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OpenStudy (anonymous):
If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.16 M solution of this acid?
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OpenStudy (cuanchi):
pH=-log[H+] [H+] for a weak acid assuming that the percentage of ionization is less than 5% can be calculated with the following formula \[[H+]=\sqrt{Ka \times Ca}\] where Ca is the initial concentration of the acid
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