Chapter 16, Problem 16.7QP

(a)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{CH}}_{\text{2}}\text{ClCOOH}$

To identify the conjugate base

${\text{CH}}_{\text{2}}\text{ClCOOH }\to {\text{ CH}}_{\text{2}}{\text{ClCOO}}^{\text{-}}+{\text{H}}^{\text{+}}$

The conjugate base is ${\text{CH}}_{\text{2}}{\text{ClCOO}}^{\text{-}}$

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

(b)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{HIO}}_{\text{4}}$

To identify the conjugate base

${\text{HIO}}_{\text{4}}\to {\text{ IO}}_{\text{4}}{}^{-}+{\text{H}}^{\text{+}}$

The conjugate base is ${\text{ IO}}_{\text{4}}{}^{-}$

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

(c)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}$

To identify the conjugate base

${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\to {\text{ H}}_2{\text{PO}}_{\text{4}}{}^{\text{-}}\text{+}{\text{H}}^{\text{+}}$

The conjugate base is ${\text{ H}}_2{\text{PO}}_{\text{4}}{}^{\text{-}}$

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

(d)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{H}}_2{\text{PO}}_{\text{4}}{}^{-}$

To identify the conjugate base

${\text{H}}_2{\text{PO}}_{\text{4}}{}^{-}\to {\text{ HPO}}_{\text{4}}{}^{2-}\text{+}{\text{H}}^{\text{+}}$

The conjugate base is ${\text{ HPO}}_{\text{4}}{}^{2-}$

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

(e)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{HPO}}_{\text{4}}{}^{2-}$

To identify the conjugate base

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

The conjugate base is ${\text{PO}}_{\text{4}}{}^{3-}$

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

(f)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$

To identify the conjugate base

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

The conjugate base is ${\text{HSO}}_{\text{4}}{}^{-}$

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

(g)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{ HSO}}_{\text{4}}{}^{-}$

To identify the conjugate base

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

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

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

(h)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of $\text{HCOOH}$

To identify the conjugate base

$\text{HCOOH }\to {\text{ HCOO}}^{-}\text{+}{\text{H}}^{\text{+}}$

The conjugate base of ${\text{HCOO}}^{-}$

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

(i)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{HSO}}_{\text{3}}{}^{-}$

To identify the conjugate base

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

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

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

(j)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{NH}}_{\text{4}}{}^{\text{+}}$

To identify the conjugate base

${\text{NH}}_{\text{4}}{}^{\text{+}}\to {\text{ NH}}_{\text{3}}+{\text{H}}^{\text{+}}$

The conjugate base is ${\text{ NH}}_{\text{3}}$

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

(k)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{H}}_{\text{2}}\text{S}$

To identify the conjugate base

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

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

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

(l)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of ${\text{HS}}^{\text{-}}$

To identify the conjugate base

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

The conjugate base of ${\text{S}}^{\text{2-}}$

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

(m)

Interpretation Introduction

Interpretation:

For the given set of acids, formula for conjugated base has to be written.

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.

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 base of $\text{HClO}$

To identify the conjugate base

$\text{HClO }\to {\text{ ClO}}^{\text{-}}\text{+}{\text{H}}^{\text{+}}$

The conjugate base of ${\text{ClO}}^{\text{-}}$

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