Preparation of hydrated Copper(II) Sulphate Crystals?

Question

(a) You were asked to prepare a pure dry sample of hydrated copper (II) sulphate crystals, starting with copper (II) oxide and 100 cm³ sulphuric acid of concentration 1.0 mol dm‾ ³.
(i) Describe how, using the usual laboratory apparatus, you would prepare this sample. Write an equation for the reaction occuring. Calculate the mass of copper sulphate crystals you would expect to obtain from the preparation.
(Relative atomic mass: Cu = 64; S = 32; O = 16; H = 1)
(ii) The supply of copper (II) oxide ran out. The teacher suggested that copper oxide could be prepared by heating either copper nitrate (a deliquescent* compound) or copper (II) carbonate (a fine powder).
Which of the these two compounds is more suitable for the preparation of copper oxide? Give ONE reason for your choice.
Write balanced equations for the action of heat on a) copper (II) nitrate and b) copper (II) carbonate.
(*Deliquescent means the compound absorbs moisture from the atmosphere and dissolves in it.)

Answer 1

CuO + H2SO4 -> CuSO4 + H2O

CuCO3 (Decomposes more easily)

CuNO3.2H2O -> CuO + NO2 + 2 H2O

CuCO3 -> CuO + CO2

Answer 2

Take a sample out of the solution and put in an evaporating dish. Heat the dish slowly, and not too hot, till the liquid is *almost* gone. Cover the dish, and let it sit. The crystals will be a mixture of hydrated and non-hydrated ZnSO4 in equilibrium with each other and the atmosphere around them.