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Calculate the acid dissociation constant of a weak monoprotic acid if a 0.5M solution of this acid gives a hydrogen-ion concentration of 0.000 1M? Show your work.

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  1. Today, 00:22
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    First we create a balanced equation

    HA H (+) + A (-)

    Then, we set up an ICE table

    HA H (+) + A (-)

    []i 0.5M 0M 0M

    Δ[] - x + x + x

    []f 0.5M-x 0.0001M 0.0001M

    From this, we can say that x = 0.0001.

    Next, we set up the equation

    Ka = [H+][A-]/[HA]

    Ka = [0.0001][0.0001]/[0.5-0.0001]

    Ka = 2x10^-8
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