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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?

Carlton Burgess

in Chemistry

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Melissa Norris on November 18, 2018

The answer is: pH of a 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 the quadratic equation: [H⁺] = 0.000524 M. pH = -log[H⁺].pH = -log(0.000524 M).pH = 3.28.


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