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Henderson Hassleback Equation

The pH of an ...

Question

The pH of an acid buffer can be raised by 2 units by:

A

Increasing the concentration of both weak acid and salt by two moles

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B

Increasing the concentration of both the acid and salt by 10 times

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C

Diluting the solution by 10 times

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D

Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times

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Solution

The correct option is D Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times
For an acidic buffer solution, we use the Henderson-Hasselbalch equation
Or
$p H = p K_{a} + l o g \frac{[s a l t]}{[a c i d]}$
So Case I
$p H_{1} = p K_{a} + l o g \frac{[s a l t_{1}]}{[a c i d_{1}]}$ ....(1)
So Case 2
$p H_{2} = p K_{a} + l o g \frac{[s a l t_{2}]}{[a c i d_{2}]}$ ....(2)
According to question,
(2)-(1) =2; $p K_{a}$ terms will get cancelled we get
2 = $l o g \frac{[a c i d_{1}] \times [s a l t_{2}]}{[s a l t_{1}] \times [a c i d_{2}]}$
taking antilog and solving
$\frac{[a c i d_{1}] \times [s a l t_{2}]}{[s a l t_{1}] \times [a c i d_{2}]} = 10^{2}$
When the concentration of salt is increased by 10 times and concentration of acid is decreased by 10 times, then we get this ratio.

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