Chapter 8, Problem 8.39UKC

(a)

Interpretation Introduction

Interpretation:

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

The given equation is,

  ${\text{H}}_{\text{3}}{\text{PO}}_{\text{4}}\left(\text{aq}\right){\text{+CN}}^{\text{-}}\left(\text{aq}\right)\stackrel{}{\to }{\text{H}}_{\text{2}}{\text{PO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right)\text{+HCN}\left(\text{aq}\right)$

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,

  ${\text{Br}}^{\text{-}}\left(\text{aq}\right){\text{+HSO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right)\stackrel{}{\to }{\text{SO}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right)\text{+HBr}\left(\text{aq}\right)$

Concept Introduction:

Refer to part (a).