Question

An aqueous solution of Iron(III) sulfate, Fe2(SO4)3, is mixed with an aqueous solution of Sodium hydroxide, NaOH. Write:_______. a. balanced molecular equation b. the total ionic equation c. the net ionic equation showing all phases.

Answer 1

Answer:

a.

$Fe_2(SO_4)_3(aq)+6NaOH(aq)\rightarrow 2Fe(OH)_3(s)+3Na_2SO_4(aq)$

b.

$2Fe^{2+}(aq)+3(SO_4)^{2-}(aq)+6Na^+(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)+6Na^+(aq)+3(SO_4)^{2-}(aq)$

c.

$Fe^{2+}(aq)+3OH^-(aq)\rightarrow Fe(OH)_3(s)$

Explanation:

Hello!

In this case, since the reaction between sodium hydroxide and iron (III) sulfate yields iron (III) hydroxide, an insoluble base, and sodium sulfate, a soluble salt, we can write the molecular equation as shown below:

a.

$Fe_2(SO_4)_3(aq)+6NaOH(aq)\rightarrow 2Fe(OH)_3(s)+3Na_2SO_4(aq)$

Now, for the total ionic equation, we make sure we separate the aqueous species in ions (dissociation) in order to write:

b.

$2Fe^{2+}(aq)+3(SO_4)^{2-}(aq)+6Na^+(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)+6Na^+(aq)+3(SO_4)^{2-}(aq)$

Finally, the net ionic equation comes up by cancelling out the spectator ions, those at both reactants and products sides:

$2Fe^{2+}(aq)+6OH^-(aq)\rightarrow 2Fe(OH)_3(s)$

Or just:

c.

$Fe^{2+}(aq)+3OH^-(aq)\rightarrow Fe(OH)_3(s)$

Best regards!