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Basic Buffer Action

Solution of 0...

Question

Solution of 0.1 N $N H_{4} O H$ and 0.1 N $N H_{4} C l$ has pH 9.25. $p K_{b}$ of $N H_{4} O H$ is :

9.25

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4.75

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3.75

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8.25

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Solution

The correct option is B 4.75
We know the relation,
$p H + p O H = 14 (a t 25^{o} C)$
$9.25 + p O H = 14$
$p O H = 14 - 9.25$
$p O H = 4.75 . . . . . (1)$
Using the Henderson-Hasselbalch equation for weak bases:
$p O H = p K_{b} + l o g [\frac{[c o n j u g a t e a c i d]}{[b a s e]}]$
$p O H = p K_{b} + l o g (1)$
$p O H = p K_{b} (∵ l o g 1 = 0)$
$p K_{b} = 4.75$ (from equation 1)
Hence $p K_{b}$ value is 4.75

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