What ratio of acetic acid to sodium acetate concentration is needed to achieve a buffer whose pH is 5-70- The dissociation constant of acetic acid is 1-8times - 10 - -5 -

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Toppr Admin · Accepted Answer

PH-pKa-log-Salt-Acid-5-7-5-x2212-log-1-8-log-Salt-Acid-5-7-5-x2212-0-255-log-Salt-Acid-0-955-log-Salt-Acid-x27F9-Salt-Acid-9

What ratio of acetic acid to sodium acetate concentration is needed to achieve a buffer whose pH is $5.70$ ? The dissociation constant of acetic acid is $1.8 \times 10^{- 5}$ .

$p H = p K_{a} + log \frac{[S a l t]}{[A c i d]}$
$5.7 = 5 - l o g (1.8) + log \frac{[S a l t]}{[A c i d]}$
$5.7 = 5 - 0.255 + log \frac{[S a l t]}{[A c i d]}$
$0.955 = log \frac{[S a l t]}{[A c i d]}$
$⟹ \frac{[S a l t]}{[A c i d]} = 9$

What ratio of acetic acid to sodium acetate concentration is needed to achieve a buffer whose pH is 5.70? The dissociation constant of acetic acid is 1.8×10−5.

pH=pKa+log[Salt][Acid]5.7=5−log(1.8)+log[Salt][Acid]5.7=5−0.255+log[Salt][Acid]0.955=log[Salt][Acid]⟹[Salt][Acid]=9

What ratio of acetic acid to sodium acetate concentration is needed to achieve a buffer whose pH is $5.70$ ? The dissociation constant of acetic acid is $1.8 \times 10^{- 5}$ .

$p H = p K_{a} + log \frac{[S a l t]}{[A c i d]}$
$5.7 = 5 - l o g (1.8) + log \frac{[S a l t]}{[A c i d]}$
$5.7 = 5 - 0.255 + log \frac{[S a l t]}{[A c i d]}$
$0.955 = log \frac{[S a l t]}{[A c i d]}$
$⟹ \frac{[S a l t]}{[A c i d]} = 9$