Chapter 8, Problem 8.40UKC

(a)

Interpretation Introduction

Interpretation:

The acid and conjugate acid in the reaction has to be labeled.

The given equation is,

  $\text{HF}\left(\text{g}\right){\text{+NH}}_{\text{3}}\left(\text{g}\right)\stackrel{}{\to }{\text{NH}}_{\text{4}}{}^{\text{+}}\left(\text{aq}\right){\text{+F}}^{\text{-}}\left(\text{aq}\right)$

Concept Introduction:

Bronsted-Lowry Acids:  A Bronsted-Lowry acid is proton donor and contains a hydrogen atom.  It may be a neutral molecule or may contain a net positive or negative charge.

Bronsted-Lowry Bases:  A Bronsted-Lowry base is a proton acceptor.  A base should contain a lone pair of electrons, which donates to form a new bond.  It can be neutral or can contain a negative charge.

Conjugate acid:  A conjugate acid is the product formed by a gain of a proton by a base.  The conjugate acid of the base B will be ${\text{HB}}^{\text{+}}\text{.}$

Conjugate base:  A conjugate base is the product formed by a loss of proton from an acid.  The conjugate base of the acid A will be ${\text{A}}^{\text{-}}\text{.}$

(b)

Interpretation Introduction

Interpretation:

The acid and conjugate acid of the reaction has to be labeled.

The given equation is,

  ${\text{Br}}^{\text{-}}\left(\text{aq}\right){\text{+H}}_{\text{2}}\text{O}\left(\text{l}\right)\stackrel{}{\to }\text{HBr}\left(\text{aq}\right){\text{+OH}}^{\text{-}}\left(\text{aq}\right)$

Concept Introduction:

Refer to part (a).