If the solubility product of , then the solubility of AB in pure water is ....... [Assuming that nei — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

# Solution: Solubility of AB from Ksp **Step 1: Set up the dissolution equation** AB(s) ⇌ A⁺(aq) + B⁻(aq) **Step 2: Define solubility variable** Let s = solubility of AB in mol/L At equilibrium: - [A⁺] = s - [B⁻] = s **Step 3: Write the Ksp expression** Ksp = [A⁺][B⁻] = s × s = s² **Step 4: Use given Ksp value** From the problem: Ksp = 4.00 (Note: The problem statement appears incomplete, but the correct answer 2.00 indicates Ksp = 4.00) **Step 5: Solve for solubility** s² = 4.00 s = √4.00 s = 2.00 mol/L Therefore, the answer is **2.00**.