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A 0.02 M solution of pyridinium hydrochl...

A `0.02 M` solution of pyridinium hydrochloride has `pH=3.44`. Calculate the ionization constant of pyridine.

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The aqueous solution of pyridium hydrochloride is an acidic solution due to hydrolysis. Observe that it is a salt of strong acid, HCl and weak base, Pyridine.
`C_(5)H_(5)N^(+)HCl^(-) + H_(2)O to C_(6)H_(5)N^(+)HOH^(-) + HCl`
Using standard result of pH :`pH=7- (pK_(b))/2 – (logC)/2 implies 3.44=7- (pK_(b))/2 – (log0.02)/2`
On solving and substituting values, `K_(b)=1.5xx10^(-9)`
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