Problem- 1. Copper (II) sulphate pentahydrate, CuSO4*5H2O, has 5 moles of water for each mole of CuSO4 in the solid crystal. The molar mass for the pentahydrate is 249.68 g/mol. Copper (II) sulphate without water in the crystal structure is called anhydrous, and would have molar mass of 159.61 g/mol. How many grams of CuSO4*5H2O should be dissolved in a volume of 500.0 mL to make 8.00 mM Cu2+?
2. An iron ore is analyzed for iron content by dissolving in acid, converting the iron to Fe2+, and then titrating with standard 0.0150 M K2Cr2O7 solution. If 35.6 mL is required to titrate the iron in a 1.68 g sample, how much Fe2+ is in the sample?
The titration reaction is: 6 Fe2+ + Cr2O72- + 14 H+ à 6 Fe3+ + 2 Cr3+ + 7 H2O.
Please explain above problem in step by step manner so I can easily understand it