Chapter 15, Problem 15.28QE

(a)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate acid of ${\text{NH}}_3$ have to be determined.

Concept Introduction:

The acid is involved in the release of a proton whereas a base is involved in acceptance of an ${\text{H}}^{+}$ ion. ${\text{H}}_2\text{O}$ acts as Bronsted acid while ${\text{NH}}_3$ is a Bronsted base as per the Bronsted-Lowry theory. This model is a better description of acid-base reaction in any media; be it aqueous or gas phase.

Conjugate acid: The substance that donates as well as releases a proton in a chemical reaction of acid and base is called conjugate acid.

Bronsted–Lowry acid transfer a proton and form base as the other compound can accept a proton. This is called conjugate acid-base pair. In pair of conjugate acid and base, the acid form is protonated and the base form lost the proton.

Every base has conjugate acid. They are related by loss and gain of proton.

The expression for base and conjugate acid is as follows:

  $\text{Base}+\text{Proton}\rightleftharpoons \text{Conjugate acid}$

(b)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate acid of ${\text{HCO}}_3{}^{-}$ have to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate acid of ${\text{Br}}^{-}$ has to be determined

Concept Introduction:

Refer to part (a)