lab2.docx - Introduction In this experiment the compound...

  • Cornell University
  • CHEM 2150
  • Lab Report
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Introduction: In this experiment, the compound potassium tris(oxalato)ferrate (III) trihydrate [K 3 Fe(C 2 O 4 ) 3 3H 2 O] was synthesized in a two-step reaction. Additionally, the compound was analyzed by determining the number of waters of hydration as well as determining the number of oxalate ions in the complex. The purpose of this analysis step was to confirm the identity of the synthesized complex. The objective of the experiment was to obtain the greatest potassium tris(oxalato)ferrate (III) trihydrate yield possible. Experimental: A two-step reaction to produce potassium tris(oxalato)ferrate(III) trihydrate was performed. The first reaction occurred between ferrous ammonium sulfate hexahydrate [Fe(NH 4 ) 2 (SO 4 ) 2 6H 2 O] and oxalic acid (H 2 C 2 O 4 ) to produce iron (II) oxalate dehydrate (FeC 2 O 4 2H 2 O). Then, the iron (II) oxalate dehydrate was reacted with oxalic acid, hydrogen peroxide (H 2 O 2 ), and potassium oxalate (K 2 C 2 O 4 ) to synthesize the potassium tris(oxalato)ferrate(III) trihydrate product. After allowing a week for the complex to develop, the potassium tris(oxalato)ferrate(III) trihydrate crystals were separated from the solution. Following the synthesis and isolation of this compound, the first analysis was to determine the number of waters of hydration of the product; a sample of the compound was heated to boil off all the water. Then, a second analysis was performed to determine the moles of oxalate ions per mole of the synthesized product. This took place through titration with the permanganate ion (MnO 4 - ). First, a permanganate solution was standardized, to calculate the exact molarity, by titrating it with sodium oxalate. Then, the oxalate part of the synthesized complex was titrated with the standardized permanganate solution to ascertain the number of moles of oxalate ion for each mole of complex. At the end of the experiment, the remaining KMnO 4 solution was reduced with solid ferrous sulfate (Fe 2 SO 4 ).

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