Copper nitrate II

Copper (II) nitrate . It is an inorganic chemical compound whose formula is Cu (NO 3 ) 2 . It comes in prismatic blue crystals with a caustic metallic flavor, which crystallize with three water molecules at a temperature of 26 ºC. It is soluble in water and alcohol, both solutions with acid reaction.

Summary

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  • 1 Physical and chemical properties
  • 2 uses
  • 3 Synthesis
  • 4 Health effects
  • 5 Sources

Physical and chemical properties

Copper (II) nitrate is a ternary or oxysalt salt consisting of: 1 copper atom, 2 nitrogen atoms and 6 oxygen atoms.

  • Molar mass: 187.56 g / mol
  • Density: 3.05 g / cm³
  • Boiling point: 170 ° C
  • Melting point: 256 ° C
  • Systematic nomenclature: bis [trioxonitrate (V)] copper
  • Stock nomenclature: copper nitrate (II)
  • Traditional nomenclature: cupric nitrate
  • Type of compound: oxysalts
  • Physical state: solid
  • Color: blue * Odor: nitric * pH value at 50 g / l H2O (20 ºC) = 3-4
  • Non-flammable flash point
  • Low explosion limit not applicable
  • Molar mass: 187.56 g / mol.
  • Boiling point: 170 ° C.
  • Molecular weight: 241.60
  • Stack density ~ 1050 kg / m3
  • Solubility in Water (20 ºC) = 2670 g / l
  • Conditions to avoid: Bumps and friction
  • Strong heating. (May form: oxygen).
  • Materials to avoid: Exothermic reaction with: acetic anhydride.
  • Risk of explosion with: ammonia / amides, cyanide complexes, organic compounds.
  • Sensitive to humidity; removal of crystallization water by heating, strong oxidant.

Applications

Cupric nitrate is used in many applications such as: • Copper source for fertilizers. • In the laboratory and industry to synthesize other compounds.

Synthesis

Hydrated copper nitrate can be prepared by anhydrous hydrolysis or treating metallic copper with aqueous solution of dilute nitric acid or silver nitrate: It is synthesized in two stages, the first the formation of copper carbonate and the following the dissolution of carbonate in nitric acid.

CuSO 4 (aq.) + (NH 4 ) 2CO 3 (aq.) -> CuCO 3 (s.) + (NH 4 ) 2 SO 4 (aq.)

CuCO 3 (s.) + 2HNO 3 (aq.) -> Cu (NO 3 ) 2 (aq.) + H 2 O (l.) + CO 2 (g.)

The copper is separated as a precipitate of copper carbonate in order to be able to obtain at the end of the reaction a reagent as pure as possible without traces of sulfate.

Health effects

Harmful if swallowed. Irritating to eyes and skin. Very toxic to aquatic organisms, may cause long-term adverse effects in the aquatic environment

 

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