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8 June, 06:37

Mixing Strong Acids with Strong Bases What is the pH of the solution that results from mixing 8.00 mL of 0.030 M perchloric acid with 28.00 mL of 0.050 M barium hydroxide? Check all of the following species that would be present in solution as a result of these two solutions being mixed. Ignore the traces of hydronium and hydroxide ions that would naturally be present from the autoionization of water. Ba2 + (aq) H2O (l) ClO3 - (aq) OH - (aq) ClO4 - (aq) H3O + (aq)

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  1. 8 June, 09:22
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    Answer: PH = 1.4

    Explanation:

    n (mole) = concentration (c) * volume (v)

    n (HClO4) = 0.08 * 0.03

    n (HClO4) = 0.0024 mole

    n (Ba (OH) 2) = 0.28 * 0.05

    n (Ba (OH) 2) = 0.014

    2HClO4 + Ba (OH) 2 ... >Ba (ClO4) 2 + 2H2O.

    Hence, the limiting reagent is perchloric acid. According to the reaction:

    0.0024 HClO4 req 1/2 * 0.0024 of Ba (OH) 2.

    n (Ba (OH) reacted = 0.0012

    Excess n (Ba (OH) 2) = 0.014-0.0012

    Excess n (Ba (OH) 2) = 0.0128

    Conc (Ba (OH) 2) unreacted = 0.0128/.32 (vol. of mix is 32ml)

    = 0.04M = [H+]

    PH = - log[0.04] = 1.397

    PH = 1.4
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