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Basic Buffer Action

Calculate p...

Question

Calculate $p H$ of a buffer solution that contains $0.1 M N H_{4} O H (K_{b} = 10^{- 5})$ and $0.1 M N H_{4} C l$ .

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Solution

$p K_{b} = - l o g K_{b} = - l o g 10^{- 5} = 5$
A mixture of ammonium hydroxide and ammonium chloride forms basic buffer solution.
The Hendrson's equation for he basic buffer solution is as given below.
$p O H = p K_{b} + l o g \frac{[s a l t]}{[a c i d]}$
Substitute values in the above expression.
$p O H = 5 + l o g \frac{0.1}{0.1} = 5$
Hence, the pH of the solution is $p H = 14 - p O H = 14 - 5 = 9$

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