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A 0.10M solution of a certain monoprotic weak acid has a pH of 2.44. Calculate Ka.

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.............HA ==> H^+ + A^-
I...........0.1.....0.....0
C...........-x......x.....x
E.........0.1-x.....x.....x

The problem tells you pH = 2.44. Convert that to (H^+) by pH = -log(H^+) and substitute the x value in for (H^+) and (A^-). Evaluate 0.1-x and substitute that for (HA) in the Ka expression and evaluate Ka.
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