Consider the fundamental relationship between the ionic product () and the solubility product (). Wh — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

$Q_{sp}$ operates like a reaction quotient. When $Q_{sp} < K_{sp}$, the system has not reached equilibrium and can dissolve more salt. When $Q_{sp} = K_{sp}$, it is saturated. When $Q_{sp} > K_{sp}$, the ion concentrations exceed equilibrium capacity, driving the reverse reaction (precipitation). Statement D is false because $Q_{sp}$ changes wildly with current ion concentrations, whereas $K_{sp}$ is the strict temperature-dependent constant.