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Nickel nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. The anhydrous form is not commonly encountered, thus "nickel nitrate" usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways: Ni(NO3)2.6H2O and, more descriptively [Ni(H2O)6](NO3)2. The latter formula indicates that the nickel(II) center is surrounded by six water molecules in this hydrated salt. In the hexahydrate, the nitrate anions are not bonded to nickel. Also known are three other hydrates: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O. Anhydrous Ni(NO3)2 is also known.[2]

Nickel(II) nitrate
Nickel(II) nitrate
Nickel(II) nitrate
IUPAC name
Nickel(II) nitrate
Other names
Nickel nitrate
Nickelous nitrate
Nitric acid, nickel(2+) salt
3D model (JSmol)
ECHA InfoCard 100.032.774
EC Number 238-076-4
Molar mass 182.703 g/mol (anhydrous)
290.79 g/mol (hexahydrate)
Appearance emerald green hygroscopic solid
Odor odorless
Density 2.05 g/cm3 (hexahydrate)
Melting point 56.7 °C (134.1 °F; 329.8 K) (hexahydrate)
Boiling point 136.7 °C (278.1 °F; 409.8 K) (hexahydrate)
243 (hexahydrate) g/100ml (0 °C)[1]
Solubility soluble in ethanol
+4300.0·10−6 cm3/mol (+6 H2O)
1.422 (hexahydrate)
monoclinic (hexahydrate)
Safety data sheet External MSDS
Oxidant (O)
Carc. Cat. 1
Muta. Cat. 3
Repr. Cat. 2
Toxic (T)
Harmful (Xn)
Irritant (Xi)
Dangerous for the environment (N)
R-phrases (outdated) R49, R61, R8, R20/22, R38, R41, R42/43, R48/23, R68, R50/53
S-phrases (outdated) S53, S45, S60, S61
NFPA 704
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1620 mg/kg (oral, rat)
Related compounds
Other anions
Nickel(II) sulfate
Nickel(II) chloride
Other cations
Palladium(II) nitrate
Related compounds
Cobalt(II) nitrate
Copper(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

It is prepared by the reaction of nickel oxide with nitric acid:

NiO + 2 HNO3 + 5 H2O → Ni(NO3)2.6H2O

The anhydrous nickel nitrate is typically not prepared by the heating the hydrates. Rather is generated by reaction of hydrates with dinitrogen pentoxide or of nickel carbonyl with dinitrogen tetroxide:[2]

Ni(CO)4 + 2 N2O4 → Ni(NO3)2 + 2 NO + 4 CO

The hydrated nitrate is often used as a precursor to supported nickel catalysts.


Like other nitrates, nickel nitrate is oxidizing. It is also irritating to the eyes, skin and, upon inhalation of the dust, respiratory tract. It may cause skin allergy. Nickel nitrate is a carcinogen, along with most other nickel compounds. The nickel ion is also toxic to aquatic organisms.


Nickel(II) nitrate is used as the precursor for the explosive Nickel Hydrazine Nitrate, which is used as lead-free and safer alternative to Lead Azide and Lead Styphnate.


  1. ^ Perry's Chem Eng Handbook, 7th Ed
  2. ^ a b Keith Lascelles, Lindsay G. Morgan, David Nicholls, Detmar Beyersmann, "Nickel Compounds" in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a17_235.pub2
Salts and covalent derivatives of the nitrate ion