The pKa value of acetic acid is 4.76. To calculate the pH of a 0.1 M solution of acetic acid, we can use the Henderson-Hasselbalch equation:pH = pKa + log [A-]/[HA] In this case, [HA] is the concentration of acetic acid 0.1 M , and [A-] is the concentration of acetate ions. Since we don't know the concentration of acetate ions, we can use the ionization constant Ka of acetic acid to find it. The Ka of acetic acid is 10^-pKa = 10^-4.76 1.74 x 10^-5 .Let x be the concentration of acetate ions [A-] and acetic acid that ionizes. Then, the ionization equation is:Ka = x x / 0.1 - x 1.74 x 10^-5 = x^2 / 0.1 - x Solving for x, we get x 1.33 x 10^-3 M. This is the concentration of acetate ions and the amount of acetic acid that ionizes.Now we can use the Henderson-Hasselbalch equation:pH = 4.76 + log 1.33 x 10^-3 / 0.1 - 1.33 x 10^-3 pH 2.87The pH of the 0.1 M solution of acetic acid is approximately 2.87.To find the percent ionization of acetic acid in this solution, we can use the following formula:Percent ionization = concentration of ionized acetic acid / initial concentration of acetic acid x 100Percent ionization = 1.33 x 10^-3 / 0.1 x 100 1.33%The percent ionization of acetic acid in this 0.1 M solution is approximately 1.33%.