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Lewis Theory

When a small ...

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When a small amount of HCL os added to a buffer solution of acetic acid and sodium acetate- Ph increases H+ decrease Dissociation of acetic acid decrease

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Q. pH of a buffer solution decreases by

0.02

0.12 g

of acetic acid is added to

250 m L

of a buffer solution of a acetic acid and potassium acetate at

27^{o} C

. The buffer capacity of the solution is:

Q. When some amount of sodium acetate is further added to a mixture of acetic acid and sodium acetate, then pH of the solution:

1 \times 10^{- 3}

H C l

is added to a buffer solution made up of

0.01 M

acetic acid and

0.10 M

sodium acetate. The final pH of the buffer will be: (given

p K_{a}

of acetic acid is

4.75

25^{o} C

)

Q. In order to prepare a buffer solution of pH 5.74, sodium acetate is added to acetic acid. If the concentration of acetic acid in the buffer is 1.0 M, the concentration of sodium acetate in the buffer is ______M. (Round off to the Nearest Integer).
[Given:

p K_{a}

(acetic acid) = 4.74]

Q. Suppose it is required to make a buffer solution of

p H = 4

, using acetic acid and sodium acetate. How much of sodium acetate is to be added to

1

N / 10

acetic acid?
Dissociation constant of acetic acid

1.8 \times 10^{- 5}

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