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Van't Hoff Factor

The pH of 0...

Question

The pH of $0.1$ M acetic acid solution is closest to[Dissociation constant of the acid, $K_{a} = 1.8 \times 10^{- 5}$ ]

2.87

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1.00

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2.07

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4.76

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Solution

The correct option is A $2.87$
$C H_{3} C O O H ⇌ C H_{3} C O O^{-} + H^{+}$
$C$
$C - C α$ $C α$ $C α$

$K_{a} = \frac{[C H_{3} C O O^{-}] [H^{+}]}{[C H_{3} C O O H]} = \frac{C α C α}{C (1 - α)} = \frac{C α^{2}}{1 - α} = C α^{2} = 1.8 \times 10^{- 5} (1 - α)$

On solving we get $α = 0.0134$

$[H^{+}] = C α = 0.00134$

$p H = - l o g ([H^{+}])$

$p H = 2.87$

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