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Chemistry Part-I

Equilibrium

The ionization constant of acetic acid is 1.74 { 10 }^{ -5 }.

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 first ionization constant of

H_{2} S

9.1 \times 10^{- 8}

. Calculate the concentration of

H S^{-}

ion in its

0.1 M

solution. How will this concentration be affected if the solution is

0.1 M

H Cl

also? If the second dissociation constant of

H_{2} S

1.2 \times 10^{- 13}

, calculate the concentration of

S^{2 -}

under both conditions.

The ionization constant of acetic acid is

1.74 \times 10^{- 5}

. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its

p H

It has been found that the

p H

of a

0.01 M

solution of an organic acid is

4.15

. Calculate the concentration of the anion, the ionization constant of the acid and its

p K_{a}

View all question

Question

Medium

Solving time: 4 mins

The ionization constant of acetic acid is $1.74 \times 10^{- 5}$ . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its $p H$ .

Name: Video solution 1: [Solved] The ionization constant of acetic acid is 1.74×10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH. - Chemistry Part-I
Uploaded: 2023-01-25T10:52:15.000Z
Duration: 11 min
Description: Video solution 1: [Solved] The ionization constant of acetic acid is 1.74×10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH. - Chemistry Part-I

Views: 5,867 students

Updated on: Jan 25, 2023

Book:

Chemistry Part-I (NCERT)

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The ionization constant of acetic acid is

1.74 \times 10^{- 5}

. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its

p H

6 mins ago

Discuss this question LIVE

6 mins ago

Text solutionVerified

The dissociation equilibrium is

C H_{3} COO H ⇌ C H_{3} CO O^{-} + H^{+}

Let

α

be the degree of dissociation.

The equilibrium concentrations of

C H_{3} COO H, C H_{3} CO O^{-}

and

H^{+}

are

c (1 - α), c (α)

and

c (α)

respectively.

The equilibrium constant expression is

K_{c} = \frac{[ C H _{3} CO O ^{-} ] [ H ^{+} ]}{[ C H _{3} COO H ]}

K_{c} = \frac{( c α ) ( c α )}{c ( 1 - α )} \approx c α^{2}

α = \frac{K _{a}}{c} = \frac{1.74 \times 1 0 ^{- 5}}{0.05} = 1.865 \times 1 0^{- 2}

[C H_{3} C O^{-}] = [H^{+}] = c α = 0.05 \times 1.865 \times 1 0^{- 2} = 9.33 \times 1 0^{- 4} M

p H = - l o g [H^{+}] = - l o g (9.33 \times 1 0^{- 4}) = 3.03

The concentration of acetate ion and its pH are

9.33 \times 1 0^{- 4}

and

3.03

respectively.

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Practice more questions from Chemistry Part-I (NCERT)

The first ionization constant of

H_{2} S

9.1 \times 10^{- 8}

. Calculate the concentration of

H S^{-}

ion in its

0.1 M

solution. How will this concentration be affected if the solution is

0.1 M

H Cl

also? If the second dissociation constant of

H_{2} S

1.2 \times 10^{- 13}

, calculate the concentration of

S^{2 -}

under both conditions.

The ionization constant of acetic acid is

1.74 \times 10^{- 5}

. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its

p H

It has been found that the

p H

of a

0.01 M

solution of an organic acid is

4.15

. Calculate the concentration of the anion, the ionization constant of the acid and its

p K_{a}

View all

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Question Text	The ionization constant of acetic acid is $1.74 \times 10^{- 5}$ . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its $p H$ .
Updated On	Jan 25, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	75
Avg. Video Duration	11 min

The ionization constant of acetic acid is $1.74 \times 10^{- 5}$ . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its $p H$ .

Text solutionVerified

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The ionization constant of acetic acid is 1.74×10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

Text solutionVerified

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The ionization constant of acetic acid is $1.74 \times 10^{- 5}$ . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its $p H$ .