An acid - base indicator which is a weak acid has a $p H$ value = 5.45. At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour half way between those of its acid and conjugate base forms?
[ $p H$ of acetic acid = 4.75. log 2 = 0.3]

4 : 1

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6 : 1

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5 : 1

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3 : 1

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Solution

The correct option is D 5 : 1
$p H = 5.45, p K a = 4.75$

$p H = p K_{a} + l o g \frac{(s o d i u m a c e t a t e i o n)}{A c e t i c a c i d}$

$5.45 = 4.75 + l o g \frac{b a s e}{a c i d}$

$\frac{(s o d i u m a c e t a t e i o n)}{(A c e t i c a c i d)} = 10^{0.7} = 5 : 1$

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