Chapter 18, Problem 18.145P

(a)

Interpretation Introduction

Interpretation:

The given ${\text{ Cu}}^{\text{2+}}{\text{+ 4Cl}}^{\text{- }}\underset{}{\rightleftharpoons }{\text{ CuCl}}_4^{2-}$ 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 ${\text{Al(OH)}}_{\text{3}}{\text{ + 3HNO}}_{\text{3}}\underset{}{\rightleftharpoons }{\text{ Al}}^{\text{3+}}{\text{+ 3H}}_{\text{2}}{\text{O + 3NO}}_3^{-}$ 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 ${\text{N}}_{\text{2}}{\text{ + 2H}}_{\text{2 }}\underset{}{\rightleftharpoons }{\text{ 2NH}}_{\text{3 }}$ 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 ${\text{H}}_{\text{2}}{\text{O + CN}}^{\text{-}}\underset{}{\rightleftharpoons }{\text{ HCN + OH}}^{\text{-}}$ 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.