Chapter 15, Problem 11PE

(a)

Interpretation Introduction

Interpretation:

Conjugate acid of ${\text{HSO}}_{\text{4}}{}^{-}$ has to be identified.

Concept Introduction:

Bronsted-Lowry acid outlined definition of acids as species 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;

(b)

Interpretation Introduction

Interpretation:

Conjugate base of ${\text{HSO}}_{\text{4}}{}^{-}$ has to be written.

Concept Introduction:

Refer to part (a).