Chapter 4, Problem 4.33QP

Write net ionic equations for the following molecular equations. HBr is a strong electrolyte.

1. a HBr(aq) + KOH(aq) → KBr(aq) + H₂O(l)
2. b AgNO₃(aq) + NaBr(aq) → AgBr(s) + NaNO₃(aq)
3. c K₂S(aq) + 2HBr(aq) →2KBr(aq) + H₂S(g)
4. d NaOH(aq) + NH₄Br(aq) → NaBr(aq) + NH₃(g) + H₂O(l)

Interpretation Introduction

Interpretation:

To write the complete and net ionic equations for the given set of molecular equations.

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.

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

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.

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

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.

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

Answer to Problem 4.33QP

The complete ionic equation

${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+K}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{K}}^{+}{}_{\text{(aq)}}+{\text{Br}}^{\text{-}}{}_{\text{(aq)}}+{\text{H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

The net ionic equation

${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

Explanation of Solution

The molecular equation for the reaction between $\text{HBr}$ and $\text{KOH}$ are given.  In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction between $\text{HBr}$ and $\text{KOH}$ is given below.

${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+K}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{K}}^{+}{}_{\text{(aq)}}+{\text{Br}}^{\text{-}}{}_{\text{(aq)}}+{\text{H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

The net ionic equation for the reaction between $\text{HBr}$ and $\text{KOH}$ is given below.  The ions common in both the sides are neglected from the equation.

${\text{H}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{O}}_{\text{(l)}}$

Interpretation Introduction

Interpretation:

To write the complete and net ionic equations for the given set of molecular equations.

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.

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

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.

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

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.

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

Answer to Problem 4.33QP

The complete ionic equation

${\text{Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}{\text{+Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{AgBr}}_{\text{(s)}}{\text{+Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}$

The net ionic equation

${\text{Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{AgBr}}_{\text{(s)}}$

Explanation of Solution

The molecular equation for the reaction between ${\text{AgNO}}_{\text{3}}$ and $\text{NaBr}$ are given.  In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction between ${\text{AgNO}}_{\text{3}}$ and $\text{NaBr}$ is given below.

${\text{Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}{\text{+Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{AgBr}}_{\text{(s)}}{\text{+Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+NO}}_{\text{3}}{{}^{\text{-}}}_{\text{(aq)}}$

The net ionic equation for the reaction between ${\text{AgNO}}_{\text{3}}$ and $\text{NaBr}$ is given below.  The ions common in both the sides are neglected from the equation.

${\text{Ag}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{AgBr}}_{\text{(s)}}$

Interpretation Introduction

Interpretation:

To write the complete and net ionic equations for the given set of molecular equations.

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.

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

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.

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

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.

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

Answer to Problem 4.33QP

The complete ionic equation

${\text{2K}}^{\text{+}}{}_{\text{(aq)}}{\text{+S}}^{2-}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}{\text{+2Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{2K}}^{\text{+}}{}_{\text{(aq)}}{\text{+2Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+H}}_{\text{2}}{\text{S}}_{\text{(g)}}$

The net ionic equation

${\text{S}}^{2-}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{S}}_{\text{(g)}}$

Explanation of Solution

The molecular equation for the reaction between ${\text{K}}_{\text{2}}\text{S}$ and $\text{HBr}$ are given.  In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction between ${\text{K}}_{\text{2}}\text{S}$ and $\text{HBr}$ is given below.

${\text{2K}}^{\text{+}}{}_{\text{(aq)}}{\text{+S}}^{2-}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}{\text{+2Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{2K}}^{\text{+}}{}_{\text{(aq)}}{\text{+2Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+H}}_{\text{2}}{\text{S}}_{\text{(g)}}$

The net ionic equation for the reaction between ${\text{K}}_{\text{2}}\text{S}$ and $\text{HBr}$ is given below.  The ions common in both the sides are neglected from the equation.

${\text{S}}^{2-}{}_{\text{(aq)}}{\text{+2H}}^{\text{+}}{}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{S}}_{\text{(g)}}$

Interpretation Introduction

Interpretation:

To write the complete and net ionic equations for the given set of molecular equations.

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.

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

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.

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

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.

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

Answer to Problem 4.33QP

The complete ionic equation

${\text{Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+H}}_{\text{2}}{\text{O}}_{\text{(g)}}{\text{+NH}}_{\text{3(g)}}$

The net ionic equation

${\text{OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{O}}_{\text{(g)}}{\text{+NH}}_{\text{3(g)}}$

Explanation of Solution

The molecular equation for the reaction between $\text{NaOH}$ and ${\text{NH}}_4\text{Br}$ are given.  In complete ionic equation the electrolytes are represented as its ions.  The complete ionic equation for the reaction is given below.

${\text{Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}\to {\text{Na}}^{\text{+}}{}_{\text{(aq)}}{\text{+Br}}^{\text{-}}{}_{\text{(aq)}}{\text{+H}}_{\text{2}}{\text{O}}_{\text{(g)}}{\text{+NH}}_{\text{3(g)}}$

The net ionic equation for the reaction between $\text{NaOH}$ and ${\text{NH}}_4\text{Br}$ is given below.  The ions common in both the sides are neglected from the equation.

${\text{OH}}^{\text{-}}{}_{\text{(aq)}}{\text{+NH}}_{\text{4}}{{}^{\text{+}}}_{\text{(aq)}}\to {\text{H}}_{\text{2}}{\text{O}}_{\text{(g)}}{\text{+NH}}_{\text{3(g)}}$