What is the pH of 0.1 M acetic acid solution $K_{a} = 1.8 \times 10^{- 5}$ . To what volume 1 liter of the solution be diluted so that pH of the solution becomes double of the initial .

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Solution

$C_{1} V_{1} = C_{2} V_{2}$
$0.1 \times 1 = 1.819 \times 10^{- 7} \times V_{2}$
$V_{2} = 5 \cdot 5 \times 10^{5} L$

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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. The pH of

0.1

M acetic acid solution is closest to[Dissociation constant of the acid,

K_{a} = 1.8 \times 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}

5.0 m L

0.1 M N a O H

solution is added to

50 m L

of the

0.1 M

acetic acid solution. Calculate the

p H

of the resulting acetic acid solution.

(K a = 1.8 \times 10^{- 5})

Q. One litre of

1 M

solution of an acid

H A

(

K_{a} = 10^{- 4}

25^{o} C

) has pH=2. It is diluted by water so that new pH becomes double. The solution was diluted to

5 \times 10^{a}

ml. The value of

a

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What is the pH of 0.1 M acetic acid solution Ka=1.8×10−5 . To what volume 1 liter of the solution be diluted so that pH of the solution becomes double of the initial .

C1V1=C2V20.1×1=1.819×10−7×V2V2=5⋅5×105L

What is the pH of 0.1 M acetic acid solution $K_{a} = 1.8 \times 10^{- 5}$ . To what volume 1 liter of the solution be diluted so that pH of the solution becomes double of the initial .

$C_{1} V_{1} = C_{2} V_{2}$
$0.1 \times 1 = 1.819 \times 10^{- 7} \times V_{2}$
$V_{2} = 5 \cdot 5 \times 10^{5} L$