Chapter 23, Problem 101A

Interpretation Introduction

(a)

Interpretation:

In the following reaction, the reactants act as acid or base needs to be identified.

$\text{HBr}\text{+}{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Br}}^{-}$

Concept introduction:

According to Bronsted-Lowry model acids and bases, an acid is a hydrogen-ion donor. A base is a hydrogen-ion acceptor. Conjugate acid is the species which is formed when a hydrogen ion is accepted by a base and conjugate base is the species that results when acid donates a hydrogen ion.

Answer to Problem 101A

In the reaction, HBr acts as an acid and ${\text{H}}_{\text{2}}\text{O}$ acts as an base.

Explanation of Solution

The reaction given is as follows:

$\text{HBr}\text{+}{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Br}}^{-}$

Upon accepting the ${\text{H}}^{+}$ ion, the water molecule becomes an acid, ${\text{H}}_3{\text{O}}^{+}$. Upon donating its ${\text{H}}^{+}$, the acid HX becomes a base, ${\text{Br}}^{-}$.

$\begin{array}{l}\text{HBr}\text{+}{\text{H}}_2\text{O}\to {\text{H}}_3{\text{O}}^{+}+{\text{Br}}^{-}\\ \text{Acid }\text{Base Conjugate Conjugate}\\ \text{acid}\text{base}\end{array}$

(b)

Interpretation Introduction

Interpretation:

In the following reaction, the reactants act as acid or base needs to be identified.

${\text{NH}}_{\text{3}}+\text{HCOOH}\to {\text{NH}}_4{}^{+}+{\text{HCOO}}^{-}$

Concept introduction:

According to Bronsted-Lowry model acids and bases, an acid is a hydrogen-ion donor. A base is a hydrogen-ion acceptor. Conjugate acid is the species which is formed when a hydrogen ion is accepted by a base and conjugate base is the species that results when acid donates a hydrogen ion.

Answer to Problem 101A

${\text{NH}}_{\text{3}}$ is an acid and HCOOH is base.

Explanation of Solution

The reaction given is as follows:

${\text{NH}}_{\text{3}}+\text{HCOOH}\to {\text{NH}}_4{}^{+}+{\text{HCOO}}^{-}$

Upon accepting the ${\text{H}}^{+}$ ion, the ammonia molecule becomes an acid, ${\text{NH}}_4{}^{+}$. Upon donating its ${\text{H}}^{+}$, the acid HCOOH becomes a base, ${\text{HCOO}}^{-}$.

$\begin{array}{l}\text{HCOOH}+{\text{NH}}_{\text{3}}\to {\text{NH}}_4{}^{+}+{\text{HCOO}}^{-}\\ \text{Acid }\text{Base Conjugate Conjugate}\\ \text{acid}\text{base}\end{array}$

(c)

Interpretation Introduction

Interpretation:

In the following reaction, the reactants act as acid or base needs to be identified.

${\text{HCO}}_{\text{3}}{}^{-}+{\text{H}}_{\text{2}}\text{O}\to {\text{CO}}_3{}^{-}+{\text{H}}_{\text{3}}{\text{O}}^{+}$

Concept introduction:

According to Bronsted-Lowry model acids and bases, an acid is a hydrogen-ion donor. A base is a hydrogen-ion acceptor. Conjugate acid is the species which is formed when a hydrogen ion is accepted by a base and conjugate base is the species that results when acid donates a hydrogen ion.

Answer to Problem 101A

Water ( ${\text{H}}_{\text{2}}\text{O}$ ) is a base and ${\text{HCO}}_{\text{3}}{}^{-}$ is an acid.

Explanation of Solution

The reaction given is as follows:

${\text{HCO}}_{\text{3}}{}^{-}+{\text{H}}_{\text{2}}\text{O}\to {\text{CO}}_3{}^{-}+{\text{H}}_{\text{3}}{\text{O}}^{+}$

Upon accepting the ${\text{H}}^{+}$ ion, the water molecule becomes an acid, ${\text{H}}_3{\text{O}}^{+}$. Upon donating its ${\text{H}}^{+}$, the acid ${\text{HCO}}_{\text{3}}{}^{-}$ becomes a base, ${\text{CO}}_3{}^{-}$.

$\begin{array}{l}{\text{HCO}}_{\text{3}}{}^{-}+{\text{H}}_{\text{2}}\text{O}\to {\text{H}}_{\text{3}}{\text{O}}^{+}+{\text{CO}}_3{}^{-}\\ \text{Acid }\text{Base Conjugate Conjugate}\\ \text{acid}\text{base}\end{array}$