The pH of a 0.14 M solution of an unknown monoprotic acid is 5.85. Calculate the Ka of the acid.
HA <------------> H+ + A-
pH = 5.85
[H+] = 10-pH = 10-5.85 = 1.41 x 10-6
[A-] = 1.41 x 10-6
[HA] = 0.14 - 1.41 x 10-6 = 0.139998
Ka = [H+] [A-] / [HA]
Ka = [1.41 x 10-6] [1.41 x 10-6] / [0.139998]
Ka = 1.42 x 10-11
The pH of a 0.14 M solution of an unknown monoprotic acid is 5.85. Calculate the...
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