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: Define solubility product expression** The $K_{sp}$ includes only the **aqueous ions** (not the solid), each raised to the power of its **stoichiometric coefficient**: $$K_{sp} = [Ag^+]^2[CrO_4^{2-}]$$ **Step 3: Verification** - From 1 mole of $Ag_2CrO_4$ dissolving: 2 moles of $Ag^+$ and 1 mole of $CrO_4^{2-}$ form - The exponent 2 on $[Ag^+]$ reflects this stoichiometry - The exponent 1 on $[CrO_4^{2-}]$ is implicit **Answer A is correct:** The solubility product constant is $K_{sp} = [Ag^+]^2[CrO_4^{2-}]$