Cobalt(II) acetate
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| Template:Longitem | Co(C2H3O2)2 |
| Molar mass | 177.02124 g/mol (anhydrous) 249.08 g/mol (tetrahydrate) |
| Appearance | Pink crystals (anhydrous) intense red crystals (tetrahydrate) |
| Odor | vinegar (tetrahydrate) |
| Density | 1.705 g/cm3 (tetrahydrate) |
| Melting point | Template:Chembox CalcTemperatures |
| Solubility | soluble in alcohol, dilute acids, pentyl acetate (tetrahydrate) |
| Template:Longitem | +11,000·10−6 cm3/mol |
| Template:Longitem | 1.542 (tetrahydrate) |
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Cobalt(II) acetate is the cobalt salt of acetic acid. It is commonly found as the tetrahydrate Co(CH3CO2)2·4 H2O, abbreviated Co(OAc)2·4 H2O. It is used as a catalyst.
Synthesis and structure
Like many other transition metal acetates, cobalt(II) acetate forms by the reaction of cobalt oxide or hydroxide and acetic acid:
- CoO + 2Script error: No such module "String".CH3CO2H + 3Script error: No such module "String".H2O → Co(CH3CO2)2·4 H2O
The tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central cobalt centre being coordinated by four water molecules and two acetate ligands.[1] The analogous nickel acetate is isostructural.[2]
Various hydrates are known including Co(CH3CO2)2·H2O and [Co(CH3CO2)2]5·0.5 H2O. These are coordination polymers:[3]
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Reactions and uses
Cobalt acetate is a precursor to various oil drying agents, catalysts that allow paints and varnishes to harden.[4]
Anhydrous cobalt acetate is a widely used source of cobalt in the synthesis of materials,[5] catalyst,[6] and complexes.[7]
Oxidation of acetic acid solutions of cobalt(II) acetate, e.g. with ozone, gives cobalt(III) acetates, which are strong oxidants.[8]
Safety
Cobalt salts are poisonous.Script error: No such module "Unsubst".
References
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- ↑ John Dallas Donaldson, Detmar Beyersmann, "Cobalt and Cobalt Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. Script error: No such module "CS1 identifiers".
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