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5 November, 23:35

If a buffer solution is 0.130 M 0.130 M in a weak acid (K a = 1.4 * 10 - 5) Ka=1.4*10-5) and 0.540 M 0.540 M in its conjugate base, what is the pH?

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  1. 5 November, 23:58
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    Answer: pH = 0.68015

    Explanation:

    From the question,

    pKa = 1.5*10-5, [salt] = 0.54M, [ acid]=0.13M

    Using the Henderson Hasselbalch equation

    pH = pKa + log[salt/acid]

    pH=1.4*10-4 + log[0.54/0.14]

    pH = 0.000015 + 0.618

    pH=0.68015
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