What is the pH of an initially 0.428 M solution of a weak monoprotic acid that is 0.11 % ionized when equilibrium is established? (assume C_a/K_a ≥10²)

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Quizplus · Accepted Answer

The degree of ionization is given as 0.11%, which means that 0.11% of the initial concentration of the acid ionizes. To find the concentration of H+ ions, we calculate 0.11% of 0.428 M, which is 0.428 M * 0.0011 = 0.000471 M. The pH is then calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions. Plugging in the numbers, pH = -log(0.000471) ≈ 3.32.

What Is the PH of an Initially 0