The sulphide ion concentration [S^{2-}] in a | vedclass

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(B) Precipitation occurs when the ionic product $(Q_{sp})$ exceeds the solubility product $(K_{sp})$. In the presence of dilute $HCl$,the concentratio

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$III, IV$

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(B) Precipitation occurs when the ionic product $(Q_{sp})$ exceeds the solubility product $(K_{sp})$. In the presence of dilute $HCl$,the concentration of $S^{2-}$ ions is suppressed due to the common ion effect of $H^{+}$ ions. Given $[S^{2-}] = 1 	imes 10^{-22} \ M$. For a metal sulphide $(MS)$ to precipitate,the condition is $Q_{sp} > K_{sp}$,where $Q_{sp} = [M^{2+}][S^{2-}]$. Assuming a typical metal ion concentration of $0.1 \ M$,the ionic product $Q_{sp} = 0.1 	imes 10^{-22} = 10^{-23}$. Comparing the given $K_{sp}$ values: $I: 1.74 	imes 10^{-16} > 10^{-23}$ (No precipitation) $II: 1.2 	imes 10^{-22} > 10^{-23}$ (No precipitation) $III: 8.2 	imes 10^{-46} $IV: 5.0 	imes 10^{-34} Thus,sulphides $(III)$ and $(IV)$ will precipitate.

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

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