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For a 0.15 M solution of pyridine, calculate the percent ionization of this weak base. Please...

For a 0.15 M solution of pyridine, calculate the percent ionization of this weak base. Please show all steps. Thanks

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Answer #1

pyridine is a weak base.

Kb of pyridine = 1.7*10^-9

Kb = CX^2

(1.7*10^-9) = 0.15*X^2

X = degree of dissociation = 1.06*10^-4

percent ionization = X*100

                             = 1.06*10^-4*100

                              = 0.0106 %

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