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Redox Titration of CobaltOxalate CompoundREBECCA FORLOINELAB PARTNER: NIYATIAPRIL 6, 2015Having read the Georgia Institute of Technology Academic Honor code, I understand and accept my responsibility as a member of the Georgia Tech Community to uphold the Academic Honor Code at all times. In addition, I understand my options for reporting honor violations as detailed in the code.
AbstractIn lab experiment 25 completed on March 31, a metal oxalate complex of cobalt was made. In this experiment, a solution of KMnO4was standardized with a primary standard of Na2C2O4. This potassium permanganate was then used as a titrant to calculate the weight percent of oxalate in the complex. It was found that the measured mass percent of oxalate was greater than the theoretical mass percent. This indicates that errors occurred somewhere in the process of making the metal oxalate or during the redox titration preformed in this experiment. IntroductionThe titrant in this experiment was made by creating an approximate 0.01 molar solution using distilled water and about 0.474g of KMnO4. This titrant was then used with a primary standard (sodium oxalate) to calculate the exact molarity. Then the known concentration of titrant and volume during the titration of the cobalt complex was used with the balanced chemical reaction to calculate the moles of oxalate at the end point which could then be used to calculate the weight percent of oxalate in the cobalt complex. The balanced reaction is as follows:2−¿+8H2O+10CO22−¿→2Mn¿−¿+5C2O4¿+¿+2MnO4¿10H¿