Chemistry pH

A 0.60 M solution of a weak acid, HA, has a pH of 3.72. What is the percentage ionization of the acid? What is the value of Ka for the acid?

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  1. pH = -log(H^+)
    pH = 3.72; (H^+) = approx 2E-4 but that's an approximation. You should do this more accurately as well as all of the calculations that follow.

    %ion = [(H^+)/Msample]*100

    ...........HA ==> H^+ + A^-
    I.........0.6.....0......0
    C...........-x....x......x
    E........0.6-x....x......x

    You know x is approx 2E-4, Substitute that for x into the Ka expression for HA and solve for Ka.

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