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Arrhenius Acid

The p K a o...

Question

The $p K_{a}$ of a weak acid is $5.85$ . The concentration of the acid and its conjugate base are equal at a pH of:

A

2.93

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B

5.85

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C

4.85

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D

7.85

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Solution

The correct option is B $5.85$
Given that,
$[A c i d] = [C o n j . b a s e]$

For weak acid,

$p H = p K a + l o g \frac{[C o n j . b a s e]}{[A c i d]} = p K a + l o g 1 = 5.85$ .

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