Chapter 6, Problem 6A.6E

(a)

Interpretation Introduction

Interpretation:

Bronsted acid and Bronsted base has to be identified in the reaction given below.

    ${\text{HSO}}_{\text{3}}{}^{-}(aq)+{\text{CH}}_{\text{3}}{\text{NH}}_{\text{3}}{}^{\text{+}}(aq)\to {\text{H}}_{\text{2}}{\text{SO}}_{\text{3}}(aq)+{\text{CH}}_{\text{3}}{\text{NH}}_{\text{2}}(aq)$

Concept Introduction:

Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base.  In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.

Generally acid donates proton to form conjugate base.  As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid.  Base accepts protons to form conjugate acid.  As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.

(b)

Interpretation Introduction

Interpretation:

Conjugate base and conjugate acid has to be identified in the reaction given below.

    ${\text{HSO}}_{\text{3}}{}^{-}(aq)+{\text{CH}}_{\text{3}}{\text{NH}}_{\text{3}}{}^{\text{+}}(aq)\to {\text{H}}_{\text{2}}{\text{SO}}_{\text{3}}(aq)+{\text{CH}}_{\text{3}}{\text{NH}}_{\text{2}}(aq)$

Concept Introduction:

Refer part (a).