Question

In this lab we will actually mix aqueous Fe(NO3)3 with aqueous KSCN to form aqueous FeSCN2 and aqueous KNO3. a. Write the molecular form of the reaction. b. Write the complete ionic form of the reaction. c. Write the net ionic form of the reaction.

Answer 1

Answer :

(a) The balanced molecular equation will be,

$3KSCN(aq)+Fe(NO_3)_3(aq)\rightarrow Fe(SCN)_3(aq)+3KNO_3(aq)$

(b) The complete ionic equation in separated aqueous solution will be,

$3K^+(aq)+3SCN^{-}(aq)+Fe^{3+}(aq)+NO_3^{-}(aq)\rightarrow Fe^{3+}(aq)+3SCN^{-}(aq)+3K^+(aq)+3NO_3^-(aq)$

(c) In this equation the all the species are in aqueous state. So, there is no net ionic form of the reaction.

Explanation :

Complete ionic equation : In complete ionic equation, all the substance that are strong electrolyte and present in an aqueous are represented in the form of ions.

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

(a) The balanced molecular equation will be,

$3KSCN(aq)+Fe(NO_3)_3(aq)\rightarrow Fe(SCN)_3(aq)+3KNO_3(aq)$

(b) The complete ionic equation in separated aqueous solution will be,

$3K^+(aq)+3SCN^{-}(aq)+Fe^{3+}(aq)+NO_3^{-}(aq)\rightarrow Fe^{3+}(aq)+3SCN^{-}(aq)+3K^+(aq)+3NO_3^-(aq)$

(c) In this equation the all the species are in aqueous state. So, there is no net ionic form of the reaction.