# How do you balance this equation? Fe(NO_3)_3 + KSCN -> Fe(NO_3)_3 + KSCN

Jun 24, 2016

NO

#### Explanation:

Since,the reactants side is the same as product side,hence, no chemical reaction has taken place.

Hence,since it isn't even a chemical reaction it cant be ballanced.

Jun 24, 2016

$F e {\left(N {O}_{3}\right)}_{3} + 3 K S C N \rightarrow \left[F e {\left(S C N\right)}_{3}\right] + 3 K N {O}_{3}$

#### Explanation:

The tristhiocyanato iron species is a so-called complex ion. Both mass and charge are balanced in the equation.

Jun 24, 2016

You haven't actually written any products but I will describe the reaction below:

#### Explanation:

Iron(III) ions form a blood-red complex with thiocyanate ions in a 1:1 molar ratio.

$F e {\left(N {O}_{3}\right)}_{3}$ + $K S C N \rightarrow {\left[F e S C N\right]}^{2 +} + {K}^{+} + 3 N {O}_{3}^{-}$

The ionic equation which omits the spectator ions is:

$F {e}_{\left(a q\right)}^{3 +} + S C {N}_{\left(a q\right)}^{-} \rightarrow {\left[F e \left(S C N\right)\right]}_{\left(a q\right)}^{2 +}$

The complex is very intensely coloured and this reaction is often used as a qualitative test for iron(III) ions.

Strictly speaking we have a ligand exchange reaction:

${\left[F e {\left({H}_{2} O\right)}_{6}\right]}^{3 +} + S C {N}^{-} \rightarrow {\left[F e {\left({H}_{2} O\right)}_{5} S C N\right]}^{2 +} + {H}_{2} O$

The reaction is shown here: