Chapter 9, Problem 9.35QP

(a)

Interpretation Introduction

Interpretation:

The balanced and ionic and net ionic equations for given reactions are should be written.

Concept introduction:

Balanced equation:

• The balanced equation is nothing but the all ionic compounds are represented as neutral compounds using the molecular formula.
• In the balanced equation, the number of atoms for each element and total charge are equal in the reaction for in both reactants and the products sides.

Ionic equation:

• In the ionic reactions, all the species present in reaction are written with respective charges is called ionic equation.

Net ionic equation:

• The removal of common ions forms ionic equation to give net ionic equation.
• To write the balanced and ionic and net ionic equations for given reaction.

Answer to Problem 9.35QP

• The balanced and ionic and net ionic equations for given reactions are,

The balanced equation is,

${\text{HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{ + KOH}}_{\text{(aq)}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{+H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

The ionic equation is,

${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{}^{\text{-}}{\text{ + K}}^{\text{+}}{\text{+OH}}^{-}{}_{\text{(aq)}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{+H}}^{\text{+}}{}_{\text{(aq)}}+{\text{OH}}^{-}{}_{\text{(aq)}}$

The net ionic equation is,

${\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{}^{\text{-}}{\text{ + K}}^{\text{+}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}$

Explanation of Solution

• The ionic compounds are dissolved in water to produced ions these ions are combined to give new product.
• The reaction is represent by the complex molecular formula means it is a balanced equation and it have equal number of atoms in both reactant and product sides.
• The ${\text{HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}$ and ${\text{KOH}}_{\text{(aq)}}$ are react to give the ${\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}$ so the balanced equation for this reaction is,

  ${\text{HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{ + KOH}}_{\text{(aq)}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{+H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

• The all the species present in above equation is writing with respective charges to give ionic reaction.

  ${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{}^{\text{-}}{\text{ + K}}^{\text{+}}{\text{+OH}}^{-}{}_{\text{(aq)}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{\text{+H}}^{\text{+}}{}_{\text{(aq)}}+{\text{OH}}^{-}{}_{\text{(aq)}}$

• The removal of common ions from the above equations to give net ionic equations.

  ${\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}{}^{\text{-}}{\text{ + K}}^{\text{+}}\to {\text{KC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2(aq)}}$

(b)

Interpretation Introduction

Interpretation:

The balanced and ionic and net ionic equations for given reactions are should be written.

Concept introduction:

Balanced equation:

• The balanced equation is nothing but the all ionic compounds are represented as neutral compounds using the molecular formula.
• In the balanced equation, the number of atoms for each element and total charge are equal in the reaction for in both reactants and the products sides.

Ionic equation:

• In the ionic reactions, all the species present in reaction are written with respective charges is called ionic equation.

Net ionic equation:

• The removal of common ions forms ionic equation to give net ionic equation.
• To write the balanced and ionic and net ionic equations for given reaction.

Answer to Problem 9.35QP

• The balanced and ionic and net ionic equations for given reactions are,

The balanced equation is,

${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}{\text{+2NaOH}}_{\text{(aq)}}\to {\text{Na}}_{\text{2}}{\text{(CO)}}_{\text{3(aq)}}{\text{+2H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

The ionic equation is,

${\text{2H}}^{\text{+}}{\text{+CO}}_{\text{3}}{{}_{\text{(aq)}}}^{\text{2-}}{\text{+2Na}}^{\text{+}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{Na}}_{\text{2}}{\text{(CO)}}_{\text{3(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}+{\text{2H}}^{\text{+}}$

The net ionic equation is,

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

Explanation of Solution

• The ionic compounds are dissolved in water to produced ions these ions are combined to give new product.
• The reaction is represent by the complex molecular formula means it is a balanced equation and it have equal number of atoms in both reactant and product sides.
• The ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}$ and ${\text{NaOH}}_{\text{(aq)}}$ are react to give the ${\text{Na}}_{\text{2}}{\text{(CO)}}_{\text{3(aq)}}$ so the balanced equation for this reaction is,

  ${\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}{}_{\text{(aq)}}{\text{+2NaOH}}_{\text{(aq)}}\to {\text{Na}}_{\text{2}}{\text{(CO)}}_{\text{3(aq)}}{\text{+2H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

• The all the species present in above equation is writing with respective charges to give ionic reaction.

  ${\text{2H}}^{\text{+}}{\text{+CO}}_{\text{3}}{{}_{\text{(aq)}}}^{\text{2-}}{\text{+2Na}}^{\text{+}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{Na}}_{\text{2}}{\text{(CO)}}_{\text{3(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}+{\text{2H}}^{\text{+}}$

• The removal of common ions from the above equations to give net ionic equations.

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

(c)

Interpretation Introduction

Interpretation:

The balanced and ionic and net ionic equations for given reactions are should be written.

Concept introduction:

Balanced equation:

• The balanced equation is nothing but the all ionic compounds are represented as neutral compounds using the molecular formula.
• In the balanced equation, the number of atoms for each element and total charge are equal in the reaction for in both reactants and the products sides.

Ionic equation:

• In the ionic reactions, all the species present in reaction are written with respective charges is called ionic equation.

Net ionic equation:

• The removal of common ions forms ionic equation to give net ionic equation.
• To write the balanced and ionic and net ionic equations for given reaction.

Answer to Problem 9.35QP

• The balanced and ionic and net ionic equations for given reactions are,

The balanced equation is,

${\text{HNO}}_{\text{3(aq)}}{\text{+Ba(OH)}}_{\text{2(aq)}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}{\text{+2H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

The ionic equation is,

${\text{2H}}^{\text{+}}{\text{+2NO}}_{\text{3(aq)}}{}^{\text{-}}{\text{+Ba}}^{\text{2+}}{\text{+2OH}}^{\text{-}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}$

The net ionic equation is,

${\text{2NO}}_{\text{3(aq)}}{}^{\text{-}}{\text{+Ba}}^{\text{2+}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}$

Explanation of Solution

• The ionic compounds are dissolved in water to produced ions these ions are combined to give new product.
• The reaction is represent by the complex molecular formula means it is a balanced equation and it have equal number of atoms in both reactant and product sides.
• The ${\text{HNO}}_{\text{3(aq)}}$ and ${\text{Ba(OH)}}_{\text{2(aq)}}$ are react to give the ${\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}$ so the balanced equation for this reaction is,

  ${\text{HNO}}_{\text{3(aq)}}{\text{+Ba(OH)}}_{\text{2(aq)}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}{\text{+2H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

• The all the species present in above equation is writing with respective charges to give ionic reaction.

  ${\text{2H}}^{\text{+}}{\text{+2NO}}_{\text{3(aq)}}{}^{\text{-}}{\text{+Ba}}^{\text{2+}}{\text{+2OH}}^{\text{-}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}{\text{+2OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}$

• The removal of common ions from the above equations to give net ionic equations.

  ${\text{2NO}}_{\text{3(aq)}}{}^{\text{-}}{\text{+Ba}}^{\text{2+}}\to {\text{Ba(NO}}_{\text{3}}{\text{)}}_{\text{2(aq)}}$