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Basic Buffer Action

The pH of a...

Question

The $p H$ of a buffer solution having $0.001 M$ $N H_{4} O H$ and $0.01 M$ $N H_{4} C l$ is ( $K_{b}$ of base is $0.01$ ) :

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Solution

The correct option is A 11
The expression for the $p O H$ of the basic buffer solution is as given below:
$p O H = p K_{b} + l o g \frac{[s a l t]}{[b a s e]}$
$p K_{b} = - l o g K_{b} = - l o g 0.01 = 2$
By substituting values in the above equation, we get
$p O H = 2 + l o g \frac{0.01}{0.001} = 3$
$p H = 14 - p O H = 14 - 3 = 11$

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