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Henderson Hassleback Equation

The pH of a b...

Question

The pH of a buffer solution containing 2.0 mol per litre $C H_{3} C O O N a$ and 1.5 mol per litre $C H_{3} C O O H$ is: ( $K_{a}$ for acetic acid is $1.8 \times 10^{- 5})$

A

4.87

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B

5.8

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C

2.4

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D

9.2

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Solution

The correct option is A 4.87
The given solution is acidic buffer so Henderson-Hasselbach equation is
$p H = - l o g K_{a} + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 4}] + l o g \frac{[S a l t]}{[A c i d]}$
$p H = - l o g [1.8 \times 10^{- 4}] + l o g \frac{2.0}{1.5}$
$p H = 4.745 + 0.124 = 4.869$

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Henderson Hassleback Equation

Standard XII Chemistry

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