Which is the correct representation of the solubility product constant of — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

# Solubility Product of $Ag_2CrO_4$ **Step 1: Write the dissolution equilibrium** $$Ag_2CrO_4(s) \rightleftharpoons 2Ag^+ + CrO_4^{2-}$$ **Step 2: Apply the solubility product expression** The $K_{sp}$ includes only dissolved ionic species (not the solid): $$K_{sp} = [Ag^+]^2[CrO_4^{2-}]$$ **Step 3: Why this is correct** - Each $Ag^+$ ion comes from stoichiometric coefficient 2 → exponent is 2 - Each $CrO_4^{2-}$ ion comes from coefficient 1 → exponent is 1 - Solids are excluded from equilibrium expressions (their activity = 1) **The correct answer is:** $K_{sp} = [Ag^+]^2[CrO_4^{2-}]$