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Finding Hydrolysis Constant

  1. Apr 30, 2007 #1
    Hi! First post I must say ... but more importantly I need help finding the hydrolysis constant (Kh) from pH of an unknown salt. This is what i have so far.

    We took the measurement of pH of a 1.0 M solution onf an unknown salt in which one of the ions hydrolyzes. The pH our group got was 0.95. This means that Ka > Kb (that's why it's acidic) and this means the cation hydrolyzes.

    We know that Kh = Ka = { [H3O+] / [BH+] }

    So to find the [H3O+] i did the following steps:

    pH = -log[H3O+]
    [H3O+] = 10^-pH
    [H3O+] = 10^-.95
    [H3O+] = .1122

    Next we know Ka = { [H3O+][A-] / [HA] } or better known as concentrations of products of concentrations of reactants. So now i get Ka = (.1122)(.1122) / 1 so Ka =.01259

    Which as stated above Kh = Ka so am I right with the hydrolyzes constant?
  2. jcsd
  3. May 1, 2007 #2


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    You are really close. The [BH+] term in your Ka expression is a little off. Remember that at equilibrium the concentration of [BH+] has been reduced by an equal amount as the [H+]. Set [H+] to x and the Ka expression becomes:

    Ka = x^2/[BH+ - x]

    Substitute a value (that you have) for 'x' and solve from there.
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