Trihydrate Lab Report

Introduction: For my final lab, I was given the task of producing the coordination complex Tris(Oxalato)Ferrate(III) Trihydrate using the following equation:
FeCl3+3K2C2O4H2OK3Fe(C2O4)33H2O(g) +3KCl(aq)
As a result, 4.105g of green crystal complex was produced and analyzed based on percent composition. To complete this analysis, four other experiments using titration, visible spectroscopy, ion sensitive electrodes, and dehydration and were used to determine the composition of oxalate, iron, potassium and water in the produced complex. The following report records the the results of these experiments and discusses any finding or errors in the procedure.
Experimental Data:
When the individual components of the complex were analyzed, it was

It can been seen that there are two distinct bonds, between two oxalates (94.06°, 93.56°, 90.61°, 94.30°) and within a singular oxalate (81.30°, 82.63°). The reason these bond angles vary within this octahedral complex are a result of lone pair repulsion creating slight variations among the bonds.
Color Determination: To explain the coloring of Potassium Tris(Oxalato)Ferrate(III) Trihydrate, we must take into account λmax. Potassium Tris(Oxalato)Ferrate(III) Trihydrate had a λmax of approximately 395 nm, and formed yellow green crystals. When we look at a color wheel it can be seen that a substance with a λmax of approximately 395 nm would absorb violet light. As a result, light at approximately 560 nm (directly between yellow and green) would be reflected and therefore seen by the human eye as a yellowish green substance. It also means that this complex has a greater crystal field splitting (Δ) than the copper complex. This is known through the application of equation E=hc. When calculated, the Δ for the iron complex was about 303 kJ/mol while the copper complex was only about 197