First slide

Ionization constants of weak acids, PH of weak acids

Question

What is the pH of a 1 M ${CH}_{3} COOH$ a solution $K_{a}$ of acetic acid = $1.8 \times 10^{- 5} ?$
$K = 10^{- 14} {mol}^{2} {litre}^{- 2}$

Moderate

A

9.4
B

4.8
C

3.6
D

2.4

Solution

${CH}_{3} {COO}^{-} + H_{2} O ⇌ {CH}_{3} COOH + {OH}^{-}$
$[{OH}^{-}] = c \times h; h = \sqrt{\frac{K_{w}}{K_{a}} \times c} = \sqrt{\frac{10^{- 14}}{1.8 \times 10^{- 5}} \times 1} = 2.35 \times 10^{- 5} ∴ pOH = 4.62; pH = 9.38 \approx 9.4$

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