Asked by Lee
Enough of a monoprotic acid is dissolved in water to produce a 0.0169 M solution. The pH of the resulting solution is 2.68. Calculate the Ka for the acid.
Answers
Answered by
DrBob222
Convert pH 2.68 to (H^+) with
pH = -log(H^+).
Then HA --> H^+ + A^-
Ka = (H^+)(A^-)/(HA)
Substitute for (H^+) and (A^-). For (HA) substitute 0.0169-(H^+)
pH = -log(H^+).
Then HA --> H^+ + A^-
Ka = (H^+)(A^-)/(HA)
Substitute for (H^+) and (A^-). For (HA) substitute 0.0169-(H^+)
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