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20 May, 23:21

A 0.070 M solution of the salt NaB has a pH of 9.60. Calculate the pH of a 0.010 M solution of HB.

Or, what is the Kb of HB?

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  1. 21 May, 00:28
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    B - + H2O HB + OH-

    pOH = 14 - 9 = 5

    [OH-] = [HB] = 10^-5 M

    Kb = (10^-5) ^2 / 0.050 - 10^-5 = 2 x 10^-9

    Ka = Kw/Kb = 5 x 10^-6 = x^2 / 0.0010-x

    x = [H+] = 0.000071 M

    pH = 4.2
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