Camila Ambros
Prof. Lovell
CHM1046 lab
Spring 2016
Le Chatelier’s Principle in Iron Thiocyanate Equilibrium
The purpose of the lab was to understand the Le Chatelier’s principle, which is when a
system adjusts itself to decrease the e+ects of concentra,on, temperature, volume, or pressure.
In the lab we measured FeSCN reac,ng with di+erent reagents. We expected to see a change in
colora,on to lighter indica,ng where the equilibrium would shi1.
First we had a control solu,on with the forma,on of FeSCN with an intense red color in
test tube 1 with A= 2.914. In test tube 2 we mixed FeSCN with FeNO3 and we got a darker red
meaning that the equilibrium was shi1ed to the products because the increase in reactants
concentra,on with A= 2.950. In test tube 3 we mixed FeSCN with KSCN and the color is the
darkest seen in the experiment because the increment of reactant concentra,on meaning that
shi1ed to the reactants with A= 2.983. In test tube 4 we added AgNO3 and the colora,on was
cloudy orange with a white precipitate meaning that the equilibrium shi1ed to the reactants
because it destroys the product concentra,on with A= 2.421. In test tube 5 we added HCL and
the colora,on was a clear orange meaning that the equilibrium shi1ed to the reactants because
it breaking the reac,on and the products are the reactant and therefore the color starts to get
lighter with A= 1.058. In test tube 6 we added Hg(NO3)2 and the colora,on was clear meaning
the equilibrium shi1ed to the reactants with A= 0.329. In test tube 7 we added NA2PO4 and the
colora,on was clear light yellow meaning that the equilibrium shi1ed to the reactant less than
in test tube 6 with A=0.185. In test tube 8 we added Na2C2O4 and the colora,on was slightly
green/yellow clear meaning that the equilibrium shi1ed to the reactant less than test tube 7
with A=0.026. In test tube 9 we added NaF(s) and the colora,on was very li>le yellow clear
shi1ed depending on whether the increase in concentra,on would be from the products or
reactants.