Calculate the % dissociation of 0.10 M solution of acetic acid (pKa = 4.75)

Question

Calculate the % dissociation of 0.10 M solution of acetic acid (pKa = 4.75)

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Doris 4 weeks 2021-08-18T04:02:06+00:00 1 Answers 1 views 0

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    2021-08-18T04:03:32+00:00

    Given :

    Molarity of acetic acid solution, M = 0.10 M.

    pKa of acetic acid, pKa = 4.75 .

    To Find :

    Percentage dissociation of 0.10 M solution of acetic acid.

    Solution :

    We know, pK_a = -log\  K_a

    Taking antilog both side, we get :

    K_a = 1.78\times 10^{-5}

    Since, acetic acid has 1 hydrogen atom to loose , so it is a monoprotic acid.

    Now, percentage dissociation of monoprotic acid is given by :

    \alpha = \sqrt{\dfrac{K_a}{C}}\\\\\alpha =\sqrt{ \dfrac{1.78\times 10^{-5}}{0.1}}\\\\\alpha = 	0.0133\times 100 = 1.33 \%

    Hence, this is the required solution.

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