Two salts AX and BX have the same value of solubility product of 4.0 × 10 . The ratio of their molar — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

**Step 1: Identify the salt types and their dissolution equations** - Salt AX is a 1:1 salt (e.g., AgCl): AX ⇌ A⁺ + X⁻ - Salt BX is a 1:2 salt (e.g., CaF₂): BX ⇌ B²⁺ + 2X⁻ **Step 2: Write the Ksp expressions** - For AX: Ksp = [A⁺][X⁻] = s₁ × s₁ = s₁² - For BX: Ksp = [B²⁺][X⁻]² = s₂ × (2s₂)² = 4s₂³ **Step 3: Set up equations using Ksp = 4.0 × 10⁻¹²** - For AX: s₁² = 4.0 × 10⁻¹² - For BX: 4s₂³ = 4.0 × 10⁻¹² **Step 4: Solve for molar solubilities** - s₁ = √(4.0 × 10⁻¹²) = 2.0 × 10⁻⁶ M - s₂³ = 1.0 × 10⁻¹² - s₂ = ∛(1.0 × 10⁻¹²) = 1.0 × 10⁻⁴ M **Step 5: Calculate the ratio** Ratio = s₁/s₂ = (2.0 × 10⁻⁶)/(1.0 × 10⁻⁴) = 0.02 = 1/50 **Step 6: Express as requested** Since the question asks for the ratio of their molar solubilities, the answer is s₂/s₁ = 50. Therefore, the answer is 50.00.