Chapter 4, Problem 4.101QP

Complete and balance each of the following molecular equations, including phase labels, if a reaction occurs. Then write the net ionic equation. If no reaction occurs, write NR after the arrow.

1. a Sr(OH)₂ + HC₂H₃O₂ →
2. b NH₄I + CsCl →
3. c NaNO₃ + CsCl →
4. d NH₄I + AgNO₃ →

Interpretation Introduction

Interpretation:

To predict if a chemical reaction can take place while mixing each of the given set of reagents.  If reaction is possible, the balanced molecular equation and net ionic equation has to be found for each reactions.

Concept introduction:

A chemical equation is the figurative representation of chemical reaction.  In a chemical equation the reactants are in the left side and the products are in the right side.  A balanced chemical equation serves as an easy tool for understanding a chemical reaction.  There are mainly three types of chemical equations, molecular equations, complete ionic equation and net ionic equation.

In molecular equations the reactants and products are represented as molecular substances, even though they exist as ions in solution phase.  The molecular equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ in solution phase is given below.

${\text{Ca(OH)}}_{\text{2(aq)}}{\text{+Na}}_{\text{2}}{\text{CO}}_{\text{3(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2NaOH}}_{\text{(aq)}}$

This equation is helpful in understanding the reactants and products involved in the reaction.

In complete ionic equations the electrolytes are represented as its ions.  Soluble compounds exist as ions in solution.  Complete ionic equation is helpful in understanding the reaction at ionic level.  The complete ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}$

The solid ${\text{CaCO}}_{\text{3}}$ is insoluble and it exist as solid in solution.

In net ionic equations the ions that are common in the reactant and product sides( Spectator ions) are cancelled.  These spectator ions are not participating in the chemical reactions.  The net ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.  As hydroxide ions and sodium ions are common in both the side it is neglected from the equation.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}\text{+}{\text{CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}$

Answer to Problem 4.101QP

The complete molecular equation

${\text{Sr(OH)}}_{\text{2(aq)}}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}\stackrel{}{\to }{\text{Sr(C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{\text{)}}_{\text{2(aq)}}{\text{ + 2H}}_{\text{2}}\text{O(l)}$

The net ionic equation

${\text{ HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}+{\text{OH}}^{\text{-}}{}_{\text{(aq)}}\stackrel{}{\to }{\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}{}_{\text{(aq)}}{\text{ + H}}_{\text{2}}\text{O(l)}$

Explanation of Solution

The molecular equation for the reaction between acetic acid and strontium hydroxide is given below.

${\text{Sr(OH)}}_{\text{2(aq)}}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}\stackrel{}{\to }{\text{Sr(C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{\text{)}}_{\text{2(aq)}}{\text{ + 2H}}_{\text{2}}\text{O(l)}$

In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction is given below.  Since acetic acid is a weak acid its ionization is not given in the equation.

${\text{Sr}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}\stackrel{}{\to }{\text{Sr}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2CH}}_{\text{3}}{\text{COO}}^{\text{-}}{}_{\text{(aq)}}{\text{ + 2H}}_{\text{2}}\text{O(l)}$

The ions common in the reactant and the product side are cancelled from the total ionic equation to get net ionic equation.

${\text{ 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}+{\text{2OH}}^{\text{-}}{}_{\text{(aq)}}\stackrel{}{\to }{\text{2CH}}_{\text{3}}{\text{COO}}^{\text{-}}{}_{\text{(aq)}}{\text{ + 2H}}_{\text{2}}\text{O(l)}$

The entire equation is divided by two,

${\text{ HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}+{\text{OH}}^{\text{-}}{}_{\text{(aq)}}\stackrel{}{\to }{\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}{}_{\text{(aq)}}{\text{ + H}}_{\text{2}}\text{O(l)}$

Interpretation Introduction

Interpretation:

To predict if a chemical reaction can take place while mixing each of the given set of reagents.  If reaction is possible, the balanced molecular equation and net ionic equation has to be found for each reactions.

Concept introduction:

A chemical equation is the figurative representation of chemical reaction.  In a chemical equation the reactants are in the left side and the products are in the right side.  A balanced chemical equation serves as an easy tool for understanding a chemical reaction.  There are mainly three types of chemical equations, molecular equations, complete ionic equation and net ionic equation.

In molecular equations the reactants and products are represented as molecular substances, even though they exist as ions in solution phase.  The molecular equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ in solution phase is given below.

${\text{Ca(OH)}}_{\text{2(aq)}}{\text{+Na}}_{\text{2}}{\text{CO}}_{\text{3(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2NaOH}}_{\text{(aq)}}$

This equation is helpful in understanding the reactants and products involved in the reaction.

In complete ionic equations the electrolytes are represented as its ions.  Soluble compounds exist as ions in solution.  Complete ionic equation is helpful in understanding the reaction at ionic level.  The complete ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}$

The solid ${\text{CaCO}}_{\text{3}}$ is insoluble and it exist as solid in solution.

In net ionic equations the ions that are common in the reactant and product sides( Spectator ions) are cancelled.  These spectator ions are not participating in the chemical reactions.  The net ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.  As hydroxide ions and sodium ions are common in both the side it is neglected from the equation.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}\text{+}{\text{CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}$

Answer to Problem 4.101QP

No reaction occurs

Explanation of Solution

When ammonium iodide and cesium chloride are mixed no reaction occurs.

${\text{NH}}_{\text{4}}{\text{I}}_{\text{(aq) }}{\text{+ CsCl}}_{\text{(aq)}}\stackrel{}{\to }\text{NR}$

Interpretation Introduction

Interpretation:

To predict if a chemical reaction can take place while mixing each of the given set of reagents.  If reaction is possible, the balanced molecular equation and net ionic equation has to be found for each reactions.

Concept introduction:

A chemical equation is the figurative representation of chemical reaction.  In a chemical equation the reactants are in the left side and the products are in the right side.  A balanced chemical equation serves as an easy tool for understanding a chemical reaction.  There are mainly three types of chemical equations, molecular equations, complete ionic equation and net ionic equation.

In molecular equations the reactants and products are represented as molecular substances, even though they exist as ions in solution phase.  The molecular equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ in solution phase is given below.

${\text{Ca(OH)}}_{\text{2(aq)}}{\text{+Na}}_{\text{2}}{\text{CO}}_{\text{3(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2NaOH}}_{\text{(aq)}}$

This equation is helpful in understanding the reactants and products involved in the reaction.

In complete ionic equations the electrolytes are represented as its ions.  Soluble compounds exist as ions in solution.  Complete ionic equation is helpful in understanding the reaction at ionic level.  The complete ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}$

The solid ${\text{CaCO}}_{\text{3}}$ is insoluble and it exist as solid in solution.

In net ionic equations the ions that are common in the reactant and product sides( Spectator ions) are cancelled.  These spectator ions are not participating in the chemical reactions.  The net ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.  As hydroxide ions and sodium ions are common in both the side it is neglected from the equation.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}\text{+}{\text{CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}$

Answer to Problem 4.101QP

No reaction occurs.

Explanation of Solution

When sodium nitrate and cesium chloride are mixed no reaction occurs.

${\text{NaNO}}_{\text{3(aq)}}+{\text{CsCl}}_{\text{(aq)}}\stackrel{}{\to }\text{NR}$

Interpretation Introduction

Interpretation:

To predict if a chemical reaction can take place while mixing each of the given set of reagents.  If reaction is possible, the balanced molecular equation and net ionic equation has to be found for each reactions.

Concept introduction:

A chemical equation is the figurative representation of chemical reaction.  In a chemical equation the reactants are in the left side and the products are in the right side.  A balanced chemical equation serves as an easy tool for understanding a chemical reaction.  There are mainly three types of chemical equations, molecular equations, complete ionic equation and net ionic equation.

In molecular equations the reactants and products are represented as molecular substances, even though they exist as ions in solution phase.  The molecular equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ in solution phase is given below.

${\text{Ca(OH)}}_{\text{2(aq)}}{\text{+Na}}_{\text{2}}{\text{CO}}_{\text{3(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2NaOH}}_{\text{(aq)}}$

This equation is helpful in understanding the reactants and products involved in the reaction.

In complete ionic equations the electrolytes are represented as its ions.  Soluble compounds exist as ions in solution.  Complete ionic equation is helpful in understanding the reaction at ionic level.  The complete ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}{\text{+2Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}$

The solid ${\text{CaCO}}_{\text{3}}$ is insoluble and it exist as solid in solution.

In net ionic equations the ions that are common in the reactant and product sides (Spectator ions) are cancelled.  These spectator ions are not participating in the chemical reactions.  The net ionic equation for the reaction between $\text{Ca}{\left(\text{OH}\right)}_{\text{2}}$ and ${\text{Na}}_{\text{2}}{\text{CO}}_{\text{3}}$ is given below.  As hydroxide ions and sodium ions are common in both the side it is neglected from the equation.

${\text{Ca}}^{\text{2+}}{}_{\text{(aq)}}\text{+}{\text{CO}}_{\text{3}}{{}^{\text{2-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{CaCO}}_{\text{3(s)}}$

Answer to Problem 4.101QP

The complete molecular equation

${\text{NH}}_{\text{4}}{\text{I}}_{\text{(aq)}}{\text{ + Ag(NO}}_{\text{3}}{\text{)}}_{\text{(aq)}}\stackrel{}{\to }{\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}{}_{\text{(aq)}}{\text{ + AgI}}_{\text{(s)}}$

The net ionic equation

${\text{ Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{ AgI}}_{\text{(s)}}$

Explanation of Solution

The complete molecular equation for the reaction between ammonium iodide and silver nitrate is given below.

${\text{NH}}_{\text{4}}{\text{I}}_{\text{(aq)}}{\text{ + Ag(NO}}_{\text{3}}{\text{)}}_{\text{(aq)}}\stackrel{}{\to }{\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}{}_{\text{(aq)}}{\text{ + AgI}}_{\text{(s)}}$

In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction is given below.

${\text{NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}{\text{+I}}^{\text{-}}{}_{\text{(aq)}}{\text{ + Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}{\text{ +NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}{\text{+ AgI}}_{\text{(s)}}$

The ions common in the reactant and the product side are cancelled from the total ionic equation to get net ionic equation.

${\text{ Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}\stackrel{}{\to }{\text{ AgI}}_{\text{(s)}}$