1. Copper (II) sulphate pentahydrate, CuSO4*5H2O, has 5 moles ofwater for each mole of CuSO4 in the solid crystal. The molar massfor the pentahydrate is 249.68 g/mol. Copper (II) sulphate withoutwater in the crystal structure is called anhydrous, and would havemolar mass of 159.61 g/mol. How many grams of CuSO4*5H2O should bedissolved in a volume of 500.0 mL to make 8.00 mM Cu2+?

2. An iron ore is analyzed for iron content by dissolving inacid, converting the iron to Fe²⁺, and then titratingwith standard 0.0150 M K₂Cr₂O₇solution. If 35.6 mL is required to titrate the iron in a 1.68 gsample, how much Fe²⁺ is in the sample?

The titration reaction is: 6Fe²⁺ + Cr₂O₇^2- + 14H⁺