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Chemical compound From Wikipedia, the free encyclopedia
Cobalt nitrate is the inorganic compound with the formula Co(NO3)2.xH2O. It is cobalt(II)'s salt. The most common form is the hexahydrate Co(NO3)2·6H2O, which is a red-brown deliquescent salt that is soluble in water and other polar solvents.[2]
_Nitrate.jpg) Hexahydrate | |
| Names | |
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| Other names
Cobaltous nitrate Nitric acid, cobalt(2+) salt | |
| Identifiers | |
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3D model (JSmol) |
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.030.353 |
| EC Number |
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PubChem CID |
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| RTECS number |
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| UNII | |
| UN number | 1477 |
CompTox Dashboard (EPA) |
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| Properties | |
| Co(NO3)2(H2O)6 | |
| Molar mass | 291.03 g/mol (hexahydrate) 182.943 g/mol (anhydrous) |
| Appearance | pale red powder (anhydrous) red crystalline (hexahydrate) |
| Odor | odorless |
| Density | 1.87 g/cm3 (hexahydrate) 2.49 g/cm3 (anhydrous) |
| Melting point | 100 °C (212 °F; 373 K) decomposes (anhydrous) 55 °C (hexahydrate) |
| Boiling point | 100 to 105 °C (212 to 221 °F; 373 to 378 K) decomposes (anhydrous)[citation needed] 74 °C, decomposes (hexahydrate) |
| anhydrous:[1] 84.03 g/100 mL (0 °C) 334.9 g/100 mL (90 °C) soluble (anhydrous) | |
| Solubility | soluble in alcohol, acetone, ethanol, ammonia (hexahydrate), methanol 2.1 g/100 mL |
| Structure | |
| monoclinic (hexahydrate) | |
| Hazards | |
| GHS labelling: | |
  | |
| Danger | |
| H317, H334, H341, H350, H360, H410 | |
| P201, P202, P261, P272, P273, P280, P281, P285, P302+P352, P304+P341, P308+P313, P321, P333+P313, P342+P311, P363, P391, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
434 mg/kg; rat, oral (anhydrous) 691 mg/kg; rat, oral (hexahydrate) |
| Safety data sheet (SDS) | Cobalt (II) Nitrate MSDS |
| Related compounds | |
Other anions |
Cobalt(II) sulfate Cobalt(II) chloride Cobalt oxalate |
Other cations |
Iron(III) nitrate Nickel(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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As well as the anhydrous compound Co(NO3)2, several hydrates of cobalt(II) nitrate exist. These hydrates have the chemical formula Co(NO3)2·nH2O, where n = 0, 2, 4, 6.
Anhydrous cobalt(II) nitrate adopts a three-dimensional polymeric network structure, with each cobalt(II) atom approximately octahedrally coordinated by six oxygen atoms, each from a different nitrate ion. Each nitrate ion coordinates to three cobalts.[3] The dihydrate is a two-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding holding the layers together.[4] The tetrahydrate consists of discrete, octahedral [(H2O)4Co(NO3)2] molecules. The hexahydrate is better described as hexaaquacobalt(II) nitrate, [Co(OH2)6][NO3]2, as it consists of discrete [Co(OH2)6]2+ and [NO3]− ions.[5] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.[2]
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It is commonly reduced to metallic high purity cobalt.[2] It can be absorbed on to various catalyst supports for use in Fischer–Tropsch catalysis.[6] It is used in the preparation of dyes and inks.[7]
Cobalt(II) nitrate is a common starting material for the preparation of coordination complexes such as cobaloximes,[8] carbonatotetraamminecobalt(III),[9] and others.[10]
The hexahydrate is prepared treating metallic cobalt or one of its oxides, hydroxides, or carbonate with nitric acid:
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