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Chemistry Part-I

Equilibrium

The ionization constant of phenol is 1.0 { 10 }^{ -10 }. What

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

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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

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Chapter 7: Equilibrium

101 questions

The ionization constant of

H F, H COO H

and

H CN

at 298K are

6.8 \times 10^{- 4}, 1.8 \times 10^{- 4}

and

4.8 \times 10^{- 9}

respectively. Calculate the ioniation constants of the corresponding conjugate base.

The ionization constant of phenol is

1.0 \times 10^{- 10}

. What is the concentration of phenolate ion in

0.05 M

solution of phenol? What will be its degree of ionization if the solution is also

0.01 M

in sodium phenolate?

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.

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Question

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Solving time: 3 mins

The ionization constant of phenol is $1.0 \times 10^{- 10}$ . What is the concentration of phenolate ion in $0.05 M$ solution of phenol? What will be its degree of ionization if the solution is also $0.01 M$ in sodium phenolate?

Views: 6,689 students

Updated on: Aug 24, 2023

Book:

Chemistry Part-I (NCERT)

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Harper Discussed

The ionization constant of phenol is

1.0 \times 10^{- 10}

. What is the concentration of phenolate ion in

0.05 M

solution of phenol? What will be its degree of ionization if the solution is also

0.01 M

in sodium phenolate?

9 mins ago

Discuss this question LIVE

9 mins ago

Text solutionVerified

The balanced chemical equation for the ionization of phenol is:

P h O H + H_{2} O ⇌ P h O^{-} + H_{3} O^{+}

The initial concentrations of phenol, phenoxide ion and hydronium ion are 0.05, 0 and 0 respectively.
Corresponding equilibrium concentrations are

0.05 - x,

x and x respectively.

K_{a} = \frac{[ P h O ^{-} ] [ H _{3} O ^{+} ]}{[ P h O H ]}

1 \times 1 0^{- 10} = \frac{x \times x}{0.05 - x}

x is very small (as the ionization constant is very small) . Hence, x can be ignored in the denominator.

1 \times 1 0^{- 10} = \frac{x \times x}{0.05}

x = 2.2 \times 1 0^{- 6} M = [H_{3} O^{+}] = [P h O^{-}]

Let

α

be the degree of dissociation of phenol in presence of 0.01 M phenoxide.

The dissociation of phenoxide is as represented:

P h ON a \to P h O^{-} + N a^{+}

Also,

P h O H + H_{2} O ⇌ P h O^{-} + H_{3} O^{+}

[P h O H] = 0.05 - 0.05 α ≃ 0.05

M (as the degree of dissociation is very small.)

[P h O^{-}] = 0.01 + 0.05 α ≃ 0.01

[H_{3} O^{+}] = 0.05 α

K_{a} = \frac{[ P h O ^{-} ] [ H _{3} O ^{+} ]}{[ P h O H ]}

1.0 \times 1 0^{- 10} = \frac{0.01 \times 0.05 α}{0.05}

α = 1 \times 1 0^{- 8}

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Practice more questions from Chemistry Part-I (NCERT)

The ionization constant of

H F, H COO H

and

H CN

at 298K are

6.8 \times 10^{- 4}, 1.8 \times 10^{- 4}

and

4.8 \times 10^{- 9}

respectively. Calculate the ioniation constants of the corresponding conjugate base.

The ionization constant of phenol is

1.0 \times 10^{- 10}

. What is the concentration of phenolate ion in

0.05 M

solution of phenol? What will be its degree of ionization if the solution is also

0.01 M

in sodium phenolate?

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.

View all

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Question Text	The ionization constant of phenol is $1.0 \times 10^{- 10}$ . What is the concentration of phenolate ion in $0.05 M$ solution of phenol? What will be its degree of ionization if the solution is also $0.01 M$ in sodium phenolate?
Updated On	Aug 24, 2023
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 3
Upvotes	311
Avg. Video Duration	7 min

The ionization constant of phenol is $1.0 \times 10^{- 10}$ . What is the concentration of phenolate ion in $0.05 M$ solution of phenol? What will be its degree of ionization if the solution is also $0.01 M$ in sodium phenolate?

Text solutionVerified

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The ionization constant of phenol is 1.0×10−10. What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01 M in sodium phenolate?

Text solutionVerified

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The ionization constant of phenol is $1.0 \times 10^{- 10}$ . What is the concentration of phenolate ion in $0.05 M$ solution of phenol? What will be its degree of ionization if the solution is also $0.01 M$ in sodium phenolate?