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Henderson Hassleback Equation

The pKb of ...

Question

The $p K_{b}$ of $C N^{⊖}$ is $4.7$ . The $p H$ of solution prepared by mixing $2.5 m o l$ of $K C N$ of $2.5 m o l$ of $H C N$ in water and making the total volume upto $500 m L$ is:

10.3

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9.3

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8.3

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4.7

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Solution

The correct option is C $4.7$
$p H = p K b + l o g \frac{[s a l t]}{[a c i d]}$
$p H = 4.7 + l o g \frac{[2.5]}{[2.5]}$
$= 4.7 + l o g 1$
$= 4.7 + 0$
$= 4.7$
Hence the option $(D)$ is correct.

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