Chapter 15.1, Problem 15.2P

(a)

Interpretation Introduction

Interpretation:

Formula for conjugate acid of ${\text{HSO}}_4^{-}$ has to be written.

Concept Introduction:

Bronsted-Lowry acid outlined the definition of acids that donate ${\text{H}}^{+}$ or a proton while bases that accept ${\text{H}}^{+}$ or a proton. In accordance with Bronsted definition the most usual type of acid-base reaction involves lone pair of base that reaches out for an acidic proton. Once deprotonation has occurred species assumes a negative charge and is referred as conjugate base of acid and other species with a positive charge as a result of proton acceptance is termed conjugate acid of given base. For instance;

The strength of conjugate acid-base pairs is inversely related to each another; thus strong acid has a weak and strong base has weak conjugate counterparts and vice-versa.

(b)

Interpretation Introduction

Interpretation:

Formula for conjugate acid of ${\text{NH}}_{\text{3}}$ has to be written.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Formula for conjugate acid of ${\text{OH}}^{-}$ has to be written.

Concept Introduction:

Refer to part (a).