Chapter 16.1, Problem 1PE

Interpretation Introduction

Interpretation:

The conjugate acid-base pairs for the given reaction has to be identified.

Concept Introduction:

Bronsted's definition is based on the chemical reaction that occurs when both acids and bases are added with each other. 

According to Bronsted's theory acid donates proton, whereas base accepts proton from acid resulting in the formation of water.

Example: Consider the following reaction.

  $\text{HCl}\text{+}{\text{NH}}_{\text{3}}\to {\text{NH}}_{\text{4}}{}^{\text{+}}\text{+}{\text{Cl}}^{\text{-}}$

Hydrogen chloride donates a proton, and hence it is a Bronsted acid.  Ammonia accepts a proton, and hence it is a Bronsted base.

Conjugate acid: When Bronsted base accepts a proton the protonated species is known as conjugate acid.

Conjugate base: When Bronsted acid loses a proton deprotonated species is known as conjugate base.

The conjugated acid-base pair is present in opposite side of the reaction.  In this the base has one proton less than the acid.