At 30,^{circ}C, the solubility of Ag_2CO_3 (K | vedclass

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(D) The solubility of a sparingly soluble salt like $Ag_2CO_3$ is affected by the presence of other ions in the solution.$(1)$ In $0.05\,M\,Na_2CO_3$

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$0.05\,M\,NH_3$

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(D) The solubility of a sparingly soluble salt like $Ag_2CO_3$ is affected by the presence of other ions in the solution.$(1)$ In $0.05\,M\,Na_2CO_3$ and $0.05\,M\,AgNO_3,$ the common ion effect ($CO_3^{2-}$ and $Ag^+$ respectively) significantly decreases the solubility of $Ag_2CO_3$.$(2)$ In pure water,the solubility is determined solely by its $K_{sp}$.$(3)$ In $0.05\,M\,NH_3,$ $Ag^+$ ions react with $NH_3$ to form a soluble complex $[Ag(NH_3)_2]^+$. This removes $Ag^+$ ions from the solution,shifting the equilibrium $Ag_2CO_3(s) \rightleftharpoons 2Ag^+(aq) + CO_3^{2-}(aq)$ to the right,thereby increasing the solubility of $Ag_2CO_3$ significantly compared to pure water.

At $30\,^{\circ}C,$ the solubility of $Ag_2CO_3$ $(K_{sp} = 8 \times 10^{-12})$ would be greatest in one litre of

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