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Experiment #26Redox Titration of Metal OxalateCompounds with PermanganateLayla GhaziJoe CantatoreApril 12, 2016CHEM 1212KSection A-27TA: Thaige GompaHonor Pledge – Freshman Chemistry LaboratoriesI did not copy any portion of this work from the work of other students,old lab reports, or unreferenced materials. I understand that such activityis a violation of the Georgia Tech Honor Code.______________________________________Signature
IntroductionA titration is a procedure used to calculate the unknown concentration of a solution by titrating, or adding a volume, of a known concentration. A redox titration is used to determine theconcentration of a specific ion, which in this case was oxalate, in a solution. In the following experiment, the redox titration given by the reaction was used to calculate the concentration of oxalate in a metal oxalate compound: 2+¿(aq)+10CO2(g)+8H2O(l)+¿(aq)→2M n¿−¿(aq)+16H¿2−¿(aq)+2MnO4¿5C2O4¿The oxalate, which was obtained from the sodium oxalate, was oxidized, and the permanganate, which was obtained from the potassium permanganate, was reduced and served as the titrant. The calculated theoretical weight percent of oxalate in Potassium tris(oxalate)ferrate (III) Trihydrate was 53.78%, so it should be expected that the calculated weight percent of oxalate be at least 50%, especially if the reaction is accurate and precise. The work undertaken by this experiment is important for further understanding the nature of redox reactions, and for practicing the calculation of an unknown concentration.