Question

The pka of acetic acid is 4.74. Calculate the average percent error and mean absolute deviation of your pka data.

Answer 1

The percent ionization of a 0.10-M solution of acetic acid with a pH of 2.89 is calculated to be 1.29%.

Step-by-step explanation:

To calculate the percent ionization of a 0.10-M solution of acetic acid with a pH of 2.89, we need to understand the relationship between the pH, pKa, and the concentration of acetic acid and its ionized form.

Firstly, calculate the concentration of H+ ions using the pH:

[H+] = 10-pH = 10-2.89 = 1.29 x 10-3M

Since acetic acid (CH3COOH) ionizes as follows:

CH3COOH → H+ + CH3COO-

We can assume that the concentration of H+ ions produced is equal to the concentration of CH3COO- ions. Therefore, the percent ionization is calculated by the formula:

Percent ionization = ([H+] / initial concentration of acetic acid) x 100%

Percent ionization = (1.29 x 10-3 / 0.10) x 100% = 1.29%