The solubility product of silver sulphide is | vedclass

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(A) The dissociation of silver sulphide is given by: $Ag_2S(s) \rightleftharpoons 2Ag^+(aq) + S^{2-}(aq)$.Let the solubility be $S \ mol/L$.Then,$[Ag^

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$2 	imes 10^{-4} \ mol/L$

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(A) The dissociation of silver sulphide is given by: $Ag_2S(s) ightleftharpoons 2Ag^+(aq) + S^{2-}(aq)$.Let the solubility be $S \ mol/L$.Then,$[Ag^+] = 2S$ and $[S^{2-}] = S$.The solubility product expression is $K_{sp} = [Ag^+]^2 [S^{2-}] = (2S)^2(S) = 4S^3$.Given $K_{sp} = 3.2 	imes 10^{-11}$.$4S^3 = 3.2 	imes 10^{-11}$.$S^3 = \frac{3.2 	imes 10^{-11}}{4} = 0.8 	imes 10^{-11} = 8 	imes 10^{-12}$.$S = \sqrt[3]{8 	imes 10^{-12}} = 2 	imes 10^{-4} \ mol/L$.

The solubility product of silver sulphide is $3.2 \times 10^{-11}$. Its solubility at the experimental temperature is

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