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Chemistry Part-I

Equilibrium

The ionization constant of nitrous acid is 4.5 { 10 }^{ -4 }.

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

The ionization constant of propanoic acid is

1.32 \times 10^{- 5}

. Calculate the degree of ionization of the acid in its 0.05 M solution and also its

p H

. What will be its degree of ionization if the solution is 0.01M in

H Cl

The ionization constant of nitrous acid is

4.5 \times 10^{- 4}

. Calculate the

p H

of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

A 0.02 M solution of pyridinium hydrochloride has

p H = 3.44

. Calculate the ionization constant of pyridine.

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Question

Medium

Solving time: 5 mins

The ionization constant of nitrous acid is $4.5 \times 10^{- 4}$ . Calculate the $p H$ of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

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Chemistry Part-I (NCERT)

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The ionization constant of nitrous acid is

4.5 \times 10^{- 4}

. Calculate the

p H

of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

5 mins ago

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Text solutionVerified

p K_{a} = - l o g K_{a} = - l o g (4.5 \times 1 0^{- 4}) = 3.35

p H = 0.5 p K_{w} + 0.5 p K_{a} + l o g c = 0.5 \times 14 + 0.5 \times 3.35 + l o g 0.04 = 7.285

K_{h} = \frac{K _{w}}{K _{a} c} = \frac{1 0 ^{- 14}}{4.5 \times 1 0 ^{- 4} \times 0.04} = 2.35 \times 1 0^{- 5}

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Practice more questions from Chemistry Part-I (NCERT)

The ionization constant of propanoic acid is

1.32 \times 10^{- 5}

. Calculate the degree of ionization of the acid in its 0.05 M solution and also its

p H

. What will be its degree of ionization if the solution is 0.01M in

H Cl

The ionization constant of nitrous acid is

4.5 \times 10^{- 4}

. Calculate the

p H

of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

A 0.02 M solution of pyridinium hydrochloride has

p H = 3.44

. Calculate the ionization constant of pyridine.

View all

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Question Text	The ionization constant of nitrous acid is $4.5 \times 10^{- 4}$ . Calculate the $p H$ of 0.04 M sodium nitrite solution and also its degree of hydrolysis.
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1
Upvotes	37

The ionization constant of nitrous acid is $4.5 \times 10^{- 4}$ . Calculate the $p H$ of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

Text solutionVerified

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The ionization constant of nitrous acid is 4.5×10−4. Calculate the pH of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

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The ionization constant of nitrous acid is $4.5 \times 10^{- 4}$ . Calculate the $p H$ of 0.04 M sodium nitrite solution and also its degree of hydrolysis.