_{sp} = 4s^

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(A) For $CuS$ ($1:1$ type salt): $K_{sp} = s^2 \implies s = \sqrt{K_{sp}} = \sqrt{10^{-31}} = 10^{-15.5}$.For $Ag_2S$ ($2:1$ type salt): $K_{sp} = 4s^3 \implies s = (K_{sp}/4)^{1/3} = (10^{-44}/4)^{1/3} \approx 0.63 \times 10^{-14.6} \approx 10^{-15.2}$.For $HgS$ ($1:1$ type salt): $K_{sp} = s^2 \implies s = \sqrt{K_{sp}} = \sqrt{10^{-54}} = 10^{-27}$.Comparing the values: $10^{-15.2} > 10^{-15.5} > 10^{-27}$.Therefore,the order of solubility is $Ag_2S > CuS > HgS$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Solubility product

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The solubility product $(K_{sp})$ values of $CuS$,$Ag_2S$,and $HgS$ are $10^{-31}$,$10^{-44}$,and $10^{-54}$ respectively. The solubilities of these sulphides are in the order:

AIPMT 1997 All AIPMT

A
$Ag_2S > CuS > HgS$
B
$Ag_2S > HgS > CuS$
C
$HgS > Ag_2S > CuS$
D
$CuS > Ag_2S > HgS$

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6-2.Equilibrium-II (Ionic Equilibrium)

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The solubility product $(K_{sp})$ values of $CuS$,$Ag_2S$,and $HgS$ are $10^{-31}$,$10^{-44}$,and $10^{-54}$ respectively. The solubilities of these sulphides are in the order:

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