Chapter 7, Problem 24CR

Write the balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed. If no reaction is likely, explain why no reaction would be expected for that combination of solutes.

l type='a'>

potassium nitrate and sodium chloride

calcium nitrate and sulfuric acid

ammonium sulfide and lead(II) nitrate

sodium carbonate and iron(III) chloride

mercurous nitrate and calcium chloride

silver acetate and potassium chloride

i>phosphoric acid and calcium nitrate

sulfuric acid and nickel(II) sulfate

Interpretation Introduction

(a)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

A net ionic equation is not available.

Explanation of Solution

When potassium nitrate and sodium chloride are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. But no change is visible as all the reactants and products are strong electrolytes, they are completely dissociated in the solution. All ions behave as spectator ions. When we write the complete ionic equation,

${\text{K}}^{+}{}_{(aq)}{\text{ + NO}}_3^{-}{}_{(aq)}{\text{ + Na}}^{+}{}_{(aq)}{\text{ + Cl}}^{-}{}_{(aq)}\to {\text{ K}}^{+}{}_{(aq)}+{\text{ Cl}}^{-}{}_{(aq)}{\text{ + Na}}^{+}{}_{(aq)}+{\text{ NO}}_3^{-}{}_{(aq)}$

All the ions in both sides are cancelled off each other. So there is no net ionic equation.

Interpretation Introduction

(b)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

A net ionic equation is not available.

Explanation of Solution

When calcium nitrate and sulfuric acid are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. But no change is visible as all the reactants and products are strong electrolytes, they are completely dissociated in the solution. All ions behave as spectator ions. When we write the complete ionic equation,

${\text{Ca}}^{2+}{}_{(aq)}{\text{ + 2 NO}}_3^{-}{}_{(aq)}{\text{ + 2 H}}^{+}{}_{(aq)}{\text{ + SO}}_4^{2-}{}_{(aq)}\to {\text{ Ca}}^{2+}{}_{(aq)}+{\text{ SO}}_4^{2-}{}_{(aq)}{\text{ + 2 H}}^{+}{}_{(aq)}+{\text{ 2 NO}}_3^{-}{}_{(aq)}$

All the ions in both sides are cancelled off each other. So there is no net ionic equation.

Interpretation Introduction

(c)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

${\text{Pb}}^{2+}{}_{(aq)}{\text{ + S}}^{2-}{}_{(aq)}\to {\text{ PbS}}_{(s)}$.

Explanation of Solution

When ammonium sulfide and lead (II) nitrate are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. Here a precipitation reaction takes place and PbS precipitate is formed. So this reaction is likely to happen. When the complete ionic equation is written,

${\text{2 NH}}_4^{+}{}_{(aq)}{\text{ + S}}^{2-}{}_{(aq)}{\text{ + Pb}}^{2+}{}_{(aq)}{\text{ + 2 NO}}_3^{-}{}_{(aq)}\to {\text{ 2 NH}}_4^{+}{}_{(aq)}+{\text{ 2 NO}}_3^{-}{}_{(aq)}{\text{ + PbS}}_{(s)}$

All the similar cations and anions in both sides are cancelled off and therefore the net ionic equation is

${\text{Pb}}^{2+}{}_{(aq)}{\text{ + S}}^{2-}{}_{(aq)}\to {\text{ PbS}}_{(s)}$.

Interpretation Introduction

(d)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

${\text{2 Fe}}^{3+}{}_{(aq)}{\text{ + 3 CO}}_3^{2-}{}_{(aq)}\to {\text{ Fe}}_2{({\text{CO}}_3)}_3{}_{(s)}$.

Explanation of Solution

When sodium carbonate and iron (III) chloride are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. Here a precipitation reaction takes place and Fe₂ (CO₃ )₃ precipitate is formed. So this reaction is likely to happen. When the complete ionic equation is written,

${\text{3 Na}}^{+}{}_{(aq)}{\text{ + 3 CO}}_3^{2-}{}_{(aq)}{\text{ + 2 Fe}}^{3+}{}_{(aq)}{\text{ + 3 Cl}}^{-}{}_{(aq)}\to {\text{ 3 Na}}^{+}{}_{(aq)}+{\text{ 3 Cl}}^{-}{}_{(aq)}{\text{ + Fe}}_2{({\text{CO}}_3)}_3{}_{(s)}$

All the similar cations and anions in both sides are cancelled off and therefore the net ionic equation is

${\text{2 Fe}}^{3+}{}_{(aq)}{\text{ + 3 CO}}_3^{2-}{}_{(aq)}\to {\text{ Fe}}_2{({\text{CO}}_3)}_3{}_{(s)}$.

Interpretation Introduction

(e)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

${\text{Hg}}_2^{2+}{}_{(aq)}\text{ + }2{\text{ Cl}}^{-}{}_{(aq)}\to {\text{ Hg}}_2{\text{Cl}}_{2(s)}$.

Explanation of Solution

When mercurous nitrate and calcium chloride are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. Here a precipitation reaction takes place and Hg₂ Cl₂ precipitate is formed. So this reaction is likely to happen. When the complete ionic equation is written,

${\text{Ca}}^{2+}{}_{(aq)}+2{\text{ Cl}}^{-}{}_{(aq)}+{\text{ Hg}}_2^{2+}{}_{(aq)}+2{\text{ NO}}_3^{-}\to {\text{ Hg}}_2{\text{Cl}}_{2(s)}+{\text{ Ca}}^{2+}{}_{(aq)}+2{\text{ NO}}_3^{-}{}_{(aq)}$

All the similar cations and anions in both sides are cancelled off and therefore the net ionic equation is

${\text{Hg}}_2^{2+}{}_{(aq)}\text{ + }2{\text{ Cl}}^{-}{}_{(aq)}\to {\text{ Hg}}_2{\text{Cl}}_{2(s)}$.

Interpretation Introduction

(f)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

${\text{Ag}}^{+}{}_{(aq)}{\text{ + Cl}}^{-}{}_{(aq)}\to {\text{ AgCl}}_{(s)}$.

Explanation of Solution

When silver acetate and potassium chloride are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. Here a precipitation reaction takes place and AgCl precipitate is formed. So this reaction is likely to happen. When the complete ionic equation is written,

$\text{A}{\text{g}}^{+}{}_{(aq)}+{\text{ CH}}_3{\text{COO}}^{-}{}_{(aq)}+{\text{ K}}^{+}{}_{(aq)}+{\text{ Cl}}^{-}{}_{(aq)}\to {\text{ AgCl}}_{(s)}+{\text{ K}}^{+}{}_{(aq)}+{\text{ CH}}_3{\text{COO}}^{-}{}_{(aq)}$

All the similar cations and anions in both sides are cancelled off and therefore the net ionic equation is

${\text{Ag}}^{+}{}_{(aq)}{\text{ + Cl}}^{-}{}_{(aq)}\to {\text{ AgCl}}_{(s)}$.

Interpretation Introduction

(g)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

${\text{3 Ca}}^{2+}{}_{(aq)}{\text{ + 2 PO}}_4^{3-}{}_{(aq)}\to {\text{ Ca}}_3{{\text{(PO}}_4)}_2{}_{(s)}$.

Explanation of Solution

When phosphoric acid and calcium nitrate are mixed, double displacement reaction happens where the two cations of the reactants simply exchange their anions. Here a precipitation reaction takes place and Ca₃ (PO₄ )₂ precipitate is formed. So this reaction is likely to happen. When the complete ionic equation is written,

${\text{6 H}}^{+}{}_{(aq)}+{\text{ 2 PO}}_4^{3-}{}_{(aq)}+{\text{ 3 Ca}}^{2+}{}_{(aq)}+{\text{ 6 NO}}_3^{-}{}_{(aq)}\to {\text{ Ca}}_3{({\text{PO}}_4)}_2{}_{(s)}+{\text{ 6 H}}^{+}{}_{(aq)}+{\text{ 6 NO}}_3^{-}{}_{(aq)}$

All the similar cations and anions in both sides are cancelled off and therefore the net ionic equation is

${\text{3 Ca}}^{2+}{}_{(aq)}{\text{ + 2 PO}}_4^{3-}{}_{(aq)}\to {\text{ Ca}}_3{{\text{(PO}}_4)}_2{}_{(s)}$.

Interpretation Introduction

(h)

Interpretation:

The balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed should be written. If no reaction is likely, why no reaction would be expected for that combination of solute should be explained.

Concept Introduction:

Deciding which products will form when two or more reactants added together is not an easy task without any experimental evidences. The best way to predict what products will form is to think of various possibilities and then decide which product is most likely to form. A solid compound must have a zero charge.

In a complete ionic equation, all strong electrolytes are represented as ions. But in net ionic equation, only the components which undergo a chemical change are shown. Ions which do not participate directly in the reaction which are called spectator ions are not shown in the net ionic equation.

Answer to Problem 24CR

A net ionic equation is not available.

Explanation of Solution

Both sulfuric acid and nickel (II) sulfate has similar anion SO₄ ^2-. Therefore, even though they exchange their anions, a chemical change will not happen. So this reaction is not likely to happen. The complete ionic equation is,

${\text{2 H}}^{+}{}_{(aq)}{\text{ + SO}}_4^{2-}{}_{(aq)}{\text{ + Ni}}^{2+}{}_{(aq)}{\text{ + SO}}_4^{2-}{}_{(aq)}\to {\text{ 2 H}}^{+}{}_{(aq)}{\text{ + SO}}_4^{2-}{}_{(aq)}{\text{ + Ni}}^{2+}{}_{(aq)}{\text{ + SO}}_4^{2-}{}_{(aq)}$

All the cations and anions cancel off each other so no net ionic equation is available.