How does complexation uniquely enhance the solubility of a sparingly soluble salt like AgCl in aqueo — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The dissolution $AgCl \rightleftharpoons Ag^+ + Cl^-$ ($K_{sp}$) couples with the complexation $Ag^+ + 2NH_3 \rightleftharpoons [Ag(NH_3)_2]^+$ ($K_f$). Adding these equations multiplies their constants, yielding a large $K_{eq} = K_{sp} \times K_f$ which drives dissolution forward.