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(D) The solubility of $MnS$ in dilute $HCl$ is governed by the following equilibrium reaction:$MnS(s) + 2H^+(aq) \rightleftharpoons Mn^{2+}(aq) + H_2S

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The concentration of sulfide ions decreases due to the formation of the weak acid $H_2S$.

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(D) The solubility of $MnS$ in dilute $HCl$ is governed by the following equilibrium reaction:$MnS(s) + 2H^+(aq) \rightleftharpoons Mn^{2+}(aq) + H_2S(aq)$In this reaction,$H^+$ ions from $HCl$ react with $S^{2-}$ ions from $MnS$ to form the weak acid $H_2S$.According to Le Chatelier's principle,the removal of $S^{2-}$ ions from the solution to form $H_2S$ shifts the equilibrium to the right,thereby increasing the solubility of $MnS$ in the acidic medium.

Which of the following provides the best explanation for the solubility of $MnS$ in dilute $HCl$?

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