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Acid-Base Equilibrium

  1. Feb 2, 2008 #1
    The base hydrazine, N2H4, has a pKb equal to 5.90. Calculate the hydroxide concentration, the pH, and the % ionization for a 0.12 M solution.

    First, is pKb the same as the pOH?

    If so, pOH = -log[OH-]
    5.90 = -log[OH-]
    log[OH-] = -5.90
    [OH-]=1.26 x 10^-6

    pH = 14.00 - pOH
    =14.00 - 5.90

    % ionized = [OH-]/0.12 M X 100% = 0.00105% ?

    Somehow I think I'm doing this problem wrong. Can anybody show me what the problem is?
  2. jcsd
  3. Feb 4, 2008 #2


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    No. pKb is analagous to pKa. It is the negative log of Kb.
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