Chapter 8, Problem 8.36UKC

(a)

Interpretation Introduction

Interpretation:

The acid, base, conjugate acid and conjugate base of the reaction has to be labeled.

The given equation is,

  ${\text{H}}_{\text{2}}{\text{Z+H}}_{\text{2}}\text{O}\stackrel{}{\to }{\text{HZ}}^{\text{-}}{\text{+H}}_{\text{3}}{\text{O}}^{\text{+}}$

Concept Introduction:

Bronsted-Lowry Acids:  A Bronsted-Lowry acid is proton donor and contains a hydrogen atom.  It may be a neutral molecule or may contain a net positive or negative charge.

Bronsted-Lowry Bases:  A Bronsted-Lowry base is a proton acceptor.  A base should contain a lone pair of electrons, which donates to form a new bond.  It can be neutral or can contain a negative charge.

Conjugate acid:  A conjugate acid is the product formed by a gain of a proton by a base.  The conjugate acid of the base B will be ${\text{HB}}^{\text{+}}\text{.}$

Conjugate base:  A conjugate base is the product formed by a loss of proton from an acid.  The conjugate base of the acid A will be ${\text{A}}^{\text{-}}\text{.}$

Answer to Problem 8.36UKC

  $\begin{array}{l}{\text{H}}_{\text{2}}\text{Z}\text{+}{\text{H}}_{\text{2}}\text{O}\stackrel{}{\to }{\text{HZ}}^{\text{-}}\text{+}{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Acid}\text{Base}\text{Conjugate}\text{Conjugate}\\ \text{base}\text{acid}\end{array}$

Explanation of Solution

Acid loses a proton and forms a conjugate base.

Base gains a proton and forms a conjugate acid.

The given reaction is,

  ${\text{H}}_{\text{2}}{\text{Z+H}}_{\text{2}}\text{O}\stackrel{}{\to }{\text{HZ}}^{\text{-}}{\text{+H}}_{\text{3}}{\text{O}}^{\text{+}}$

A proton is lost by ${\text{H}}_{\text{2}}\text{Z}$ and becomes ${\text{HZ}}^{\text{-}}\text{.}$  Water gains a proton and becomes ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\text{.}$

  $\begin{array}{l}{\text{H}}_{\text{2}}\text{Z}\text{+}{\text{H}}_{\text{2}}\text{O}\stackrel{}{\to }{\text{HZ}}^{\text{-}}\text{+}{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\\ \text{Acid}\text{Base}\text{Conjugate}\text{Conjugate}\\ \text{base}\text{acid}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The acid, base, conjugate acid and conjugate base of the reaction has to be labeled.

The given equation is,

  ${\text{HZ}}^{\text{-}}{\text{+OH}}^{\text{-}}\stackrel{}{\to }{\text{Z}}^{\text{2-}}{\text{+H}}_{\text{2}}\text{O}$

Concept Introduction:

Refer to part (a).

Answer to Problem 8.36UKC

  $\begin{array}{l}{\text{HZ}}^{\text{-}}{\text{+OH}}^{\text{-}}\stackrel{}{\to }{\text{Z}}^{\text{2-}}\text{+}{\text{H}}_{\text{2}}\text{O}\\ \text{Acid}\text{ Base}\text{Conjugate}\text{Conjugate}\\ \text{Base}\text{Acid}\end{array}$

Explanation of Solution

The given reaction is,

  ${\text{HZ}}^{\text{-}}{\text{+OH}}^{\text{-}}\stackrel{}{\to }{\text{Z}}^{\text{2-}}{\text{+H}}_{\text{2}}\text{O}$

A proton is lost by ${\text{HZ}}^{\text{-}}$ and becomes ${\text{Z}}^{\text{2-}}\text{.}$  Hydroxide ion gains a proton and becomes ${\text{H}}_2\text{O}\text{.}$

  $\begin{array}{l}{\text{HZ}}^{\text{-}}{\text{+OH}}^{\text{-}}\stackrel{}{\to }{\text{Z}}^{\text{2-}}\text{+}{\text{H}}_{\text{2}}\text{O}\\ \text{Acid}\text{ Base}\text{Conjugate}\text{Conjugate}\\ \text{Base}\text{Acid}\end{array}$