Chapter 4, Problem 4.163QP

(1-a)

Interpretation Introduction

Interpretation:

The balanced molecular equation and net ionic equation for given reaction with given assumptions 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 4.163QP

The complete molecular equation

${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}\text{ + Ba}{\left(\text{OH}\right)}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

The complete ionic equation

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

The net ionic equation

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

Explanation of Solution

Assume that both hydrogen atoms of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ ionize completely.

${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}\text{ + Ba}{\left(\text{OH}\right)}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

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

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

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

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

(1-b)

Interpretation Introduction

Interpretation:

The balanced molecular equation and net ionic equation for given reaction with given assumptions 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 4.163QP

The complete molecular equation

${\text{H}}_{\text{2­}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}\text{ + Ba}{\left(\text{OH}\right)}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

The complete ionic equation

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right){\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

The net ionic equation

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{+ HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{+ Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

Explanation of Solution

Assume that only first hydrogen ion of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ ionize completely and other one is weakly ionizing.

${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}\text{ + Ba}{\left(\text{OH}\right)}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

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

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

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

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + Ba}}^{\text{2+}}{}_{\left(\text{aq}\right)}{\text{ + 2OH}}^{\text{-}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

(2-a)

Interpretation Introduction

Interpretation:

The balanced molecular equation and net ionic equation for given reaction with given assumptions 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 4.163QP

The complete molecular equation

${\text{H}}_{\text{2­}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2NaC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

The complete ionic equation

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right){\text{ + 2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

The net ionic equation

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{ HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

Explanation of Solution

Assume that both hydrogen atoms of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ ionize completely.

${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}\text{ + Ba}{\left(\text{OH}\right)}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{BaSO}}_{\text{4}}{}_{\left(\text{s}\right)}{\text{ + 2H}}_{\text{2}}{\text{O}}_{\left(\text{l}\right)}$

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

${\text{2H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{}^{\text{2-}}\left(\text{aq}\right){\text{ + 2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

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

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{ HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

(2-b)

Interpretation Introduction

Interpretation:

The balanced molecular equation and net ionic equation for given reaction with given assumptions 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 4.163QP

(b)

The complete molecular equation

${\text{H}}_{\text{2­}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2NaC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

The complete ionic equation

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + 2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

The net ionic equation

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{ SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

Explanation of Solution

Assume that only first hydrogen ion of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ ionize completely and other one is weakly ionizing.

${\text{H}}_{\text{2­}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2NaC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}{}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

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

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + 2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{2Na}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$

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

${\text{H}}^{\text{+}}{}_{\left(\text{aq}\right)}{\text{ + HSO}}_{\text{4}}{{}^{\text{-}}}_{\left(\text{aq}\right)}{\text{ + 2C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{{}^{\text{-}}}_{\left(\text{aq}\right)}\stackrel{}{\to }{\text{ SO}}_{\text{4}}{{}^{\text{2-}}}_{\left(\text{aq}\right)}{\text{ + 2HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}{}_{\left(\text{aq}\right)}$