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    Acid-Base Equilibria

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    Hey there. I am having trouble with this question.

    Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations:
    a) 0.250 M
    b) 0.0800 M
    c) 0.0200 M
    ** Ka = 1.3 x 10 ^ -5

    Could you please show the work. And no power points please.

    Thanks in advance!

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    Solution Preview

    Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations:
    a) 0.250 M
    b) 0.0800 M
    c) 0.0200 M
    ** Ka = 1.3 x 10 ^ -5

    a) 0.250 M
    C2H5COOH ↔ H+ + C2H5COO-
    Initial 0.25 --- ------
    Change -x +x +x
    Equilibrium 0.25-x x x

    Ka = [H+][ C2H5COO-] / ...

    Solution Summary

    Acid base equilibria are examined. The percent ionization of propionic acid is calculated.

    $2.49

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