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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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wallace

  1. ...............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.

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    DrBob222

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