If you had an acetic acid solution that was 0.10 M, what would the acetate concentration have to be in order to get a pH of 5.35? Show your calculations
The pH of a solution is determined by the concentration of hydrogen ions (H+) in the solution. The concentration of H+ in a 0.10 M acetic acid solution can be calculated using the following equation:
[H+] = 10^(-pH)
[H+] = 10^(-5.35)
[H+] = 3.16 x 10^-6 M
The concentration of acetate ions (CH3COO-) can be calculated using the following equation:
[CH3COO-] = [H+] / Ka
Where Ka is the acid dissociation constant for acetic acid, which is 1.8 x 10^-5.
[CH3COO-] = 3.16 x 10^-6 / 1.8 x 10^-5
[CH3COO-] = 1.76 x 10^-1 M
Therefore, the acetate concentration must be 1.76 x 10^-1 M in order to get a pH of 5.35.