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Electrolysis and Electrolytes

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A solution is obtained by mixing 0.2M,500ml NH_4OH and 0.1M,200ml HCl. Then find pH of a)solution formed b)when 0.4g NaOH is added to it c)when 0.365g HCl is added to it K_b of NH_4OH is 10^{-5

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50 m L

0.1 M

{N H}_{4} O H

50 m L

0.05 M

H C l

solution, the pH is:

Q. A solution of weak acid

H A

was titrated with base

N a O H

. The equivalence point was reached when

36.12 m L

0.1 M

N a O H

has been added. Now

18.06 m L

0.1 M

H C l

were added to titrated solution, the

p H

was found to be

4.92

. What will be the

p H

of the solution obtained by mixing

10 m L

0.2 M

N a O H

10 m L

0.2 M

H A

?

Q. A buffer solution with

p H = 9

is to be prepared by mixing

N H_{4} C I

N H_{4} O H

. Calculate the number of moles of

N H_{4} C I

that should be added to one litre pf

1.0 M

N H_{4} O H

[K_{b} = 1.8 \times 10^{- 5}]

Q. A solution contains 0.2 M

{N H}_{4} O H

{N H}_{4} C I .

If 1.0 ml of 0.001 M HCl is added to it. What will be the

[{O H}^{-}]

of the resulting solution

[K_{b} = 2 \times 10^{- 5}]

:

500 m L

0.2 M

aqueous solution of acetic acid is mixed with

500 m L

0.2 M

H C l

25^{o} C

(a) Calculate the degree of dissociation of acetic acid in the resulting solution and pH of the solution.
(b) If

6 g

N a O H

is added to the above solution, determine final pH. Assume there is no change in volume on mixing.

K_{a}

for acetic acid is

1.75 \times 10^{- 5} M L^{- 1}

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