Chapter 16, Problem 16.5QP

(a)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.

(b)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.

(c)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.

(d)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.

(e)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.

(f)

Interpretation Introduction

Interpretation:

In the given set of reactions acid-base conjugate pairs has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other.  In Bronsted's theory acid donates proton, while base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

$\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

When Bronsted base accepts a proton the protonated species is known as conjugate acid and when Bronsted acid loses a proton deprotonated species is known as conjugate base.  The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.

The acid-base conjugate pair for the given reaction.