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Will Germaine11/20/2019Chem 3B-QRESynthesis and Analysis ofK3[Fe(C2O4)3]·3H2OLABORATORY REPORT
Introduction2Fe(NH4)2(SO4)2•6H2O(aq)+3H2C2O4+H2O2+3K2C2O4(aq)→2K3Fe(C2O4)3•3H2O(s)+4(NH4)HSO4(aq)+8We are Synthesizing Iron(II) oxalate hydrate and from that creating Potassium iron(III)oxalate trihydrate and analyzing the iron and oxalate.We first synthesized iron(II) oxalate hydrate solid:Fe(NH4)2(SO4)2•6H2O(aq)+H2C2O4→FeC2O4•2H2O(s)+2(NH4)HSO4(aq)+4H2O(l)Next we oxidized iron(II) to iron(III):−¿3+¿+3e¿2+¿→Fe¿Fe¿2¿oxidation−¿→2H2O+¿+2e¿H2O2+2H¿reduction3+¿+2H2O(l)+¿→2Fe¿2+¿+H2O2+2H¿2Fe¿overallLastly we added potassium oxalate to precipitate potassium iron(III) oxalate trihydrate:
+¿3+¿+3K2C2O4(aq)+3H2O(l)→ K3Fe(C2O4)3•3H2O(s)+3K¿Fe¿ExperimentalTo create iron (II) oxalate hydrate solid we started began with 5.0g of ammoniumiron (II) sulfate and dissolved it in 15.0ml of deionized water with 5 drops of 3.0Msulfuric acid and 25.0 ml of 1.0M oxalic acid solution. The mixture in the flask was thenheated with a Bunsen burner to dissolve the mixture and allowed the solid to settle. Theliquid was then decanted and the solid was reheated with 20.0ml of deionized water andthe solid was allowed to settle again before allowing the liquid to decant again. The solidwas iron (II) oxalate hydrate. 10ml of potassium oxalate solution was then added to thesolid. In a separate beaker 20.0ml of 3% H2O2and 8.0ml of 1.0M oxalic acid solution ina graduated cylinder was measured. The solution was then reheated to 40° and H2O2was added slowly while stirring. Once done the solution was brought to a boil and 5.0mlof 1.0M of the oxalic solution was added at once and the other 3.0ml slowly. After mixingwell the hot solution was filtered into the Erlenmeyer flask and the transferred into a150ml beaker when cooled to room temperature. 15.0 ml of ethyl alcohol was addedand mixed into the solution and the beaker was placed into the lab drawer with a pieceof filter paper atop the beaker and left to precipitate until the next week.