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Henderson Hassleback Equation

pH of 0.5 M...

Question

$p H$ of $0.5 M B a (C N)_{2}$ solution ( $p K_{b}$ of $C N^{-}$ is $9.3$ )

8.35

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3.35

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9.35

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9.50

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Solution

The correct option is C $9.35$
$[C N^{-}] = 2 \times 0.5 = 1.0 M$

$p H = \frac{1}{2} [p K_{w} + p K_{a} + l o g (C N^{-})]$

$\Rightarrow \frac{1}{2} [14 + (14 - K_{b}) + l o g (1.0)]$

$∴$ pH = 9.35

Hence, option C is correct.

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