Chapter 8.3, Problem 8.13P

(a)

Interpretation Introduction

Interpretation:

The stronger acid and conjugate base in each pair $\left({\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}\text{(or)}{\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\right)$ has to be labeled.

Concept Introduction:

Bronsted-Lowry Acids:  A Bronsted-Lowry acid is a 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 ${\text{A}}^{\text{-}}\text{.}$

The stronger the acid, weaker will be its conjugate base.

(b)

Interpretation Introduction

Interpretation:

The stronger acid and conjugate base in each pair $\left(\text{HCl}\text{(or)}\text{HF}\right)$ has to be labeled.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The stronger acid and conjugate base in each pair $\left({\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(or)}{\text{NH}}_{\text{4}}{}^{\text{+}}\right)$ has to be labeled.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The stronger acid and conjugate base in each pair $\left(\text{HCN}\text{(or)}\text{HF}\right)$ has to be labeled.

Concept Introduction:

Refer to part (a).