The solubility of is ‘s’ moles/litre. Then its solubility product is........ — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

# Solubility Product of $CaF_2$ ## Step 1: Write the dissolution equilibrium $$CaF_2(s) \rightleftharpoons Ca^{2+}(aq) + 2F^-(aq)$$ ## Step 2: Express ion concentrations in terms of solubility 's' If solubility = $s$ mol/L, then at equilibrium: - $[Ca^{2+}] = s$ moles/L - $[F^-] = 2s$ moles/L (For every 1 mole of $CaF_2$ dissolved, 2 moles of $F^-$ are produced) ## Step 3: Apply solubility product expression $$K_{sp} = [Ca^{2+}][F^-]^2$$ $$K_{sp} = (s)(2s)^2$$ $$K_{sp} = s \cdot 4s^2$$ $$\boxed{K_{sp} = 4s^3}$$ **Answer B is correct:** The solubility product of $CaF_2$ is **$4s^3$**