Chapter 6, Problem 6A.3E

(a)

Interpretation Introduction

Interpretation:

Chemical equation for the proton transfer equilibrium of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ in aqueous solution has to be written and the conjugate acid‑base pair has to be identified.

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:

Chemical equation for the proton transfer equilibrium of ${\text{C}}_{\text{6}}{\text{H}}_{\text{5}}{\text{NH}}_{\text{3}}{}^{\text{+}}$ in aqueous solution has to be written and the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

(c)

Interpretation Introduction

Interpretation:

Chemical equation for the proton transfer equilibrium of ${\text{H}}_{\text{2}}{\text{PO}}_{\text{4}}{}^{-}$ in aqueous solution has to be written and the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

(d)

Interpretation Introduction

Interpretation:

Chemical equation for the proton transfer equilibrium of $\text{HCOOH}$ in aqueous solution has to be written and the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).

(e)

Interpretation Introduction

Interpretation:

Chemical equation for the proton transfer equilibrium of ${\text{NH}}_{\text{2}}{\text{NH}}_{\text{3}}{}^{\text{+}}$ in aqueous solution has to be written and the conjugate acid‑base pair has to be identified.

Concept Introduction:

Refer part (a).