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The metal oxalates used in this experiment are coordinate complexes because they have coordinate covalent bonds. Oxalate is the ligand and acts as a Lewis acid. It donates electrons which allows for a redox reaction with the permanganate solution to occur. The solution of potassium permanganate was standardized in part A by titrating it against a solution of sodium oxalate with a known concentration and volume. The analyte solution was heated to guarantee that the solute was completely dissolved in the solvent before it reacted with the permanganate solution. The measured concentrations of the permanganate solutions were 0.00972M and 0.0102M for trial 1 and 2, respectively. The average of the permanganate concentrations was 0.00996 M with a standard deviation of 3.41x10-4, which shows that our measured concentrationswere quite precise. Some errors could be due to the sodium oxalate not being completely dissolved in the solution from lack of heating and mixing, which would cause an improper calculation of the concentration of permanganate.The permanganate in the titration and the coefficients of the chemical reaction allowed for the mass of oxalate from the metal oxalate compound in solution to be calculated. Comparingthe mass of oxalate and initial mass of the metal oxalate compound allowed for the calculation ofthe weight percent of oxalate. The mean value of the weight percent of oxalate was 48.5% with a
standard deviation of 0.566. The small standard deviation shows that the measurements were quite precise. Since the percent error, which was .831%, was quite low our results were also