Calculating Ka given pH
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Calculating Ka given pH

[From: ] [author: ] [Date: 11-11-07] [Hit: ]
[H+] equals 10^(-pH).10^-9.6 = [H+] = 2.Ka = (2.5188643x10^-10)^2 / .35 = 1.......
A 0.350 M solution of the salt NaA has pH=9.60. Calculate Ka for the acid HA

Could someone explain how to do this please?

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9.6 = -log[H+]. [H+] equals 10^(-pH).

10^-9.6 = [H+] = 2.51188643x10^-10

Weak acids dissociate into equal amounts of H+ and their conjugate base

Ka = (2.5188643x10^-10)^2 / .35 = 1.8x10^-19
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