Acids and bases can be thought of as chemical opposites (acids are proton donors, and bases are proton acceptors). Therefore, one might think that K a = 1/ K b . Why isn’t this the case? What is the relationship between K a and K b ? Prove it with a derivation.

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Interpretation Introduction Interpretation: The explanation is to be given for the expression K a ≠ 1 K b . The relation between K a and K b is to be given. This relation is to be derived. Concept introduction: A substance that donate proton is known as acid whereas the substance that accepts proton is known base. The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, K a . The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, K b . Explanation Explanation To determine : The reason that K a ≠ 1 K b and the relation between K a and K b . The value of K a and K b is only applicable for conjugate acid-base pair. And conjugate acid-base pair is temperature dependent. Hence, it is not correct to say that, K a = 1 K b The acid dissociation constant K a and base dissociation constant K b are used in case of conjugate-acid base pair only. A pair of substance that is related to each other by donating and accepting of a single proton is known as conjugate acid-base pair. This equilibrium constant are temperature dependent. The value of K a and K b is different at different temperature. Hence, it is not correct to say that, K a = 1 K b The relation between K a and K b is, K w = K a × K b The acid dissociation constant is known as K a whereas base dissociation constant is known as K b . The relation between K a and K b is, K w = K a × K b Where, K w is ion product constant. To derive : The relation between K a and K b . The relation between K a and K b is, K a ⋅ K b = K w A reaction representing conjugate acid base pair is, HA ( a q ) + H 2 O ( l ) ⇌ H 3 O + ( a q ) + A − ( a q ) The K a is the equilibrium constant for the above reaction where proton is removed from HA to form conjugate base A −

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Section

Answer 3

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Answer 4

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Answer 5

Interpretation Introduction

Interpretation: The explanation is to be given for the expression Ka≠1Kb .

The relation between Ka and Kb is to be given. This relation is to be derived.

Concept introduction: A substance that donate proton is known as acid whereas the substance that accepts proton is known base. The equilibrium constant for the dissociation reaction of a given acid is known as the acid dissociation constant and is denoted by the symbol, Ka . The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

Explanation of Solution

Explanation

To determine: The reason that Ka≠1Kb and the relation between Ka and Kb .

The value of Ka and Kb is only applicable for conjugate acid-base pair. And conjugate acid-base pair is temperature dependent. Hence, it is not correct to say that,

Ka=1Kb

The acid dissociation constant Ka and base dissociation constant Kb are used in case of conjugate-acid base pair only. A pair of substance that is related to each other by donating and accepting of a single proton is known as conjugate acid-base pair. This equilibrium constant are temperature dependent. The value of Ka and Kb is different at different temperature. Hence, it is not correct to say that,

Ka=1Kb

The relation between Ka and Kb is,

Kw=Ka×Kb

The acid dissociation constant is known as Ka whereas base dissociation constant is known as Kb . The relation between Ka and Kb is,

Kw=Ka×Kb

Where,

Kw is ion product constant.

To derive: The relation between Ka and Kb .

The relation between Ka and Kb is,

Ka⋅Kb=Kw

A reaction representing conjugate acid base pair is,

HA(aq)+H2O(l)⇌H3O+(aq)+A−(aq)

The Ka is the equilibrium constant for the above reaction where proton is removed from HA to form conjugate base A−

Acids and bases can be thought of as chemical opposites (acids are proton donors, and bases are proton acceptors). Therefore, one might think that K a = 1/ K b . Why isn’t this the case? What is the relationship between K a and K b ? Prove it with a derivation.

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach