Chemistry, asked by ganesh989, 11 months ago

When 0.2M acetic acid is neutralised with 0.1M NaOH in 0.5 litre of water the resulting solution is slightly alkaline. Calculate the pH of the resulting solution. K a ​ for CH 3 ​ COOH=1.8×10 −5 .

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Answered by sakina212
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Answer:

CHEMISTRY

When 0.2M acetic acid is neutralised with 0.1M NaOH in 0.5 litre of water the resulting solution is slightly alkaline. Calculate the pH of the resulting solution. K

a

for CH

3

COOH=1.8×10

−5

.

November 22, 2019avatar

Bellatrix Sree

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ANSWER

0.2M acetic acid will form 0.2M CH

3

COONa and 0.5 litre of water. Hence, concentration of sodium acetate [CH

3

COONa]=0.1molL

−1

CH

3

COO

+H

2

O⇌CH

3

COOH+OH

C(1−x) CxCx

K

h

=

(1−x)

Cx

2

=Cx

2

(1−x)→1

K

h

=

K

a

K

w

=

1.8×10

−5

1×10

−14

=5.5×10

−10

So, K

h

=Cx

2

=5.5×10

−10

or x

2

=55×10

−10

or x=7.42×10

−5

[OH

]=Cx=7.42×10

−5

×0.1=7.42×10

−6

M

[H

+

]=

[OH

]

K

w

=1.3477×10

−9

M

pH=−log[H

+

]=8.87

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