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24 April, 16:02

Pyridine, C5H5N, is a commonly used reagent in the lab. It is a highly flammable, weakly basic, water-miscible liquid with a distinctive, unpleasant fish-like smell. Suppose now in a buffer solution, the concentration of [C5H5N] is 0.01 M and the concentration of [C5H6N+] (the conjugate acid) is 0.02M. What pH is the buffer? (Given that the Kb for C5H5N is 1.8 x 10-9)

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  1. 24 April, 18:30
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    5.0

    Explanation:

    We have a buffer system formed by a weak base (C₅H₅N) and its conjugate acid (C₅H₆N⁺). We can calculate the pOH using the Henderson-Hasselbach's equation.

    pOH = pKb + log [acid]/[base]

    pOH = - log 1.8 * 10⁻⁹ + log 0.02/0.01

    pOH = 9.0

    Then, we will calculate the pH.

    pH + pOH = 14

    pH = 14 - pOH = 14 - 9.0 = 5.0
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