3. (part a). You are given 0.104 g of a sample of KwFex(C204),(H20)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C2O4)2- in the sample. Please show all of your detailed calculations. (part b). Calculate the mass and moles of [C2O4)2- that is present in a 100. gram sample of Kw Fe (C2O4)/(H20)z. Please show all of your detailed calculations. 4. Normally, the volume of a buret is measured by reading the bottom of the meniscus. For this experiment, why is the top of the meniscus is read and recorded to determine the volume in the buret? Explain your reasoning concisely. 5. In this experiment you will be heating the solution containing KwFex(C2O4)(H20)z to about 60 .C before doing the titration with a KMnO4 solution. Give two reasons for heating the solution to 60 oC for the analysis. 6. The following data were collected for two different experiments. For each experiment, 0.100 g of KwFex(C204)/(H2O)z was used. Experiment 1: Titration of oxalate ion with 0.0100 M KMnO4. For this titration, 26.1 mL of 0.0100M KMnO4 was needed to reach the stoichiometric point. The balanced equation for the titration is 2[MnO4]- (aq) + 5[C204)2- (aq) + 16H+(aq) 2Mn2+ (aq) +10CO2 (g) + 8H20 (1) Experiment 2: From a spectrophotometric analysis measurement (completed in experiment 39C next week), a mass of 18.2 mg of iron(III) ion was found to be present in a 0.100 g sample. Determine the values of w, x, y and z in KwFex(C204),(H20)z. What is the formula of the coordination complex? Show all of your detailed calculations to support your answers. The molar masses which you will need are: K+ = 39.1 g/mol; Fe3+= 55.85 g/mol; [C2O4)2- = 88.0 g/mol; H20 = 18.0 g/mol