The reactions between copper and nitric acid are examples of oxidation-reduction reactions, where gaining electrons reduces one element and losing them oxidises the other. Nitric acid is not only a strong acid, it is an oxidising agent. Therefore, it can oxidise copper to Cu+2. If you plan to experiment with these reactions, it is important to remember that they release toxic, noxious fumes.
Copper can undergo one of two reactions when combined with nitric acid, depending on the concentration of the solution. If the nitric acid is dilute, the copper will be oxidised to form copper nitrate with nitric oxide as a byproduct. If the solution is concentrated, the copper will be oxidised to form copper nitrate with nitrogen dioxide as a byproduct. Both nitric oxide and nitrogen dioxide are noxious and potentially toxic at high levels; nitrogen dioxide is the ugly brown gas present in the smog haze over many cities.
The equations for the two reactions that can take place are: Cu + 4 HNO3 --> Cu(NO3)2 + 2 NO2 + 2 H2O, which produces nitrogen dioxide and
3 Cu + 8 HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O, which produces nitric oxide.
With the concentrated acid, the solution will first turn green, then greenish-brown, and finally blue once diluted with water. Either reaction is highly exothermic and releases energy in the form of heat.
Another way to understand this reaction is by breaking it down into two half-reactions, one for oxidation (loss of electrons) and the other for reduction (gain of electrons). The half-reactions are: Cu --> Cu+2 + 2 e- , meaning that copper loses two electrons, and 2 e- + 4 HNO3 ---> 2 NO3 -1 + 2 H2O, which shows that two electrons have been transferred to the products. The speed of this reaction depends on the surface area of the copper; copper wire will react more quickly than copper bars, for example.
The solution changes colour because of the water. Unlike the copper solid, the copper ions in solution can form a type of interaction called a coordination complex with the water molecules, and these complexes lend the solution a blue colour. Mineral acids like hydrochloric acid do not oxidise copper in the same way as nitric acid because they are not strong oxidising agents. Sulphuric acid, however, is a strong oxidising agent. Under the right conditions, it will react with copper to release sulphur dioxide gas.