Chapter 6, Problem 6A.12E

(a)

Interpretation Introduction

Interpretation:

The amphiprotic character of ${\text{H}}_{\text{2}}{\text{PO}}_{\text{3}}{}^{-}$ has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic.  This reacts with both acid and base.  Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.

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:

The amphiprotic character of ${\text{NH}}_{\text{3}}$ has to be demonstrated using chemical equations and also the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).