Question

How do i find the net ionic equation for the reaction between ammonium hydroxide and iron(III)chloride ?

Answer 1

How do I find the net ionic equation for the reaction between ammonium hydroxide and iron(III)chloride?

Solution. The molecular reaction can be described with the following equation:

$$3 \mathrm{NH_4OH} + \mathrm{FeCl_3} = \mathrm{Fe(OH)_3} + 3 \mathrm{NH_4Cl}.$$

Net ionic equation describes the reaction between the ions present on the solution. Ammonium hydroxide and iron(III)chloride dissociate and give the next ions: $\mathrm{NH_4^+}$, $\mathrm{OH^-}$, $\mathrm{Fe^{3+}}$, $\mathrm{Cl^-}$. $\mathrm{Fe(OH)_3}$ doesn't dissociate to give the ions, because it is a solid compound, it is a precipitate. $\mathrm{NH_4Cl}$ is a soluble in the water salt. It gives $\mathrm{NH_4^+}$ and $\mathrm{Cl^-}$ ions. The molecular reaction can be overwritten into total ionic equation:

$$3 \mathrm{NH_4^+} + 3 \mathrm{OH^-} + \mathrm{Fe^{3+}} + 3 \mathrm{Cl^-} = \mathrm{Fe(OH)_3} + 3 \mathrm{NH_4^{2+}} + 3 \mathrm{Cl^-};$$

You can see, that in the in both left and right parts there are the same ions: $\mathrm{NH_4^+}$ and $\mathrm{Cl^-}$ and they can be reduced. In this case the net ionic equation is formed:

$$\mathrm{Fe^{3+}} + 3 \mathrm{OH^-} = \mathrm{Fe(OH)_3}$$