Nickel(II) nitrate
| Names | |
|---|---|
| IUPAC name
Nickel(II) nitrate
| |
| Other names
Nickel bis(nitrate)
Nickel dinitrate Nickelous nitrate | |
| Properties | |
| Ni(NO3)2 (anhydrous) Ni(NO3)2·6H2O (hexahydrate) | |
| Molar mass | 182.703 g/mol (anhydrous) 290.79 g/mol (hexahydrate) |
| Appearance | Turquoise or greenish solid (hydrate) |
| Odor | Odorless |
| Density | 2.05 g/cm3 (hexahydrate) (at 20 °C) |
| Melting point | 56.7 °C (134.1 °F; 329.8 K) (hexahydrate) |
| Boiling point | 136.7 °C (278.1 °F; 409.8 K) (hexahydrate) >200 °C (anhydrous) |
| 94.17 g/100 ml (anhydrous) (20 °C)[1] 243 g/100 ml (hexahydrate) (0 °C) | |
| Solubility | Soluble in ethanol, methanol Slightly soluble in DMSO, ethylene glycol, hydrazine[2] |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (hexahydrate) |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
1,620 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Nickel(II) perchlorate Nickel(II) sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Nickel(II) nitrate is the chemical compound Ni(NO3)2. It is more commonly encountered as hydrate, more exactly the hexahydrate form, Ni(NO3)2·6H2O or [Ni(H2O)6](NO3)2.
Contents
Properties
Chemical
Nickel(II) nitrate reacts with NaOH to yield sodium nitrate and forming a greenish precipitate of nickel(II) hydroxide.
- Ni(NO3)2 + 2 NaOH → 2 NaNO3 + Ni(OH)2 ↓
Physical
Nickel(II) nitrate is a blue-green/turquoise hygroscopic solid. It is soluble in water and low-weight primary alcohols.
Availability
Nickel(II) nitrate is sold by chemical suppliers.
Preparation
Nickel nitrate can be prepared by reacting nickel oxide with nitric acid:
- NiO + 2 HNO3 → Ni(NO3)2 + H2O
This route produces the hexahydrate form. Anhydrous nickel nitrate cannot be produced by heating nickle nitrate hexahydrate, since it decomposes upon heating.
Several routes exist for the preparation of the anhydrous form: Nickel nitrate hexahydrate may be reacted with an excess dinitrogen pentoxide, then gently dried under vacuum.
Another route involves the reaction of nickel tetracarbonyl with dinitrogen tetroxide:[3]
- Ni(CO)4 + 2 N2O4 → Ni(NO3)2 + 2 NO + 4 CO
Projects
- Electrotyping and electroplating nickel
- Preparation of nickel coordination complexes
- Make nickel hydrazine nitrate
- Make nickel catalysts
Handling
Safety
Like other nitrates, nickel(II) nitrate is oxidizing. It is also irritating to the eyes, skin and, upon inhalation of the dust, respiratory tract. Like all nickel compounds, nickel(II) nitrate is a known allergen and carcinogen.
Storage
In closed plastic or glass bottles, away from moisture and combustible materials.
Disposal
Nickel(II) nitrate can be neutralized by precipitating insoluble nickel, either as oxide or some other insoluble form, then taken to waste disposal centers.
References
- ↑ https://en.crystalls.info/Nickel_nitrate
- ↑ IARC. Monographs on the Evaluation of the Carcinogenic Risk of Chemicals to Humans. Geneva: World Health Organization, International Agency for Research on Cancer, 1972-PRESENT. (Multivolume work). Available at: http://monographs.iarc.fr/ENG/Classification/index.php, p. V11 79 (1976)
- ↑ https://onlinelibrary.wiley.com/doi/abs/10.1002/14356007.a17_235.pub2
