ferric oxalate lab report.edited for butha - Students Name...

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Student’s Name: Professor’s Name: Course: Date: Experiment #26 Synthesis and Analysis of K 3 Fe(C 2 O 4 ) 3 ∙ 3H 2 O
Surname 1 Introduction: The aim of the practical is to make potassium ferric oxalate, then determine the oxalate ion in the product (potassium ferric oxalate) and determine the amount of iron in the product. In the first step ammonium iron (2) sulfate hexahydrate was reacted with oxalic acid to form an insoluble yellow solid (ferrous oxalate). The next step involved oxidation of ferrous oxalate using hydrogen peroxide, acidified potassium permanganate, and oxalate ion to form an insoluble green solid (ferric potassium oxalate). The product was then analyzed for purity using two methods; in the first method, the product was made into a solution and titrated using acidified potassium permanganate. In this reaction, the oxalate iron was oxidized into carbon dioxide and potassium into manganate(2) ion(Mn 2+ ) while the acid was reduced to water, a kind of acid-base reaction. The amount of iron in the product was determined using the spectrometer. Spectrophotometry uses absorbance to measure the concentration of a substance in a solution. The more concentrated a solution is, the higher the amount of light it absorbs. To accomplish this, the Iron was first made into a complex molecule by adding phenanthroline to form a red solution. Experimental: The experiment was started by dissolving Fe(NH 4 ) 2 (SO 4 ) 2 ∙6H 2 0 into deionized water and a small amount of 3M H 2 SO 4 . An amount of 1M oxalic acid (H 2 C 2 O 4 ) solution was then added, and this solution was heated and stirred until it started to boil. The solution was then placed aside, letting the solid settle. The liquid was poured out while the solid remained. Deionized water was added to the solid and heated a second time. The same PAGE 1
Surname 2 process of removing the liquid from the solid was used. An amount of saturated potassium oxalate (K 2 C 2 O 4 ) solution was added to this solid and put aside while a simple filtration system was set up. Once this was done, the solution with yellow solid was heated. An amount of H 2 O 2 was added to this hot solution very slowly. This was then heated until it started boiling and an amount of 1M H 2 C 2 O 4 solution was added. This was mixed and filtered. Once the solution had cooled, it was transferred to a beaker, where ethyl alcohol was added and mixed. This was then allowed to sit for 1 week. After this period, the solid crystals in the beaker were collected and washed with ethyl alcohol and deionized water. The weight of the dry crystals was obtained. An amount of the sample was then weighed and transferred to a volumetric flask. Deionized water and a small amount of 3M H 2 SO 4 was added to dissolve the solid and reach the calibration mark. This solution was then mixed thoroughly and transferred to a clean and dry

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