The dissociation constant of acetic acid is . When 25 mL of 0.2 M solution is mixed with 25 mL of 0.02 M solution, the pH of the resultant solution is found to be equal to 5. The value of is ______. [2023]

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Solution

Q.
The dissociation constant of acetic acid is $x \times 10^{- 5}$ . When 25 mL of 0.2 M ${CH}_{3} COONa$ solution is mixed with 25 mL of 0.02 M ${CH}_{3} COOH$ solution, the pH of the resultant solution is found to be equal to 5. The value of $x$ is ______. [2023]

Ans.
(10)

$p^{H} = p K_{a} + \log [\frac{Salt}{Acid}]$

$5 = p K_{a} + \log (\frac{0.2}{0.02}) = p K_{a}$

$K_{a} = 10 \times 10^{- 5}$

$∴$ $x = 10$

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