Salt of Weak ...

Salt of Weak Acid and Strong Base

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Q. What is the pH when 25.0 mL of 0.2 M of

C H_{3} C O O H

has been titrated with 35.0 mL of 0.1 M

N a O H

p K_{a} (C H_{3} C O O H) = 4.752

l o g 2.333 = 0.368

7
3.45
5.12
6.52

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K_{a}

for butyric acid is

2.0 \times 10^{- 5}

. Calculate pH and hydroxyl ion concentration in

0.2 M

aqueous solution of sodium butyrate.

$p H = 5; [O H]^{-} = 10^{- 5} M$
$p H = 9; [O H]^{-} = 10^{- 9} M$
$p H = 9; [O H]^{-} = 10^{- 5} M$
$p H = 5; [O H]^{-} = 10^{- 9} M$

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Which of the following statement(s) is/are true?

The pH of $10^{- 8} M H C l$ is 8
The conjugate base of $H_{2} P O_{4}^{-}$ is $H P O_{4}^{2 -}$
If in an aqueous solution $[H^{+}]_{s t r o n g a c i d} < 10^{- 6} M$
$[H^{+}]$ of water cannot be neglected.
If in an aqueous solution $[O H^{-}]_{s t r o n g b a s e} < 10^{- 6}$ then in $[O H^{-}]$ of water can be neglected.

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Q. Which of the following statement(s) is/are correct for an equimolar aqueous solution of

H C l

and

N H_{4} O H

$N H_{4}^{+}$ ions will undergo hydrolysis to form $N H_{4} O H$
Solution will be basic in nature.
Solution will be acidic in nature.
Hydrolysis does not occur

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Q. A solution consists of

C H_{3} C O O H (p K_{a} = 4.74)

and

C H_{3} C O O N a

. If the

p H

of the solution reaches 6.74, the percentage dissociation of

C H_{3} C O O H

is:

50%
1%
99%
None of these

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Q. Calculate pH of

0.002 N N H_{4} O H

having 2 % dissociation.

7.6
8.6
9.6
10.6

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The degree of hydrolysis and pH of $0.1 M$ sodium acetate solution are:
Hydrolysis constant of sodium acetate is $5.6 \times 10^{- 10}$ .

$h$ = $7.5 \times 10^{- 7} M$ , $p H$ = $7.9$
$h$ = $8.5 \times 10^{- 6}$ , $p H$ = $6.9$
$h$ = $8.5 \times 10^{- 7}$ , $p H$ = $7.9$
$h$ = $7.5 \times 10^{- 6}$ , $p H$ = $7.9$

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Q. The sodium salt of a certain weak monobasic organic acid is hydrolysed to an extent of

3 %

in its

0.1 M

solution at

25^{\circ} C

. Given that the ionic product of water is

10^{- 14}

at this temperature, what is the dissociation constant of the acid ?

$1 \times 10^{- 10}$
$1 \times 10^{- 9}$
$3.33 \times 10^{- 9}$
$3.33 \times 10^{- 10}$

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40 m L

0.5 M C H_{3} C O O H

is titrated with of

0.5 M N a O H .

Find the

p H

of the solution when

39 m L

N a O H

has been added.
Given:

K_{a} (C H_{3} C O O H) = 1.9 \times 10^{- 5}

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Q. Which of the following is correct for a salt of weak acid and strong base?
Here C is the concentration of the salt.

$p H = 7 + \frac{1}{2} (p K_{a} + l o g C)$
$p H = 7 + \frac{1}{2} (p K_{b} + l o g C)$
$K_{h} = \frac{K_{w}}{K_{a}}$
$K_{h} \times K_{w} = K_{a}$

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Q. Given

N O_{2}^{-} + H_{2} O ⇋ H N O_{2} + O H^{-}

K_{b} = 2.22 \times 10^{- 11}

Thus, the degree of hydrolysis of 0.04

M

N a N O_{2}

solution is:

$1.14 \times 10^{- 2}$
$2.36 \times 10^{- 5}$
$0.11$
$4.86 \times 10^{- 3}$

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Q. Choose the correct statements for an aqueous solution of

K O C l

The solution will be basic in nature
The solution will be acidic in nature.
Cationic $(K^{+})$ hydrolysis occurs.
Anionic $(O C l^{-})$ hydrolysis occurs

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Q. Calculate

[O H^{-}]

of 0.01 M solution of ammonium hydroxide solution. The ionization constant (

K_{b}

) for

N H_{4} O H = 1.8 \times 10^{- 5}

$4.24 \times 10^{- 4} m o l L^{- 1}$
$4.24 \times 10^{- 2} m o l L^{- 1}$
$1.80 \times 10^{- 4} m o l L^{- 1}$
$1.80 \times 10^{- 3} m o l L^{- 1}$

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Q. Which of the following concentrations of

N H_{4}^{+}

will be sufficient to prevent the precipitation of

M g (O H)_{2}

from a solution which is

0.01 {M MgCl}_{2}

and

0.1 {M NH}_{3} (a q)

? Given that the

K_{s p}

M g (O H)_{2} = 2.5 \times 10^{- 11}

and

K_{b}

for

N H_{3} (a q) = 2 \times 10^{- 5}

0.01 M
0.02 M
0.03 M
0.04 M

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20 m L

0.2 M C H_{3} C O O N a

solution is titrated against

0.1 M H C l

. Calculate the

p H

of solution when

10 m L H C l

has been added.
Given:

p K_{a} (C H_{3} C O O H) = 4.74

5.22
6.44
3.55
7.64

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Q.
Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is ___

KCN

K_{2} S O_{4}

(N H_{4})_{2} C_{2} O_{4}

N a C l

Z n (N O_{3})_{2}

F e C l_{3}

K_{2} C O_{3}

N H_{4} N O_{3}

L i C N

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Q. What amount (in milli mole) of sodium acetate

(C H_{3} C O O N a)

must be added to

2 L

0.1 M

acetic acid solution to given a solution of pH = 3 [Given:

K_{a (C H_{3} C O O H)} = 10^{- 5}]

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Q. Calcium lactate is a salt of weak organic acid and is represented by

C a (L a c)_{2}

. A saturated solution of

C a (L a c)_{2}

contains 0.13 mol of this salt in 0.5 L solution. The pOH of this solution is 5.60. Assuming complete dissociation of the salt. Calculate

p K_{a}

of lactic acid.

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1.00 L

of a buffer that is

0.100 M

H O A c

(

p K_{a} = 4.74)

and

0.100 M

N a O A c

. What is the pH after the addition of

0.0200 m o l

N a O H

(l o g 1.5 = 0.176)

4.92
4.74
8.74
6.74

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Q. When 50 mL of 0.1 M NaOH is added to 50 mL of 0.1 M

C H_{3} C O O H

solution, the pH will be:
(use :

(p K_{a})_{a c e t i c a c i d} = 5, l o g 2 = 0.3, l o g 3 = 0.5, l o g 5 = 0.7)

4.75
9.75
4.25
8.85

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Q. A solution consists of

C H_{3} C O O H (p K_{a} = 4.74)

and

C H_{3} C O O N a

. If the

p H

of the solution reaches 6.74, the percentage dissociation of

C H_{3} C O O H

is:

50%
1%
99%
None of these

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50 m L

of a

0.1 M C H_{3} C O O N a (a q)

is titrated against a

0.1 M H C l (a q)

. Calculate the

p H

of solution when

50 m L H C l

was added.
Given:

p K_{a} (C H_{3} C O O H) = 4.74 a t 25^{o} C

4.74
3.02
5.25
4.24

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The addition of ammonium chloride to 0.1 M acetic acid will cause:

increase in its pH value
decrease in its pH value
no change in pH value
change in pH which cannot be predicted

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Q. For sodium acetate solution in water, the given equilibrium reaction occur:

C H_{3} C O O^{-} (a q) + H_{2} O (l) h y d r o l y s i s ⇌ C H_{3} C O O H (a q) + O H^{-} (a q)

Which of the following describes the correct relation ?
(where

h

is the degree of hydrolysis of salt)

$h = \sqrt{\frac{K_{w} \cdot C}{K_{a}}}$
$h = \sqrt{\frac{K_{w}}{K_{a} \cdot C}}$
$h = \sqrt{\frac{K_{a} \cdot C}{K_{w}}}$
$h = \sqrt{\frac{K_{a}}{K_{w} \cdot C}}$

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Q. Calculate the pH at the equivalence point in the titration of 25 mL of

0.10 M

formic acid with a

0.1 M N a O H

solution (given that

p K_{a}

of formic acid = 3.74).

l o g 0.1 = - 1

4.74
8.74
8.37
6.06

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H X

is a weak acid

(K_{a} = 10^{- 5}) .

It forms a salt

N a X

having concentration of

0.1 M

, on reacting with caustic soda. What is the degree of hydrolysis (

h

) of the salt?

$10^{- 4}$
$10^{- 2}$
$10^{- 6}$
$10^{- 5}$

View Solution

The degree of hydrolysis and pH of $0.1 M$ sodium acetate solution are:
Hydrolysis constant of sodium acetate is $5.6 \times 10^{- 10}$ .

$h$ = $7.5 \times 10^{- 7} M$ , $p H$ = $7.9$
$h$ = $8.5 \times 10^{- 6}$ , $p H$ = $6.9$
$h$ = $8.5 \times 10^{- 7}$ , $p H$ = $7.9$
$h$ = $7.5 \times 10^{- 6}$ , $p H$ = $7.9$

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Q. Calcium lactate is a salt of weak organic acid and is represented by

C a (L a c)_{2}

. A saturated solution of

C a (L a c)_{2}

contains 0.13 mol of this salt in 0.5 L solution. The pOH of this solution is 5.60. Assuming complete dissociation of the salt. Calculate

p K_{a}

of lactic acid.

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Q. On shaking

H_{2} O_{2}

with acidified potassium dichromate and ether, the ethereal layer becomes:

Black
Green
Red
Blue

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Q. Which of the following property of ammonia explains its basic nature?

Reaction with metal salts
All of the above
Reaction with acids
Complex formation

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