The solubility product (K_sp; mol^3 dm^–9) of MX2 at 298 K based on the information available for th — Electrochemistry Chemistry Question

💡 Solution & Explanation

The Nernst equation for the cell is E_cell = (0.059/2) × log([M^2+]_cathode / [M^2+]_anode). Substituting values gives 0.059 = (0.059/2) × log(0.001 / [M^2+]_anode). Thus, log(0.001 / [M^2+]_anode) = 2, meaning 0.001 / [M^2+]_anode = 100. This yields [M^2+]_anode = 10^-5 M. The salt dissociates as MX2 <=> M^2+ + 2X^-, so [X^-] = 2 × [M^2+] = 2 × 10^-5 M. The solubility product Ksp = [M^2+][X^-]^2 = (10^-5) × (2 × 10^-5)^2 = 4 × 10^-15. Therefore, correct answer is B.