The concentration of and of a aqueous solution of a weak monoprotic acid that is ionized is (Assume — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The degree of ionization $\alpha = 2\% = 0.02$. The hydrogen ion concentration is $[H^+] = C\alpha = 0.1 \times 0.02 = 2 \times 10^{-3} \text{ M}$. The hydroxide ion concentration is obtained via the ionic product of water: $[OH^-] = \frac{K_w}{[H^+]} = \frac{10^{-14}}{2 \times 10^{-3}} = 5 \times 10^{-12} \text{ M}$.