weak acid, HA, is 0.1 % ionized in a 0.2 M solution.
(a) What is the equilibrium constant for the dissociation of the acid (Ka)?
(b) What is the pH of the solution?

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  1. ..................HA ==> H^+ + A^-
    HA = 0.2 M and 0.1% ionized; therefore,
    (H^+) = (A^-) = 0.2 M x 0.001 = 2E-4 and (HA) = 0.2-2E-4
    Ka = (H^+)(A^-)/(HA)
    Substitute the numbers into the Ka expression and solve for Ka.

    b part. pH = -log(H^+). You know (H^+) from above, calculate pH. Post your work if you get stuck.

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