Calculate the percentage of pyridine ( C5H5N) that forms pyridinium ion

Question: Calculate the percentage of pyridine ( C5H5N) that forms pyridinium ion, C5H5NH+ , in a 0.10 M aqueous solution of pyridine (Kb = 1.7×10-9). Please Explain how ! i dont get it at all !! please help !

Solution: Concepts and reason

The concept used to solve this problem is determining the ratio between present hydroxide ion concentration and total base concentration. Fundamentals

The percentage ionization of any base is calculated as follows:

The chemical equation and equilibrium constant expression for Pyridine is as follows:

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According to the problem;

base dissociation or equilibrium constant

Therefore for the weak base calculate the

by using the following formula:

is the concentration of base and is the equilibrium constant for base.

Now Find out; Percentage ionization =?

Now we calculate the percentage ionization:

Thus, in the given solution of pyridine there is 0.013% ammonium ions are present.

The percentage ionization is given by following expression:

Thus, in the given solution of pyridine there is 0.013% ammonium ions are present.