Synthesis and Characterization of K2[Ni(CN)4] , K3[Fe(C2O4)3] and Cu(acac)2 Complexes :: Lab Report

Synthesis and act of K2Ni(CN)4 , K3Fe(C2O4)3 and Cu(acac)2 complexes(IV , V and VI) with different structuresand Properties1. first appearanceThe aim of this experiment was to synthesize HgCo(SCN)4 , Ni(en)3S2O3 , NiCl2(PPh3)2 , K2Ni(CN)4 , K3Fe(C2O4)3 and Cu(acac)2 but only K2Ni(CN)4 , K3Fe(C2O4)3 and Cu(acac)2 were synthesized and explained in this report. Characterization was then done on apiece of the 3 synthesized complexes by obtaining their UV-Vis spectrum. The UV-Vis spectrum of each complex would identify different properties and would help to explain the observations made when they were synthesized (for causa their colour and how they reacted).2. mannerTable 1 Synthesis of K2Ni(CN)4Amount of Reagents useMethodObservationsNiSO4 7H2O 6.00 gKCN 3.01gIn 20ml water NiSO4 7H2O was dissolved and the upshot containing KCN (dissolved in 7ml water) was added to the Nickel solution. This solution was filtered and the precipitate was washed with small quantities of water. Th is precipitate was added to the solution of KCN (dissolved in 3ml of water). This solution was heat and swirled so that the crystals that formed dissolved. It was het again and left so that crystals started forming again. This solution was then placed in an codswallop bath to enhance crystallization and the crystals were remove by filtration. The water was removed by drying the crystals in the oven at 100C. A small core of the sample was dissolved in water and the UV-Vis spectrum was obtained.Nickel (II) sulphate hexahydrate was utilize in place of heptahydrate.When the precipitate was added to the KCN solution, it turned dark red. As it was heated it darkened even more but as the crystals started forming the colour changed to a light red.As the crystals dried more its colour changed from light red-orange to a light yellow colour.These crystals were dissolved in water for the UV-vis spectrum. The solution was a yellow colour.Table 2 Synthesis of K3Fe(C2O4)3Amount of Re agents usedMethodObservations(NH4)2Fe(SO4)2 6H2O 5.03gTo a solution of (NH4)2Fe(SO4)2 6H2O (dissolved in 20ml water) 1 ml of sulphuric harsh was added and stirred. The oxalic acid (dissolved in 25ml water) was also added and this combined solution was slowly heated to boiling, resulting in the formation of yellow iron(II) oxalate precipitate. The liquid was decanted and 15ml of hot water was added again to the precipitate, this was stirred and filtered. The precipitate (iron(II) oxalate) was transferred to another beaker and a potassium oxalate solution (dissolved in 10ml hot water) was added.