Question

Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: $$ \mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between \(\mathrm{NiO}(s)\) and an aqueous solution of nitric acid.

Short answer

The net ionic equations for the given reactions are: (a) \( \mathrm{FeO}(s)+2 \mathrm{H^{+}}(a q) \rightarrow \mathrm{Fe^{2+}}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \) (b) \( \mathrm{NiO}(s)+2 \mathrm{H^{+}}(a q) \rightarrow \mathrm{Ni^{2+}}(a q) + \mathrm{H}_{2}\mathrm{O}(l) \)

Step-by-step solution

Molecular Equation

Given equation: \[ \mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \] #Step 2: Write the complete ionic equation#

Complete Ionic Equation

Break down strong electrolytes into their respective ions: \[ \mathrm{FeO}(s)+2 \mathrm{H^{+}}(a q)+2 \mathrm{ClO}_{4}^{-}(a q) \rightarrow \mathrm{Fe^{2+}}(a q) + 2\mathrm{ClO}_{4}^{- }(a q) + \mathrm{H}_{2} \mathrm{O}(l) \] #Step 3: Identify and remove the spectator ions#

Spectator Ions

The spectator ion is: \(2\mathrm{ClO}_{4}^{-}(a q)\) #Step 4: Write the net ionic equation#

Net Ionic Equation for (a)

After removing the spectator ion, the net ionic equation is: \[ \mathrm{FeO}(s)+2 \mathrm{H^{+}}(a q) \rightarrow \mathrm{Fe^{2+}}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \] For part (b): #Step 1: Write the balanced molecular equation#

Molecular Equation for (b)

We replace FeO with NiO and replace HClO4 with HNO3 to get the molecular equation: \[ \mathrm{NiO}(s)+2 \mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}\mathrm{O}(l) \] #Step 2: Write the complete ionic equation#

Complete Ionic Equation for (b)

Break down strong electrolytes into their respective ions: \[ \mathrm{NiO}(s)+2 \mathrm{H^{+}}(a q)+2 \mathrm{NO}_{3}^{-}(a q) \rightarrow \mathrm{Ni^{2+}}(a q) + 2\mathrm{NO}_{3}^{-}(a q) + \mathrm{H}_{2}\mathrm{O}(l) \] #Step 3: Identify and remove the spectator ions#

Spectator Ions for (b)

The spectator ion is: \(2\mathrm{NO}_{3}^{-}(a q)\) #Step 4: Write the net ionic equation#

Net Ionic Equation for (b)

After removing the spectator ion, the net ionic equation is: \[ \mathrm{NiO}(s)+2 \mathrm{H^{+}}(a q) \rightarrow \mathrm{Ni^{2+}}(a q) + \mathrm{H}_{2}\mathrm{O}(l) \]