The chemistry of copper(II) is mainly summarised from elsewhere on the site with links available to more detailed explanations. The page also covers some simple copper(I) chemistry. Reactions of copper(II) ions in solution The simplest ion that copper forms in 2
Put 2 spatulas of copper(II) oxide into the tube and spread it out as much as possible. Weigh the tube again with the copper oxide in it (mass 2). Assemble the apparatus as shown in the diagram but do not place the Bunsen burner underneath yet.
When all the copper(II) oxide has been added continue to heat gently for 1–2 minutes to ensure reaction is complete. Then turn out the Bunsen burner. It may be wise to check (using pH or litmus paper) that no acid remains.
Recovering: Copper oxide containing wastes can be concentrated through the use of ion exchange reverse osmosis or evaporators to the point where copper can be electrolytically removed and sent to a reclaiming firm. If recovery is not feasible the copper can be precipitated through the use of caustics and the sludge deposited in a chemical waste landfill.
Copper(II) oxide or cupric oxide is the inorganic compound with the formula CuO. A black solid it is one of the two stable oxides of copper the other being Cu 2 O or copper(I) oxide (cuprous oxide). As a mineral it is known as tenorite.It is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.