Chapter 15, Problem 15.25QE

(a)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate base of $\text{HCN}$ 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 base: The substance that is left over after an acid donates a proton in a chemical reaction of acid and base is called conjugate base.

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 acid has a conjugate base. They are related by loss or gain of proton.

The expression for conjugate base and acid is as follows:

  $\text{Acid}\rightleftharpoons \text{Proton}+\text{Conjugate base}$

(b)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate base of ${\text{HSO}}_4{}^{-}$ have to be determined.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate base of ${\text{H}}_2{\text{PO}}_3{}^{-}$ have to be determined.

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The formula and name of the conjugate base of hydrogen chloride have to be determined

Concept Introduction:

Refer to part (a).