# Is iron(III)nitrate changed and if so how?

We have the solution:

$$\ce{Fe^3+(aq) + SCN-(aq) <=>Fe(SCN)^2+}$$

When we add more $$\ce {SCN-}$$ to the solution above, the solution produces more product.

My question is, how does it affect $$\ce {Fe^3+}$$? Do the concentration of iron(III)nitrate change or something?

If a stoichiometric amount of $$\ce{SCN-}$$ is added then the reaction is mostly
$$\ce{Fe^3+(aq) + SCN-(aq) <=>Fe(SCN)^2+(aq)}$$
If an excess of of $$\ce{SCN-}$$ is added then the reaction is mostly
$$\ce{Fe^3+(aq) + 2SCN-(aq) <=>[excess SCN-] Fe(SCN)2^+(aq)}$$