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14 January, 07:20

If the ka of a monoprotic weak acid is 1.2 * 10-6, what is the ph of a 0.23 m solution of this acid?

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  1. 14 January, 08:12
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    Answer is: pH of monoprotic weak acid is 3.28.

    Chemical reaction: HA (aq) ⇄ A⁻ (aq) + H⁺ (aq).

    c (monoprotic acid) = 0.23 M.

    Ka = 1.2 ·10⁻⁶.

    [A⁻] = [H⁺ ] = x.

    [HA] = 0.23 M - x.

    Ka = [A⁻]·[H⁺] / [HA].

    1.2·10⁻⁶ = x² / (0.23 M - x).

    Solve quadratic equation: [H⁺] = 0.000524 M.

    pH = - log[H⁺].

    pH = - log (0.000524 M).

    pH = 3.28.
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