Chapter 15, Problem 15.105QE

(a)

Interpretation Introduction

Interpretation:

Whether the acid-base reaction between $\text{HCl}$ and ${\mathrm{NH}}_3$ follows the definitions of Arrhenius, Bronsted–Lowry, or Lewis or not has to be stated.

Concept Introduction:

As per the definition proposed by Arrhenius acid refers to the one which produces hydronium ions in aqueous solution, while the base produces ${\text{OH}}^{-}$ ions in aqueous solution. Examples of Arrhenius acids include $\text{HBr}$${\text{HNO}}_3$${\text{H}}_2{\text{SO}}_4$ while $\text{NaOH}$ and $\text{KOH}$ are Arrhenius bases. This theory, however, is only applicable to aqueous solutions.

An acid serves to accepts an electron-pair from another electron-rich species while a base donates electrons to another electron-deficient species in the reaction in accordance with Lewis definition. For instance of Lewis acids include ${\text{BF}}_3$ and ${\text{SO}}_3$.

The acid is a species involved in the release of a proton whereas a base is the one that accepts a ${\text{H}}^{+}$ 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.

(b)

Interpretation Introduction

Interpretation:

Whether the given acid-base reaction between ${\text{SO}}_{\text{2}}$ and $\text{NaOH}$ is as per the definitions of Arrhenius, Bronsted–Lowry, or Lewis or not has to be stated.

Concept Introduction:

Refer to part (a).