The solubility products of NiS,ZnS,CdS,and Hg | vedclass

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(D) The precipitation of a metal sulphide $MS$ occurs when the ionic product $[M^{2+}][S^{2-}]$ exceeds the solubility product $K_{sp}$.Given that the

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$Hg^{2+}$,$Ni^{2+}$

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(D) The precipitation of a metal sulphide $MS$ occurs when the ionic product $[M^{2+}][S^{2-}]$ exceeds the solubility product $K_{sp}$.Given that the concentrations of all metal ions are equal,the ion with the lowest $K_{sp}$ will require the lowest concentration of $S^{2-}$ to exceed its $K_{sp}$ and precipitate first.Comparing the $K_{sp}$ values:$K_{sp}(HgS) = 4 	imes 10^{-53}$$K_{sp}(CdS) = 8 	imes 10^{-27}$$K_{sp}(ZnS) = 1.6 	imes 10^{-24}$$K_{sp}(NiS) = 4.7 	imes 10^{-5}$Since $HgS$ has the lowest $K_{sp}$,$Hg^{2+}$ will precipitate first.Since $NiS$ has the highest $K_{sp}$,$Ni^{2+}$ will precipitate last.Therefore,the first and last ions to precipitate are $Hg^{2+}$ and $Ni^{2+}$ respectively.

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