Salt of Stron...

Salt of Strong Acid and Weak Base

Trending Questions

100ml of 0.1 M NaOH is added to 100 ml of a 0.2 M CH₃COOH solution. The pH of the resulting solution will be (pk_a=4.74)

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Q. The base dissociation constant for hydrazine

N_{2} H_{4}

9.6 \times 10^{- 7}

. What would be the percent hydrolysis of

0.1 M N_{2} H_{5} C l

, a salt containing the acid ion conjugate to hydrazine base at

25^{\circ} C

$2.667 \times 10^{- 3}$
$1.525 \times 10^{- 4}$
$3.225 \times 10^{- 2}$
$4.557 \times 10^{- 6}$

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Q. What is the approximate value of

p H

of a

0.2 M

solution of ammonia? Given,

K_{b} = 1.76 \times 10^{- 5}

$9.82$
$11.28$
$13.47$
$8.56$

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Which of the following solution will have a pH exactly equal to 9 ?

$10^{- 9} M H C l solution at 25^{0} C$
$2 \times 10^{- 3} M B a (O H)_{2} solution at 25^{0} C$
$10^{- 9} M N a O H solution at 25^{0} C$
None of the above

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2 M

solution of

N a_{2} C O_{3}

is boiled in a closed container with excess of

C a F_{2} .

Very little amount of

C a C O_{3}

and

N a F

are formed. If the solubility product

(K_{s p}

C a C O_{3}

is x and molar solubility of

C a F_{2}

is y, find the molar concentration of

F^{-}

in resulting solution after equilibrium is attained.

$\frac{8 y^{3}}{x}$
$\sqrt{\frac{4 y^{3}}{x}}$
$\frac{4 y^{3}}{x}$
$\sqrt{\frac{8 y^{3}}{x}}$

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Q. Consider a strong base,

A O H

solution having a

p H = 11

mixed in an equal volume with another solution of strong base,

B O H

to give a resultant solution of

p H = 12

. Find the

p H

of solution containing strong base

B O H

13.9
12.8
12.3
13.3

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Q. Calculate amount of

N H_{4} C l

required to be dissolved in

500 m L

water to have

p H = 5. [K_{b} N H_{4} O H = 1.8 \times 10^{- 5}] .

(Molar mass of

N H_{4} C l = 53.5 g m o l^{- 1}

)

1.855 g
2.543 g
4.815 g
6.066 g

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Q. In the dissociation of

N H_{4} O H

, if

N H_{4} C l

is added what will be the change in

p H

for the

N H_{4} O H

solution ?

Increases
No change
first decreases and then increases.
Decreases

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Q. Calculate pH of mixture of

(400 m L, \frac{1}{200} M B a (O H)_{2}) + (400 m L, \frac{1}{50} M H C l) + (200 mL of water)

l o g 2 = 0.3010

2.4
7
more than 7
4.5

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Q. A solution contains

N a_{2} C O_{3}

and

N a H C O_{3}

10 mL

of this solution required

2.5 mL

0.1 M H_{2} S O_{4}

for neutralization using phenolphthalein as an indicator. Methyl orange is then added when a further

2.5 mL

0.2 M H_{2} S O_{4}

was required. The amount of

N a_{2} C O_{3}

and

N a H C O_{3}

respectively, in 1 litre of solution is:

$5.3 g and 4.2 g$
$3.3 g and 6.2 g$
$4.2 g and 5.3 g$
$6.2 g and 3.3 g$

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A solution of $C u S O_{4}$ is

Acidic in nature
Alkaline in nature
Neutral in nature
Amphoteric in nature

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Q. What is pH of 50 ml 0.1 (M)

N H_{4} O H

and 50 ml 0.05 (M) HCI?

p K_{b} = 4.73

9.37
8.37
9.47
9.27

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Q. Aniline behaves as a weak base. When

0.1 M, 50 m L

solution of aniline was mixed with

0.1 M, 25 m L

solution of

H C l

the

p H

of resulting solution was 8. The

p H

0.01 M

solution of anilinium chloride will be:

$5$
$4.5$
$6$
$6.5$

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Q. If the hydrolysis constant of

N H_{4} C l

4 \times 10^{- 10}

298 K

. Find the

p H

0.5 M

solution of

N H_{4} C l

at equilibrium.
Given :

log 5 = 0.7

8.22
2.5
7.34
4.85

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Q. 40 ml of 0.1 M ammonia solution is mixed with 20 mL of 0.1 M HCl. What is the pH of a mixture? (

p K_{b}

of ammonia solution is 4.74)

4.74
2.26
9.26
5

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Q. 2.5 mL of

\frac{2}{5} M

weak monoacidic base (

K_{b} = 1 \times 10^{- 12}

) at

25^{o} C

is titrated with

\frac{2}{15} M

HCl in water at

25^{o} C .

The concentration of

H^{+}

at equivalence point is

(K_{w} = 1 \times 10^{- 14} a t 25^{o} C)

$3.7 \times 10^{- 13} M$
$3.2 \times 10^{- 7} M$
$3.2 \times 10^{- 2} M$
$2.7 \times 10^{- 2} M$

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2.5 m L

\frac{2}{5} M

weak monoacidic base

(K_{b} = 1 \times 10^{- 12})

25^{o} C

is titrated with

\frac{2}{15} M

H C l

in water at

25^{o} C .

The concentration of

H^{+}

at equivalence points is

(K_{w} = 1 \times 10^{- 14} a t 25^{o} C)

$3.7 \times 10^{- 13} M$
$3.2 \times 10^{- 7} M$
$3.2 \times 10^{- 2} M$
$2.7 \times 10^{- 2} M$

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Q. What is pH of 50 ml 0.1 (M)

N H_{4} O H

and 50 ml 0.05 (M) HCI?

p K_{b} = 4.73

9.27
9.37
8.37
9.47

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