Read the Assertion and Reason below and choose the correct option. — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

When a saturated solution of a sparingly soluble salt like $\text{Sr(OH)}_2$ is diluted, more solid (if present) will dissolve to restore equilibrium, which actually increases the total moles of $\text{Sr}^{2+}$ in solution. Therefore, Statement I is false. The solubility product ($K_{sp}$) is an equilibrium constant that depends only on temperature and is independent of the volume or dilution of the solution. Therefore, Statement II is true.