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

💡 Solution & Explanation

The dissolution $AgCl \rightleftharpoons Ag^+ + Cl^-$ ($K_{sp}$) couples with complexation $Ag^+ + 2NH_3 \rightleftharpoons [Ag(NH_3)_2]^+$ ($K_f$). The overall reaction adds both, so the equilibrium constants multiply: $K_{eq} = K_{sp} \times K_f$.