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Copper ii nitrate is soluble in water and aqueous ammonia.
Cu(NO3)2 is a blue-green inorganic salt with the formula (C2H5O2)2, which has an electronic configuration of d9. Its labile nature is due to the repulsion between the oxygen atoms of its nitrate anion and the copper sphere in its center.
It is an excellent reagent in chemical voltaic cells and has many uses in organic synthesis, including the oxidative coupling of 2, 6-dimethylphenol to produce a polymer that is an important engineering material. It also catalyzes the solvent-free synthesis of 3-aminopropenones and 3-aminopropenoates.
The hydrates of cupric nitrate are crystalline and sublime in a vacuum at 150-200 degC. They form blue solids and hygroscopic salts that absorb and emit nitrogen oxide gas.
They can be prepared by reacting metallic copper with nitric acid. They are a strong oxidant and may ignite combustible materials, which is why they should be used carefully!
This salt is soluble in aqueous ammonia and can be used to separate metal ions. This test is very sensitive and requires stoichiometric quantities of ammonia.
Another common copper ii nitrate reaction is with potassium ferrocyanide, in which it reacts stoichiometrically with aqueous sodium hydroxide to precipitate light blue Cu(OH)2 and some basic salts. This is an excellent reagent to demonstrate chemical voltaic cells and is very useful in science fairs, where it shows the ability of copper metal to reduce silver ions.
As with all other nitrates, it is very toxic and should be avoided by children. It is corrosive and can cause severe burns, so always wear gloves and eye protection when handling it!