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(D) The solubility of a sparingly soluble salt $Ag_2CO_3$ is affected by the common ion effect and complex formation. $1$. 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 $Ag_2CO_3$ is affected by the common ion effect and complex formation. $1$. In $0.05 \, M \, Na_2CO_3$,the common ion $CO_3^{2-}$ decreases the solubility. $2$. In $0.05 \, M \, AgNO_3$,the common ion $Ag^+$ decreases the solubility. $3$. In pure water,the solubility is determined by $K_{sp}$ alone. $4$. 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 significantly.

In which of the following solutions will the solubility of $Ag_2CO_3$ $(K_{sp} = 8 \times 10^{-12})$ be maximum at $30 \, ^\circ C$?

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