iron oxalate lab - Chris Stanton Chemistry 216 March 15,...

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Chris Stanton March 15, 2007 Chemistry 216 Potassium Iron Oxalate I. Introduction This lab consisted of the synthesis of the potassium iron oxalate compound and then the determination of the stoichiometry of the hydrated salt compound. The salt (with formula K x Fe y (C 2 O 4 ) z ∙nH 2 O) is synthesized by allowing crystals to form twice to eliminate contamination and then analysis of the compound can begin. The mass of the dry sample is determined and then heated slowly to drive off any water, which at that point the mass can be taken again to allow for the calculation for the loss of the water of hydration. The anhydrous sample is then taken and eluted using a cation exchange column. The final solution can be titrated with NaOH to determine each equivalence point. The first equivalence point yields the calculation of the mass percent of K in the sample and the second yields the calculation of the mass percent of Fe. Using these figures and the weights in the beginning, the stoichiometry of the compound (both the hydrated and anhydrous parts) can be determined. II. Experimental Procedure A. Synthesis of the Complex 1. Put about 8 mL of the FeCl 3 solution into a clean 100 mL beaker. Weigh out about 12 grams of potassium oxalate, K 2 C 2 O 4 ∙H 2 O, into a clean 50 mL beaker and add about 20 mL of distilled water. Heat to dissolve solution. 2. Once it has dissolved, add the hot solution into the beaker containing the FeCl 3 and stir. 3. Make an ice bath with water and ice and then place the beaker containing the stirred hot solution in it for 30 – 45 minutes. Crystals should form. 4. After 30 – 45 minutes, carefully pour off the solvent (discard into sink), trying not to lose any crystals. 5.
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iron oxalate lab - Chris Stanton Chemistry 216 March 15,...

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