For pure water at , which of the following relations and values hold true? — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The density of water is $1 \text{ g/mL}$, giving a molarity of $1000/18 = 55.55 \text{ M}$. At $25^\circ C$, $K_w = 10^{-14}$. The degree of ionization $\alpha = [H^+]/[H_2O] = 10^{-7}/55.55 = 1.8 \times 10^{-9}$. The dissociation constant $K_d = K_w / [H_2O] = 10^{-14} / 55.55 = 1.8 \times 10^{-16}$. All statements are correct.