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

💡 Solution & Explanation

# Solubility Product Constant 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 the concentrations of dissolved ions (not the solid). $$K_{sp} = [Ag^+]^2[CrO_4^{2-}]$$ **Step 3: Verify the stoichiometry** - The coefficient of $Ag^+$ is 2 → its concentration is raised to power 2 - The coefficient of $CrO_4^{2-}$ is 1 → its concentration is raised to power 1 **Why this is correct:** The $K_{sp}$ expression is the product of ion concentrations, each raised to a power equal to its stoichiometric coefficient in the balanced equation. For $Ag_2CrO_4$, we get $[Ag^+]^2[CrO_4^{2-}]$.