(40 points) In a laboratory experiment you react 20.0 mL of 25% by mass C2H8N2 with 8.000 g of NiCl2.6H2O to obtain the product Ni(NH2CH2CH2NH2)3Cl2 complex. The C2H8N2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NiCl2.6H2O= 237.69 g/mole, MW C2H8N2=60.10 g/mole, MW tris(ethylenediamine)nickel(II)chloride = 309.89 g/mole)

A)Write down the balanced equation of the synthesis. (10 points)

B) Determine the number of moles of each reactant that you use. (10 points)

C) Determine the number of moles of each reactant that you use. (10 points)

D)Calculate your percent yield if the dry product weighs 7.000 g. (15 points)

3)(40 points) In a chemistry experiment you titrate a sample of K2C2O4 with a standard KMnO4 solution in acidic environment.

A)a. Balance the following redox reaction, showing all your work (and the half reactions if needed). (14 points)

___ K2C2O4 + ___ H2SO4 + ___ KMnO4 ! ___ MnSO4 + ___ CO2 + ___ H2O + ___ K2SO4

B)Which one is the oxidizing agent and which one is the reducing agent? Explain why? (6 points)

C)c. If you used 6.0 ml of 0.01 M KMnO4 to reach the end point in the titration of a 15.0 ml sample of K2C2O4, determine the molarity (in M) of the K2C2O4 sample you used. (20 points)