The basicity constant of pyridine can be expressed as pKb = 8.75 what will be the pH of a 1M (1 mole per liter) solution of pyridine in water?
Py + HOH ==> PyH^+ + OH^-
Kb = (PyH^+)(OH^-)/(Py)
Change pKb to Kb, plug in x for (PyH^+) and (OH^-) and 1 for (Py) and solve for x. That will be OH^- so determine pOH and remember pH + pOH = 14.
Post your work if you get stuck.
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The pKb of pyridine is 8.75. What is the pH of a 0.480M solution of pyridine?
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