...............HA ==> H^+ + A^-
I...............0.1.........0.......0
C..............-x..........x........x
E...........0.1-x........x.........x
Ka = (H^+)(A^-)/(HA)
Plug in values for Ka and the E line for the others. Solve for (H^+) which is x, then pH = -log(H^+)
Post your work if you get stuck.
Find a pH of a 0.100 M solution of the weak acid HA. The pKa for the acid 5.0
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