The concentrations of acetic acid and sodium acetate is a buffer solution of total moalrity 0.39 M and having a pH of 4.4 if the Ka of acetic acid is is 1.83×10-5 is

$K_{a} = 10 - 4.2 = 6.31 \times 10^{- 5}$ , $log \frac{[S a l t]}{[A c i d]} = p H - p K_{a}$

$= p H + log K_{a}$ = $4.4 + log (1.83 \times 10^{- 5})$ = 4.4 – 4.7 = - 0.3

$\frac{[S a l t]}{[A c i d]} = 10^{- 0.3} = 0.5$ $1 + \frac{[S a l t]}{[A c i d]} = 1 + 0.5$

$\frac{[A c i d] + [S a l t]}{[A c i d]} = 1.5$ , $\frac{t o t a l m o l a r i t y}{[A c i d]} = 1.5$ , $\frac{0.39}{[A c i d]} = 1.5$

$[A c i d] = \frac{0.39}{1.5} = 0.26$ [Salt] = 0.39 – 0.26 = 0.13

The concentrations of acetic acid and sodium acetate is a buffer solution of total moalrity 0.39 M and having a pH of 4.4 if the $K_{a}$ of acetic acid is is $1.83 \times 10^{- 5}$ is