What is the $p H$ of a $1.0 M$ solution of acetic acid? To what volume must $1$ litre of the solution be diluted so that the $p H$ of the resulting solution will be twice the original value. Given $K_{a} = 1.8 \times 10^{- 5}$ . (in lit).

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Solution

In begining $[H^{+}] = \sqrt{K_{a} C}$
$[H^{+}] = \sqrt{1.8 \times 10^{- 5}} = 0.004242$
$p H = 2.372$
On doubling $p H$ , new $p H$
$= 4.744$
$[H^{+}] = 1.8 \times 10^{- 5}$
${C H}_{3} C O O H ⇌ {C H}_{3} C O O^{-} + H^{+}$
$C$
$C - C α$ $C α$ $C α$
$K_{a} = \frac{{(C α)}^{2}}{C (1 - α)}$ , $C α = [H^{+}] = 1.8 \times 10^{- 5}$
$1.8 \times 10^{- 5} = \frac{{(1.08 \times 10^{- 5})}^{2}}{(C - C α)}$
$C - C α = 1.8 \times 10^{- 5}$
$V = \frac{1}{C} = 2.77 \times 10^{4} L = 27700 l i t .$

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To what volume one litre of 0.1M acetic acid solution diluted so that the pH of the solution becomes double of the initial ? ( $K_{a} = 1.8 \times 10^{- 5}$ )

Q. What is the pH of the solution when 0.2 mole of hydrochloric acid is added to one litre of a solution containing 1 M acetic acid and acetate ion? Assume that the total volume is one litre.

K_{a}

for

{CH}_{3} COOH = 1.8 \times 10^{- 5}

1

litre solution of

p H = 1

is diluted up to

10

times. What volume of a solution with

p H = 2

is to be added in the diluted solution, so that the final

p H

remains

^{'} 2^{'}

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What is the pH of a 1.0M solution of acetic acid? To what volume must 1 litre of the solution be diluted so that the pH of the resulting solution will be twice the original value. Given Ka=1.8×10−5. (in lit).

In begining [H+]=√KaC[H+]=√1.8×10−5=0.004242pH=2.372On doubling pH, new pH=4.744[H+]=1.8×10−5CH3COOH⇌CH3COO−+H+CC−Cα Cα CαKa=(Cα)2C(1−α), Cα=[H+]=1.8×10−51.8×10−5=(1.08×10−5)2(C−Cα)C−Cα=1.8×10−5V=1C=2.77×104L=27700lit.

What is the $p H$ of a $1.0 M$ solution of acetic acid? To what volume must $1$ litre of the solution be diluted so that the $p H$ of the resulting solution will be twice the original value. Given $K_{a} = 1.8 \times 10^{- 5}$ . (in lit).