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A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine. |
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Answer» Pyridinium hydrochloride is a salt of a weak base (pyridine) and a strong acid (HCl). The pH of an aqueous solution of this salt is given by the relation: pH = \(\frac{1}{2}\) [pKw - pKb - logC] 3.44 = \(\frac{1}{2}\) [14+logkb - log (0.02)] 6.88 = 14 + log Kb + 1.7 log Kb = -8.82 ∴Kb = antilog(-8.82) = 1.514 x 10-9 |
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