Chapter 5, Problem 112QP

(a)

Interpretation Introduction

Interpretation:

The balanced molecular and net ionic equations for the reaction of ammonium carbonate with chromium (III) chloride.

Explanation of Solution

Ammonium nitrate and chromium chloride are electrolytes that react to produce chromium (III) carbonate and ammonium chloride.Chromium ion in a solution reacts with carbonate ion to form chromium (III) carbonate, which is insoluble in an aqueous solution. The given reaction is an example of a precipitation reaction. The balanced molecular equation is as follows:

${\text{3(NH}}_{\text{4}}{\text{)}}_{\text{2}}{\text{CO}}_{\text{3}}(aq)+2{\text{CrCl}}_{\text{3}}(aq)\to {\text{Cr}}_{\text{2}}{{\text{(CO}}_{\text{3}}\text{)}}_{\text{3}}(s)+6{\text{NH}}_{\text{4}}\text{Cl}(aq)$

Except for chromium (III) carbonate, all other substances are electrolytes. Therefore, the balanced ionic equation of the given reaction is as follows:

$6{\text{NH}}_4^{+}(aq)+3{\text{CO}}_3^{2-}(aq)+2{\text{Cr}}^{3+}(aq)+6{\text{Cl}}^{-}(aq)\to {\text{Cr}}_{\text{2}}{{\text{(CO}}_{\text{3}}\text{)}}_{\text{3}}(s)+6{\text{NH}}_4^{+}(aq)+6{\text{Cl}}^{-}(aq)$

As ammonium and chloride ionsare spectator ions, the net ionic equation is as follows:

$3{\text{CO}}_3^{2-}(aq)+2{\text{Cr}}^{3+}(aq)\to {\text{Cr}}_{\text{2}}{{\text{(CO}}_{\text{3}}\text{)}}_{\text{3}}(s)$

(b)

Interpretation Introduction

Interpretation:

The balanced molecular and net ionic equations for the reaction of barium hydroxide with hydrochloric acid in an aqueous solution.

Explanation of Solution

The reaction of barium hydroxide with hydrochloric acid is an example of an acid-base neutralization reaction.The products of the given reaction are barium chloride and molecular water. The balanced molecular equation is as follows:

${\text{Ba(OH)}}_{\text{2}}(aq)+2\text{HCl}(aq)\to {\text{BaCl}}_{\text{2}}^{}(aq)+2{\text{H}}_{\text{2}}\text{O}(l)$

Except for water, all other substances are electrolytes. The ionic equation is written as follows:

${\text{Ba}}^{2+}(aq)+2{\text{OH}}^{-}(aq)+2{\text{H}}^{+}(aq)+2{\text{Cl}}^{-}(aq)\to {\text{Ba}}^{2+}(aq)+2{\text{Cl}}^{-}(aq)+2{\text{H}}_{\text{2}}\text{O}(l)$

As barium and chloride ions are spectator ions, the net ionic equation can be written as:

${\text{OH}}^{-}(aq)+{\text{H}}^{+}(aq)\to {\text{H}}_{\text{2}}\text{O}(l)$

(c)

Interpretation Introduction

Interpretation:

The balanced molecular and net ionic equations for the reaction of iron (III) chloride with sodium hydroxide in an aqueous solution.

Explanation of Solution

Iron (III) chloride reacts with sodium hydroxide to produce a precipitate of iron (III) hydroxide. The balanced molecular equation is as follows:

${\text{FeCl}}_{\text{3}}(aq)+3\text{NaOH}(aq)\to {\text{Fe(OH)}}_{\text{3}}^{}(s)+3\text{NaCl}(aq)$

Except for ferric hydroxide, all other substances are electrolytes. The balanced ionic equation of the given reaction is as follows:

${\text{Fe}}^{3+}(aq)+3{\text{Cl}}^{-}(aq)+3{\text{Na}}^{+}(aq)+{\text{3OH}}^{-}(aq)\to {\text{Fe(OH)}}_{\text{3}}^{}(s)+3{\text{Cl}}^{-}(aq)+3{\text{Na}}^{+}(aq)$

As sodium and chloride ionsare spectator ions, the net ionic equation is as follows:

${\text{Fe}}^{3+}(aq)+{\text{3OH}}^{-}(aq)\to {\text{Fe(OH)}}_{\text{3}}^{}(s)$

(d)

Interpretation Introduction

Interpretation:

The balanced molecular and net ionic equations for the reaction of calcium bicarbonate with nitric acid.

Explanation of Solution

The reaction of calcium bicarbonate with nitric acid is an example of an acid-base neutralization reaction. The products of the given reaction are calcium nitrate and carbonic acid which further decomposes to water and carbon dioxide. The balanced molecular equation is as follows:

${\text{Ca(HCO}}_3{)}_2(aq)+2{\text{HNO}}_{\text{3}}(aq)\to {\text{Ca(NO}}_{\text{3}}{\text{)}}_2(aq)+2{\text{H}}_{\text{2}}\text{O}(l)+2{\text{CO}}_2(g)$

The balanced ionic equation of the given reaction is as follows:

${\text{Ca}}^{2+}(aq)+2{\text{HCO}}_3^{-}(aq)+{\text{2H}}^{+}(aq)+2{\text{NO}}_3^{-}(aq)\to {\text{Ca}}^{2+}(aq)+2{\text{NO}}_3^{-}(aq)+2{\text{H}}_{\text{2}}\text{O}(l)+2{\text{CO}}_2(g)$

As calcium and nitrate ionsare spectator ions, the net ionic equation is as follows:

$2{\text{HCO}}_3^{-}(aq)+{\text{2H}}^{+}(aq)\to 2{\text{H}}_{\text{2}}\text{O}(l)+2{\text{CO}}_2(g)$