Chapter U4, Problem 6RE

(a)

Interpretation Introduction

Interpretation: The complete and net ionic equation for the reaction between magnesium nitrate and calcium chloride is to be written.

Concept introduction: In ionic equation, all the aqueous species are written in their ionic form. The net ionic equation is the equation in which the species which are actually taking part in the reaction are written.

Answer to Problem 6RE

The complete ionic equation for the reaction between magnesium nitrate and calcium chloride is shown below:

  ${\text{Mg}}^{2+}\left(aq\right)+2{\text{NO}}_3^{-}\left(aq\right)+{\text{Ca}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to {\text{MgCl}}_2\left(s\right)+{\text{Ca}}^{2+}\left(aq\right)+2{\text{NO}}_3^{-}\left(aq\right)$

The net ionic equation for the reaction between magnesium nitrate and calcium chloride is below:

  ${\text{Mg}}^{2+}\left(aq\right)+{\text{2Cl}}^{-}\left(aq\right)\to {\text{MgCl}}_{\text{2}}\left(s\right)$

Explanation of Solution

Magnesium nitrate reacts with calcium chloride to form precipitate of magnesium chloride and calcium nitrate. The corresponding equation is shown below:

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

In the above equation, magnesium nitrate dissociates into ${\text{Mg}}^{\text{2}+}$ and two ${\text{NO}}_3^{-}$ ions. The calcium chloride dissociates into ${\text{Ca}}^{2+}$ and two ${\text{Cl}}^{-}$ ions. The calcium nitrate dissociates into ${\text{Ca}}^{2+}$ and two ${\text{NO}}_3^{-}$ ions. Therefore, the complete ionic equation is shown below:

  ${\text{Mg}}^{2+}\left(aq\right)+2{\text{NO}}_3^{-}\left(aq\right)+{\text{Ca}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to {\text{MgCl}}_2\left(s\right)+{\text{Ca}}^{2+}\left(aq\right)+2{\text{NO}}_3^{-}\left(aq\right)$ The ${\text{Ca}}^{2+}$ ion and two ${\text{NO}}_3^{-}$ ions are spectator ions. Therefore, these ions can be cancelled. The net ionic equation for the reaction between magnesium nitrate and calcium chloride is below:

  ${\text{Mg}}^{2+}\left(aq\right)+{\text{2Cl}}^{-}\left(aq\right)\to {\text{MgCl}}_{\text{2}}\left(s\right)$

(b)

Interpretation Introduction

Interpretation:

The complete and net ionic equation for the reaction between silver nitrate and potassium iodide is to be written.

Concept introduction: In ionic equation, all the aqueous species are written in their ionic form. The net ionic equation is the equation in which the species which are actually taking part in the reaction are written.

Answer to Problem 6RE

The complete ionic equation for the reaction between silver nitrate and potassium iodide is shown below:

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

The net ionic equation for the reaction between silver nitrate and potassium iodide is below:

  ${\text{Ag}}^{+}\left(aq\right)+{\text{I}}^{-}\left(aq\right)\to \text{AgI}\left(s\right)$

Explanation of Solution

Aqueous silver nitrate reacts with potassium iodide to form precipitate of silver iodide and potassium nitrate. The corresponding equation is shown below:

  ${\text{AgNO}}_{\text{3}}\left(aq\right)+\text{KI}\left(aq\right)\to \text{Agl}\left(s\right)+{\text{KNO}}_{\text{3}}\left(aq\right)$

In the above equation, silver nitrate dissociates into ${\text{Ag}}^{+}$ and ${\text{NO}}_3^{-}$ ion. The potassium iodide dissociates into ${\text{K}}^{+}$ and ${\text{I}}^{-}$ ion. The potassium nitrate dissociates into ${\text{K}}^{+}$ and ${\text{NO}}_3^{-}$ ions. Therefore, the complete ionic equation is shown below:

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

The ${\text{K}}^{+}$ ion and ${\text{NO}}_3^{-}$ ions are spectator ions. Therefore, these ions can be cancelled. The net ionic equation for the reaction between silver nitrate and potassium iodide is below:

  ${\text{Ag}}^{+}\left(aq\right)+{\text{I}}^{-}\left(aq\right)\to \text{AgI}\left(s\right)$

(c)

Interpretation Introduction

Interpretation:

The complete and net ionic equation for the reaction between sodium sulfate and barium chloride is to be written.

Concept introduction: In ionic equation, all the aqueous species are written in their ionic form. The net ionic equation is the equation in which the species which are actually taking part in the reaction are written.

Answer to Problem 6RE

The complete ionic equation for the reaction between sodium sulfate and barium chloride is shown below:

  ${\text{2Na}}^{+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)+{\text{Ba}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to {\text{BaSO}}_4\left(s\right)+2{\text{Na}}^{+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)$

The complete and net ionic equation for the reaction between sodium sulfate and barium chloride is shown below:

  ${\text{Ba}}^{2+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)\to {\text{BaSO}}_{\text{4}}\left(s\right)$

Explanation of Solution

Aqueous sodium sulfate reacts with barium chloride to form precipitate of barium sulfate and sodium chloride. The corresponding reaction is shown below:

  ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{4}}\left(aq\right)+{\text{BaCl}}_{\text{2}}\left(aq\right)\to {\text{BaSO}}_{\text{4}}\left(s\right)+2\text{NaCl}\left(aq\right)$

In the above equation, sodium sulfate dissociates into two ${\text{Na}}^{+}$ and ${\text{SO}}_4^{2-}$ ions. The barium chloride dissociates into

  ${\text{Ba}}^{2+}$ and two ${\text{Cl}}^{-}$ ions. The sodium chloride dissociates into ${\text{Na}}^{+}$ and ${\text{Cl}}^{-}$ ions. Therefore, the complete ionic equation for the reaction is shown below:

  ${\text{2Na}}^{+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)+{\text{Ba}}^{2+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)\to {\text{BaSO}}_4\left(s\right)+2{\text{Na}}^{+}\left(aq\right)+2{\text{Cl}}^{-}\left(aq\right)$

The ${\text{K}}^{+}$ ion and ${\text{NO}}_3^{-}$ ions are spectator ions. Therefore, these ions can be cancelled. The net ionic equation for the reaction between silver nitrate and potassium iodide is below:

  ${\text{Ba}}^{2+}\left(aq\right)+{\text{SO}}_4^{2-}\left(aq\right)\to {\text{BaSO}}_4\left(s\right)$