Chapter 15.1, Problem 15.1P

(a)

Interpretation Introduction

Interpretation:

The formula for the conjugate base of ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}$ 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. The acidic strength is known from the ability of acid to donate ${\text{H}}^{+}$ in an aqueous solution. Explicitly the acidity strength is quantified by the magnitude of a parameter called acid ionization constant. The strong acids tend to possess higher magnitudes of acid ionization constant or $K_{\text{a}}$.

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 to as the 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 example;

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

(b)

Interpretation Introduction

Interpretation:

Formula for conjugate base of ${\text{HNO}}_2$ has to be written.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Formula for conjugate base of ${\text{HC}}_2{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}$ has to be written.

Concept Introduction:

Refer to part (a).