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A 0.02M solution of pyridinium hydrochlo...

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

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Pyridinium hydrochloride

is salt of `S_(A)//W_(B)`
`pH=1/2 [pK_(w)-pK_(b)- log C]`
`3.44xx2=14-pK_(b)-log(0.02)`
`6.88-14=-pK_(b)-(-1.698)`
`6.88-14-1.698=-pK_(b)`
`pK_(b)=8.818`
`-log K_(b)=8.818`
`K_(b)= Antilog of (-8.818)=-8-0.818+1-1`
`=bar(9).182=1.5xx10^(-9)`.
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