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Dissociation constants of $C H_{3} C O O H a n d N H_{4} O H$ are $1.8 \times 10^{- 5}$ each at $25^{o} C$ . The equilibrium constant for the reaction of $C H_{3} C O O H$ and $N H_{4} O H$ will be -

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Important Questions on Ionic Equilibrium

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

A weak acid is titrated with a weak base. Consider the following statements regarding the

pH

of the solution at the equivalence point:
(i)

pH

depends on the concentration of acid and base.
(ii)

pH

is independent of the concentration of acid and base
(iii)

pH

depends on the

{pK}_{a}

of acid and

{pK}_{b}

of base.
(iv)

pH

is independent of the

{pK}_{a}

of acid and

{pK}_{b}

of base.
The correct statements are:-

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Arrange the aqueous solutions of the following salts in the increasing order of their $pH$ .

$I . {CuSO}_{4} II . NaCN III . KCl$

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

In the hydrolysis of a salt of weak acid and weak base, the hydrolysis constant

K_{h}

is equal to

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

The

{pK}_{b}

of dimethylamine and

{pK}_{a}

of acetic acid are

3.27

and

4.77

respectively at

T (K) .

The correct option for the

pH

of dimethyl ammonium acetate solution is:

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

The

p H

of a

0.02 M

N H_{4} C l

solution will be [Given:

K_{b} (N H_{4} O H) = 10^{- 5}

and

\log 2 = 0.301

]

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Which of the following statements is correct?

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

50 mL

0.02 MNaOH

solution is mixed with

50 mL

0.06 M

acetic acid solution, the

pH

of the resulting solution is_________

(pKa

of acetic acid is

4.76, \log 5 = 0.70)

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

If the

pKa

of lactic acid is

5

, then the

pH

0.005 M

calcium lactate solution at

25 ° C

is __________

\times 10^{- 1}

(Nearest integer)

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Which of the following salts will give highest

p H

in water?

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Which among the following salt solutions is basic in nature?

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Given the

{pK}_{a}

of a weak acid

HA

4.60

and

{pK}_{b}

of a weak base

BOH

4.80,

then find the

pH

0.1 M

solution of the salt

BA,

formed from

HA

and

BOH .

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

The pH of 0.1 M aqueous solution of

N a C l, C H_{3} C O O N a a n d N H_{4} C l

will follow the order:

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

20 mL

0.1 M {NH}_{4} OH

is mixed with

40 mL

0.05 M HCl

. The

pH

of the mixture is nearest to:
(Given:

K_{b} ({NH}_{4} OH) = 1 \times 10^{- 5}, \log 2 = 0.30

\log 3 = 0.48, \log 5 = 0.69, \log 7 = 0.84

\log 11 = 1.04

)

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

The

pH

of ammonium phosphate solution, if

{pk}_{a}

of phosphoric acid and

{pk}_{b}

of ammonium hydroxide are

5.23

and

4.75

respectively, is

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Match the following

	List-I		List-II
(A)	$Aq .$ Solution of ${AlCl}_{3}$	(I)	Basic
(B)	$Aq .$ solution of ${CH}_{3} COONa$	(II)	Acidic
(C)	$Aq .$ solution of $KCl$	(III)	Highly conductive
(D)	${Al}_{2} O_{3}$	(IV)	Strongly basic
		(V)	Amphoteric

The correct match is

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

A soft drink was bottled with a partial pressure of

{CO}_{2}

of 3 bar over the liquid at room temperature. The partial pressure of

{CO}_{2}

over the solution approaches a value of 30 bar when

44 g

{CO}_{2}

is dissolved in

1 kg

of water at room temperature. The approximate

pH

of the soft drink is ___________

\times 10^{- 1}

.
(First dissociation constant of

H_{2} {CO}_{3} = 4.0 \times 10^{- 7}; \log 2 = 0.3;

density of the soft drink

= 1 g {mL}^{- 1}

)

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

The initial rate of hydrolysis of methyl acetate

(1 M)

by a weak acid

(HA, 1 M)

1 / 100^{th}

of that by a strong acid

(HX, 1 M)

, at

25 ° C

. The

K_{a}

HA

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

25^{o} C

, the ionization constant for anilinium hydroxide is

5.00 \times 10^{- 10}

. The hydrolysis constant of anilinium chloride is

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

Which of the following salts is the most basic in aqueous solution?

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>Hydrolysis of Salts and pH of their Solutions

{pK}_{a}

of a weak acid

(HA)

and

{pK}_{b}

of a weak base

(BOH)

are

3.2

and

3.4

respectively. The

pH

of their salt

(AB)

solution at

25^{o} C

Dissociation constants of CH3COOH and NH4OH are 1.8 × 10–5 each at 25oC . The equilibrium constant for the reaction of CH3COOH and NH4OH will be -

Important Questions on Ionic Equilibrium

Learn and Prepare for any exam you want !

Dissociation constants of $C H_{3} C O O H a n d N H_{4} O H$ are $1.8 \times 10^{- 5}$ each at $25^{o} C$ . The equilibrium constant for the reaction of $C H_{3} C O O H$ and $N H_{4} O H$ will be -