Chapter 18, Problem 18.143P

(a)

Interpretation Introduction

Interpretation:

The given ${\text{ Ag}}^{\text{+}}{\text{+ 2NH}}_{\text{3}}\underset{}{\rightleftharpoons }{\text{ Ag(NH}}_{\text{3}}{\text{)}}_2^{+}$ reaction as Arrhenius, Brønsted - Lowry, or Lewis acid-base reactions has to be classified.

Concept introduction:

Arrhenius Acids and Bases:

Acid release hydrogen ion in water, Base release hydroxide ions in water.

$\begin{array}{l}\text{HCl(aq) }\to {\text{H}}^{\text{+}}{\text{(aq) + Cl}}^{\text{-}}\text{(aq)}\mathrm{.........}\text{Acid}\\ \text{NaOH(aq) }\to {\text{Na}}^{\text{+}}{\text{(aq)+ OH}}^{\text{-}}\text{(aq)}\mathrm{...........}\text{Base}\end{array}$

An acid is a substance that produces hydronium ions, ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion (${\text{H}}^{\text{+}}$), a Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion (${\text{H}}^{\text{+}}$).

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair. A Lewis base is a substance that can donate and share an electron pair.

(b)

Interpretation Introduction

Interpretation:

The given ${\text{ H}}_{\text{2}}{\text{SO}}_{\text{4}}{\text{ + NH}}_{\text{3}}\underset{}{\rightleftharpoons }{\text{ HSO}}_4^{-}{\text{ + NH}}_4^{+}$ reaction as Arrhenius, Brønsted - Lowry, or Lewis acid-base reactions has to be classified.

Concept introduction:

Arrhenius Acids and Bases:

Acid release hydrogen ion in water, Base release hydroxide ions in water.

$\begin{array}{l}\text{HCl(aq) }\to {\text{H}}^{\text{+}}{\text{(aq) + Cl}}^{\text{-}}\text{(aq)}\mathrm{.........}\text{Acid}\\ \text{NaOH(aq) }\to {\text{Na}}^{\text{+}}{\text{(aq)+ OH}}^{\text{-}}\text{(aq)}\mathrm{...........}\text{Base}\end{array}$

An acid is a substance that produces hydronium ions, ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion (${\text{H}}^{\text{+}}$), a Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion (${\text{H}}^{\text{+}}$).

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair. A Lewis base is a substance that can donate and share an electron pair.

(c)

Interpretation Introduction

Interpretation:

The given $\text{ 2HCl }\underset{}{\rightleftharpoons }{\text{ H}}_{\text{2}}{\text{ + Cl}}_{\text{2 }}$ reaction as Arrhenius, Brønsted - Lowry, or Lewis acid-base reactions has to be classified.

Concept introduction:

Arrhenius Acids and Bases:

Acid release hydrogen ion in water, Base release hydroxide ions in water.

$\begin{array}{l}\text{HCl(aq) }\to {\text{H}}^{\text{+}}{\text{(aq) + Cl}}^{\text{-}}\text{(aq)}\mathrm{.........}\text{Acid}\\ \text{NaOH(aq) }\to {\text{Na}}^{\text{+}}{\text{(aq)+ OH}}^{\text{-}}\text{(aq)}\mathrm{...........}\text{Base}\end{array}$

An acid is a substance that produces hydronium ions, ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion (${\text{H}}^{\text{+}}$), a Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion (${\text{H}}^{\text{+}}$).

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair. A Lewis base is a substance that can donate and share an electron pair.

(d)

Interpretation Introduction

Interpretation:

The given ${\text{AlCl}}_{\text{3}}{\text{ + Cl}}^{\text{-}}\underset{}{\rightleftharpoons }{\text{ AlCl}}_4^{-}$ reaction as Arrhenius, Brønsted - Lowry, or Lewis acid-base reactions has to be classified.

Concept introduction:

Arrhenius Acids and Bases:

Acid release hydrogen ion in water, Base release hydroxide ions in water.

$\begin{array}{l}\text{HCl(aq) }\to {\text{H}}^{\text{+}}{\text{(aq) + Cl}}^{\text{-}}\text{(aq)}\mathrm{.........}\text{Acid}\\ \text{NaOH(aq) }\to {\text{Na}}^{\text{+}}{\text{(aq)+ OH}}^{\text{-}}\text{(aq)}\mathrm{...........}\text{Base}\end{array}$

An acid is a substance that produces hydronium ions, ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion (${\text{H}}^{\text{+}}$), a Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion (${\text{H}}^{\text{+}}$).

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair. A Lewis base is a substance that can donate and share an electron pair.