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pH the Power of H

1 M solution ...

Question

$1 M$ solution of $C H_{3} C O O H$ is diluted to x-time so that pH of the solution is doubled. calculate x ? Given: $K_{a} = 1.8 \times 10^{- 5}$

4.55 \times 10^{4}

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5.55 \times 10^{6}

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5.55 \times 10^{4}

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None of the above

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Solution

The correct option is C $5.55 \times 10^{4}$
Given $[C H_{3} C O O H] = 1 M, K_{a} = 1.8 \times 10^{- 5}$
We know that the relation between $p H$ and $p K_{a}$ is given by
$p H = \frac{1}{2} (p K_{a} - l o g C)$
$p H = \frac{1}{2} (p K_{a} - l o g ([C H_{3} C O O H])$
$p H = \frac{1}{2} (p K_{a} - l o g 1)$
$p H = \frac{1}{2} p K_{a}$
Also given,
$p H^{^{'}} = 2 \times p H = 2 \times \frac{1}{2} p K_{a} = p K_{a}$
$p H^{^{'}} = p K_{a}$
$p H^{^{'}} = p K_{a} = \frac{1}{2} (p K_{a} - l o g C^{^{'}})$
$p K_{a} = - l o g C^{^{'}} = - l o g K_{a}$
$- l o g C^{^{'}} = - l o g K_{a}$
$C^{^{'}} = K_{a} = 1.8 \times 10^{- 5}$
Dilution, $x = \frac{1}{C^{^{'}}} = 5.55 \times 10^{4}$

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pH the Power of H

Standard XII Chemistry

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1 M solution of CH3COOH is diluted to x-time so that pH of the solution is doubled. calculate x ? Given: Ka=1.8×10−5

$1 M$ solution of $C H_{3} C O O H$ is diluted to x-time so that pH of the solution is doubled. calculate x ? Given: $K_{a} = 1.8 \times 10^{- 5}$