Calculate the [H+] of the following solutions from their pH. Then, calculate experimental Ka and Kb values using an ICE table.
A. Acetic acid - pH=3.02
B. Ammonuim hydroxide - pH=10.53
A. [H+] = 10-pH = 10-3.02 M = 9.55*10-4 M
The experimental Ka value = [H+][CH3COO-]/[CH3COOH]
i.e. Ka = 9.55*10-4 * 9.55*10-4/[CH3COOH]
Kb = 10-14/Ka
Note: [CH3COOH] should be given. If it is there, you can substitute and calculate accordingly.
B. [H+] = 10-10.53 M = 2.95*10-11 M
The experimental Kb value = [NH4+][OH-]/[NH4OH]
i.e. Ka = 2.95*10-11 * 2.95*10-11/[NH4OH]
Ka = 10-14/Kb
Note: [NH4OH] should be given. If it is there, you can substitute and calculate accordingly.
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