Questions: Write the balanced COMPLETE ionic equation for the reaction when Fe(NO3)3 and NaOH are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

Write the balanced COMPLETE ionic equation for the reaction when Fe(NO3)3 and NaOH are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

Transcript text: Write the balanced COMPLETE ionic equation for the reaction when $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}$ and NaOH are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

Solution

Solution Steps

Step 1: Identify the Reactants and Products

The reactants in this reaction are iron(III) nitrate, $\mathrm{Fe(NO_3)_3}$, and sodium hydroxide, $\mathrm{NaOH}$. When these two compounds are mixed in aqueous solution, a double displacement reaction occurs, forming iron(III) hydroxide, $\mathrm{Fe(OH)_3}$, and sodium nitrate, $\mathrm{NaNO_3}$.

Step 2: Write the Molecular Equation

The molecular equation for the reaction is: \[ \mathrm{Fe(NO_3)_3(aq) + 3NaOH(aq) \rightarrow Fe(OH)_3(s) + 3NaNO_3(aq)} \]

Step 3: Write the Complete Ionic Equation

In the complete ionic equation, all strong electrolytes (soluble ionic compounds) are dissociated into their ions: \[ \mathrm{Fe^{3+}(aq) + 3NO_3^-(aq) + 3Na^+(aq) + 3OH^-(aq) \rightarrow Fe(OH)_3(s) + 3Na^+(aq) + 3NO_3^-(aq)} \]

Step 4: Cancel Spectator Ions

Spectator ions are ions that appear on both sides of the equation and do not participate in the reaction. In this case, the spectator ions are $\mathrm{Na^+}$ and $\mathrm{NO_3^-}$.

Step 5: Write the Net Ionic Equation

After removing the spectator ions, the net ionic equation is: \[ \mathrm{Fe^{3+}(aq) + 3OH^-(aq) \rightarrow Fe(OH)_3(s)} \]