Chapter 8, Problem 110P

(a)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of aqueous solution of nitric acid and solid barium oxide needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

According to question, nitric acid reacts with solid barium oxide. The chemical equation can be represneted as follows:

${\text{2HNO}}_{\text{3}}\left(aq\right)+\text{BaO}\left(s\right)\to \text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}\left(aq\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

Since, all nitrates are soluble thus, $\text{Ba}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$ will be soluble in water.

The ionic equation can be represneted as follows:

${\text{2H}}^{+}\left(aq\right){\text{+2NO}}_3^{-}\left(aq\right)+\text{BaO}\left(s\right)\to {\text{Ba}}^{2+}\left(aq\right)+2{\text{NO}}_3^{-}\left(aq\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

Here, $2{\text{NO}}_3^{-}\left(aq\right)$ are on both sides of the reaction arrow thus, the net ionic equation can be represneted as follows:

${\text{2H}}^{+}\left(aq\right)+\text{BaO}\left(s\right)\to {\text{Ba}}^{2+}\left(aq\right)+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

Thus, the above equation is balanced net ionic equation.

(b)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of aqueous solution of calcium bicarbonate and hydrobromic acid needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The reaction between calcium bicarbonate and hydrobromic acid is represneted as follows:

${\text{Ca(HCO}}_{\text{3}}{\text{)}}_{\text{2}}\left(aq\right)+2\text{HBr}\left(aq\right)\to {\mathrm{CaBr}}_2\left(s\right)+2{\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}\left(aq\right)$

As per the solubility rule, all common chlorides, bromides, and iodides are soluble except ${\text{AgCl, Hg}}_{\text{2}}{\text{Cl}}_{\text{2}}{\text{, PbCl}}_{\text{2}}{\text{, AgBr, Hg}}_{\text{2}}{\text{Br}}_{\text{2}}{\text{, PbBr}}_{\text{2}}{\text{, AgI, Hg}}_{\text{2}}{\text{I}}_{\text{2}}{\text{, PbI}}_{\text{2}}$ thus, ${\mathrm{CaBr}}_2$ is insoluble in water. Also, all carbonates are insoluble except those of ammonium ion and Group 1A (the alkali metal) cations thus, hydrogen carbonate is soluble in water.

The above equation can be rewritten as follows:

${\text{Ca}}^{2+}\left(aq\right){\text{+2HCO}}_3^{-}\left(aq\right)+2{\text{H}}^{+}\left(aq\right){\text{+2Br}}^{-}\left(aq\right)\to {\mathrm{CaBr}}_2\left(s\right)+2{\text{H}}^{+}\left(aq\right)+2{\text{HCO}}_3^{-}\left(aq\right)$

Cancel the ions which are on both sides of the reaction arrow:

${\text{Ca}}^{2+}\left(aq\right)+2{\text{Br}}^{-}\left(aq\right)\to {\mathrm{CaBr}}_2\left(s\right)$

Therefore, the above reaction is balanced net ionic equation.

(c)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the burning of acetylene needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The equation for burning of acetylene is represented as follows:

${\text{C}}_{\text{2}}{\text{H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\to {\text{CO}}_{\text{2}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)$

The above reaction can be balanced as follows:

${\text{C}}_{\text{2}}{\text{H}}_{\text{2}}\left(g\right)+\frac{5}{2}{\text{O}}_{\text{2}}\left(g\right)\to 2{\text{CO}}_{\text{2}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)$

Or,

${\text{2C}}_{\text{2}}{\text{H}}_{\text{2}}\left(g\right)+5{\text{O}}_{\text{2}}\left(g\right)\to 4{\text{CO}}_{\text{2}}\left(g\right)+2{\text{H}}_{\text{2}}\text{O}\left(g\right)$

All the species are in gaseous state thus, ionic equation is not possible for the above reaction.

(d)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of aluminum sulfate and sodium hydroxide needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The equation for the above reaction is represneted as follows:

${\text{Al}}_{\text{2}}{\left({\text{SO}}_{\text{4}}\right)}_{\text{3}}\left(aq\right)+\text{NaOH}\left(aq\right)\to {\text{Na}}_{\text{2}}{\text{SO}}_4\left(s\right)+\text{Al}{\left(\text{OH}\right)}_{\text{3}}\left(s\right)$

As per the solubility rule, most sulfates are soluble except ${\text{CaSO}}_{\text{4}}{\text{ , SrSO}}_{\text{4}}{\text{ , BaSO}}_{\text{4}}{\text{ , PbSO}}_{\text{4}}$ thus, ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ is insoluble in water.

Also, all hydroxides are insoluble except those of ammonium ion and Group 1A (the alkali metal) cations. Thus, $\text{Al}{\left(\text{OH}\right)}_{\text{3}}$ is insoluble in water.

The ionic equation can be represented s follows:

${\text{2Al}}^{3+}\left(aq\right)+3{\text{SO}}_4^{2-}\left(aq\right)+{\text{Na}}^{+}\left(aq\right){\text{OH}}^{-}\left(aq\right)\to {\text{Na}}_{\text{2}}{\text{SO}}_4\left(s\right)+\text{Al}{\left(\text{OH}\right)}_{\text{3}}\left(s\right)$

Thus, the above reaction is balanced net ionic equation.

(e)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of solid zinc strips and dilute sulfuric acid needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The reaction is represneted as follows:

$\text{Zn}\left(s\right)+{\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}\left(aq\right)\to {\text{ZnSO}}_{\text{4}}\left(aq\right)+{\text{H}}_{\text{2}}\left(g\right)$

According to solubility rule, most sulfates are soluble except ${\text{CaSO}}_{\text{4}}{\text{ , SrSO}}_{\text{4}}{\text{ , BaSO}}_{\text{4}}{\text{ , PbSO}}_{\text{4}}$ thus, ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}$ is insoluble in water. Thus, ${\text{ZnSO}}_{\text{4}}$ is soluble in water. The above reaction will be:

$\text{Zn}\left(s\right)+2{\text{H}}^{+}\left(aq\right){\text{+SO}}_4^{2-}\left(aq\right)\to {\text{Zn}}^{2+}\left(aq\right){\text{+SO}}_4^{2-}\left(aq\right)+{\text{H}}_{\text{2}}\left(g\right)$

The balanced net ionic equation can be represented as follows:

$\text{Zn}\left(s\right)+2{\text{H}}^{+}\left(aq\right)\to {\text{Zn}}^{2+}\left(aq\right)+{\text{H}}_{\text{2}}\left(g\right)$

(f)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of aqueous solution of magnesium chloride and silver nitrate needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The equation for the given reaction is represneted as follows:

${\text{MgCl}}_{\text{2}}\left(aq\right)+2{\text{AgNO}}_{\text{3}}\left(aq\right)\to \text{Mg}{\left({\text{NO}}_{\text{3}}\right)}_2\left(aq\right)+2\text{AgCl}\left(s\right)$

According to the solubility rule, all nitrates are soluble thus, magnesium nitrate is soluble. Also, all common chlorides, bromides, and iodides are soluble except ${\text{AgCl, Hg}}_{\text{2}}{\text{Cl}}_{\text{2}}{\text{, PbCl}}_{\text{2}}{\text{, AgBr, Hg}}_{\text{2}}{\text{Br}}_{\text{2}}{\text{, PbBr}}_{\text{2}}{\text{, AgI, Hg}}_{\text{2}}{\text{I}}_{\text{2}}{\text{, PbI}}_{\text{2}}$ thus, $\text{AgCl}$ is insoluble in water.

The above equation can be converted into ionic equation as follows:

${\text{Mg}}^{2+}\left(aq\right){\text{+2Cl}}^{-}\left(aq\right)+2{\text{Ag}}^{+}\left(aq\right){\text{+2NO}}_3^{-}\left(aq\right)\to {\text{Mg}}^{2+}\left(aq\right)+{\text{2NO}}_3^{-}\left(aq\right)+2\text{AgCl}\left(s\right)$

For the above reaction, net ionic equation will be:

${\text{2Cl}}^{-}\left(aq\right)+2{\text{Ag}}^{+}\left(aq\right)\to 2\text{AgCl}\left(s\right)$

Thus, the above reaction is net balanced equation.

(g)

Interpretation Introduction

Interpretation: The balanced net ionic equation for the reaction of solid potassium and lithium nitrate needs to be determined.

Concept Introduction: The net ionic equation is defined as a balanced chemical equation in which reactants and products in aqueous state are represneted in ionic form. The net ionic equation does not involved the spectator ions (which are on both sides of the reaction arrow as they gets cancelled out).

Explanation of Solution

The chemical equation for the given reaction is represneted as follows:

$\text{K}\left(s\right)+{\text{LiNO}}_{\text{3}}\left(aq\right)\to {\text{KNO}}_{\text{3}}\left(aq\right)+\text{Li}\left(s\right)$

According to the solubility rule, all nitrates are soluble thus, potassium nitrate will be soluble in water.

The ionic equation can be represneted as follows:

$\text{K}\left(s\right)+{\text{Li}}^{+}\left(aq\right){\text{+NO}}_3^{-}\left(aq\right)\to {\text{K}}^{+}\left(aq\right){\text{+NO}}_3^{-}\left(aq\right)+\text{Li}\left(s\right)$

The net ionic equation will be:

$\text{K}\left(s\right)+{\text{Li}}^{+}\left(aq\right)\to {\text{K}}^{+}\left(aq\right)+\text{Li}\left(s\right)$