Final answer:
The percent ionization of a 0.10M solution of acetic acid with a pH of 2.89 is 1.29%.
Step-by-step explanation:
To calculate the percent ionization of a 0.10M solution of acetic acid with a pH of 2.89, you must first determine the concentration of hydronium ions ([H3O+]) in the solution.
The pH is the negative logarithm of the hydronium ion concentration, so [H3O+] can be calculated using the equation:
[H3O+] = 10-pH
For a pH of 2.89:
[H3O+] = 10-2.89
= 1.29 x 10-3 M
This concentration [H3O+] is also the concentration of the acetic acid that ionized since they are in a 1:1 ratio. To find the percent ionization, divide the concentration of ionized acetic acid by the initial concentration and multiply by 100:
Percent ionization = ยก([H3O+] / Initial Concentration of Acetic Acid) x 100
Percent ionization = (1.29 x 10-3 M / 0.10 M) x 100
Percent ionization = 1.29%