Chapter 16, Problem 16.6QP

(a)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{HS}}^{\text{-}}$

To identify the conjugate acid

${\text{HS}}^{\text{-}}{\text{ + H}}^{\text{+}}\to {\text{ H}}_{\text{2}}\text{S}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(b)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{HCO}}_{\text{3}}{}^{-}$

To identify the conjugate acid

${\text{HCO}}_{\text{3}}{}^{-}{\text{ + H}}^{\text{+}}\to {\text{ H}}_{\text{2}}{\text{CO}}_{\text{3}}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(c)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{CO}}_{\text{3}}{}^{2-}$

To identify the conjugate acid

${\text{CO}}_{\text{3}}{}^{2-}{\text{ + H}}^{\text{+}}\to {\text{ HCO}}_{\text{3}}{}^{-}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(d)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{H}}_{\text{2}}{\text{PO}}_{\text{4}}{}^{-}$

To identify the conjugate acid

${\text{H}}_{\text{2}}{\text{PO}}_{\text{4}}{}^{-}{\text{ + H}}^{\text{+}}\to {\text{ H}}_3{\text{PO}}_{\text{4}}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(e)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{HPO}}_{\text{4}}{}^{2-}$

To identify the conjugate acid

${\text{HPO}}_{\text{4}}{}^{2-}{\text{ + H}}^{\text{+}}\to {\text{ H}}_{\text{2}}{\text{PO}}_{\text{4}}{}^{-}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(f)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{PO}}_{\text{4}}{}^{3-}$

To identify the conjugate acid

${\text{PO}}_{\text{4}}{}^{3-}{\text{ + H}}^{\text{+}}\to {\text{ HPO}}_{\text{4}}{}^{2-}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(g)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{HSO}}_{\text{4}}{}^{-}$

To identify the conjugate acid

${\text{HSO}}_{\text{4}}{}^{-}{\text{ + H}}^{\text{+}}\to {\text{ H}}_2{\text{SO}}_{\text{4}}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(h)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{SO}}_{\text{4}}{}^{2-}$

To identify the conjugate acid

${\text{SO}}_{\text{4}}{}^{2-}{\text{ + H}}^{\text{+}}\to {\text{ HSO}}_{\text{4}}{}^{-}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(i)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{NO}}_2{}^{\text{-}}$

To identify the conjugate acid

${\text{NO}}_2{}^{\text{-}}{\text{ + H}}^{\text{+}}\to {\text{ HNO}}_2$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.

(j)

Interpretation Introduction

Interpretation:

For the given set of bases, formula for conjugated acid has to be written.

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.

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

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

Bronsted base accepts a proton to give a protonated species known as conjugate acid and Bronsted acid loses a proton to give a deprotonated species is known as conjugate base.  When a proton is removed the resulting species will have a negative charge and when a proton is added the resulting species will have a positive charge.

Explanation of Solution

The conjugate acid of ${\text{SO}}_{\text{3}}{}^{\text{2-}}$

To identify the conjugate acid

${\text{SO}}_{\text{3}}{}^{\text{2-}}{\text{ + H}}^{\text{+}}\to {\text{ HSO}}_{\text{3}}{}^{\text{-}}$

Conjugate acid is formed when a proton is added to the Bronsted base.  The scheme for the formation of conjugate acid for the given base is shown above.