Chapter 9, Problem 9.58E

Interpretation Introduction

(a)

Interpretation:

The balanced molecular, total ionic and net ionic form of the given reaction is to be stated.

Concept introduction:

In a balanced molecular chemical equation, all the reactants and products are written with their stoichiometric coefficient and physical states. The total ionic equation is the chemical equation of a reaction in which the ionic compounds are written in their dissociated ionic forms. The net ionic equation is the one in which the common ions present on both the sides of the complete ionic reaction get eliminated and only the chemical species actually participating in the reaction is represented.

Answer to Problem 9.58E

The balanced molecular equation for the given reaction is represented as,

$\text{3RbOH}\left(\text{aq}\right)+{\text{H}}_3{\text{PO}}_4\left(\text{aq}\right)\to {\text{Rb}}_3{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{3Rb}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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

Explanation of Solution

The base $\text{RbOH}$ will react with ${\text{H}}_3{\text{PO}}_4$ to form ${\text{Rb}}_3{\text{PO}}_4$ salt and water. The balanced molecular equation for the given reaction is represented as,

$\text{3RbOH}\left(\text{aq}\right)+{\text{H}}_3{\text{PO}}_4\left(\text{aq}\right)\to {\text{Rb}}_3{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{3Rb}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

${\text{Rb}}^{+}$ and ${\text{PO}}_4{}^{3-}$ ions are common on both sides of the total ionic reaction; therefore, to write net ionic reaction these ions must be eliminated from the reaction. The net ionic equation is represented as,

${\text{3OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)\to 3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The above equation is further simplified as shown below,

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

Conclusion

The balanced molecular equation for the given reaction is represented as,

$\text{3RbOH}\left(\text{aq}\right)+{\text{H}}_3{\text{PO}}_4\left(\text{aq}\right)\to {\text{Rb}}_3{\text{PO}}_4\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{3Rb}}^{+}\left(\text{aq}\right)+3{\text{OH}}^{-}\left(\text{aq}\right)+3{\text{H}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)\to 3{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{PO}}_4{}^{3-}\left(\text{aq}\right)+3{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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

Interpretation Introduction

(b)

Interpretation:

The balanced molecular, total ionic and net ionic form of the given reaction is to be stated.

Concept introduction:

In a balanced molecular chemical equation, all the reactants and products are written with their stoichiometric coefficient and physical states. The total ionic equation is the chemical equation of a reaction in which the ionic compounds are written in their dissociated ionic forms. The net ionic equation is the one in which the common ions present on both the sides of the complete ionic reaction get eliminated and only the chemical species actually participating in the reaction is represented.

Answer to Problem 9.58E

The balanced molecular equation for the given reaction is represented as,

$\text{2RbOH}\left(\text{aq}\right)+{\text{H}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)\to {\text{Rb}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{2Rb}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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

Explanation of Solution

The base $\text{RbOH}$ will react with ${\text{H}}_2{\text{C}}_2{\text{O}}_4$ (oxalic acid) to form ${\text{Rb}}_2{\text{C}}_2{\text{O}}_4$ salt and water. The balanced molecular equation for the given reaction is represented as,

$\text{2RbOH}\left(\text{aq}\right)+{\text{H}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)\to {\text{Rb}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{2Rb}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

${\text{Rb}}^{+}$ and ${\text{C}}_2{\text{O}}_4{}^{2-}$ ions are common on both sides of the total ionic reaction; therefore, to write net ionic reaction these ions must be eliminated from the reaction. The net ionic equation is represented as,

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

The above equation is further simplified as shown below,

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

Conclusion

The balanced molecular equation for the given reaction is represented as,

$\text{2RbOH}\left(\text{aq}\right)+{\text{H}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)\to {\text{Rb}}_2{\text{C}}_2{\text{O}}_4\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{2Rb}}^{+}\left(\text{aq}\right)+2{\text{OH}}^{-}\left(\text{aq}\right)+2{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)\to 2{\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{O}}_4{}^{2-}\left(\text{aq}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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

Interpretation Introduction

(c)

Interpretation:

The balanced molecular, total ionic and net ionic form of the given reaction is to be stated.

Concept introduction:

In a balanced molecular chemical equation, all the reactants and products are written with their stoichiometric coefficient and physical states. The total ionic equation is the chemical equation of a reaction in which the ionic compounds are written in their dissociated ionic forms. The net ionic equation is the one in which the common ions present on both the sides of the complete ionic reaction get eliminated and only the chemical species actually participating in the reaction is represented.

Answer to Problem 9.58E

The balanced molecular equation for the given reaction is represented as,

$\text{RbOH}\left(\text{aq}\right)+{\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)\to {\text{RbC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{Rb}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)\to {\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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

Explanation of Solution

The base $\text{RbOH}$ will react with acetic acid $\left({\text{HC}}_2{\text{H}}_3{\text{O}}_2\right)$ to form ${\text{RbC}}_2{\text{H}}_3{\text{O}}_2$ salt and water. The balanced molecular equation for the given reaction is represented as,

$\text{RbOH}\left(\text{aq}\right)+{\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)\to {\text{RbC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{Rb}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)\to {\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The ${\text{Rb}}^{+}$ and ${\text{SO}}_4{}^{2-}$ ions are common on both sides of the total ionic reaction; therefore, to write net ionic reaction these ions must be eliminated from the reaction. The net ionic equation is represented as,

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

Conclusion

The balanced molecular equation for the given reaction is represented as,

$\text{RbOH}\left(\text{aq}\right)+{\text{HC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)\to {\text{RbC}}_2{\text{H}}_3{\text{O}}_2\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The total ionic chemical equation of the given reaction is represented as,

${\text{Rb}}^{+}\left(\text{aq}\right)+{\text{OH}}^{-}\left(\text{aq}\right)+{\text{H}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)\to {\text{Rb}}^{+}\left(\text{aq}\right)+{\text{C}}_2{\text{H}}_3{\text{O}}_2{}^{-}\left(\text{aq}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$

The net ionic chemical equation of the given reaction is represented as,

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