Cobalt(II) sulfate

Cobalt(II) sulfate is any of the inorganic compounds with the formula CoSO₄(H₂O)_x. Usually cobalt sulfate refers to the hydrate CoSO₄^.7H₂O, which is one of the most commonly available salts of cobalt.

Cobalt(II) sulfate

Names
IUPAC name Cobalt(II) sulfate
Other names Colbaltous sulfate
Identifiers
CAS Number	10124-43-3^Y 13455-64-0 (monohydrate)^N 10026-24-1 (heptahydrate)^N
3D model (JSmol)	Interactive image
ChEBI	CHEBI:53470^Y
ChemSpider	23338^Y
ECHA InfoCard	100.030.291
EC Number	233-334-2
KEGG	C17383 C19215 (heptahydrate)
PubChem CID	24965
RTECS number	GG3100000 (anhydrous) GG3200000 (heptahydrate)
UNII	H7965X29HX^Y
CompTox Dashboard (EPA)	DTXSID1031042
InChI InChI=1S/Co.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2^Y Key: KTVIXTQDYHMGHF-UHFFFAOYSA-L^Y InChI=1/Co.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Key: KTVIXTQDYHMGHF-NUQVWONBAJ
SMILES [Co+2].[O-]S([O-])(=O)=O
Properties
Chemical formula	CoSO4·(H2O)7
Molar mass	154.996 g/mol (anhydrous) 173.01 g/mol (monohydrate) 263.08 g/mol (hexahydrate) 281.103 g/mol (heptahydrate)
Appearance	reddish crystalline (anhydrous, monohydrate) pink salt (hexahydrate)
Odor	odorless (heptahydrate)
Density	3.71 g/cm^3 (anhydrous) 3.075 g/cm^3 (monohydrate) 2.019 g/cm^3 (hexahydrate) 1.948 g/cm^3 (heptahydrate)
Melting point	735 °C (1,355 °F; 1,008 K)
Solubility in water	anhydrous: 36.2 g/100 mL (20 °C) 38.3 g/100 mL (25 °C) 84 g/100 mL (100 °C) heptahydrate: 60.4 g/100 mL (3 °C) 67 g/100 mL (70 °C)
Solubility	anhydrous: 1.04 g/100 mL (methanol, 18 °C) insoluble in ammonia heptahydrate: 54.5 g/100 mL (methanol, 18 °C)
Magnetic susceptibility (χ)	+10,000·10^−6 cm^3/mol
Refractive index (nD)	1.639 (monohydrate) 1.540 (hexahydrate) 1.483 (heptahydrate)
Structure
Crystal structure	orthorhombic (anhydrous) monoclinic (monohydrate, heptahydrate)
Hazards
Safety data sheet	JT Baker MSDS
GHS pictograms
GHS Signal word	Danger
GHS hazard statements	H302, H317, H334, H341, H350, H360, H400, H410
GHS precautionary statements	P201, P202, P261, P264, P270, P272, P273, P280, P281, P285, P301+312, P302+352, P304+341, P308+313, P321, P330, P333+313, P342+311, P363, P391, P405, P501
NFPA 704 (fire diamond)	0 2 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	424 mg/kg (oral, rat)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is ^YN ?)
Infobox references

Properties, preparation, and structure

Cobalt sulfate heptahydrate under a microscope.

Cobalt(II) sulfate heptahydrate appears as red monoclinic crystals that liquify around 100 °C and become anhydrous at 250 °C. It is soluble in water, slightly soluble in ethanol, and especially soluble in methanol. The salts are paramagnetic.

It forms by the reaction of metallic cobalt, its oxide, hydroxide, or carbonate with aqueous sulfuric acid.[1]

The hexahydrate is a metal aquo complex consisting of octahedral [Co(H₂O)₆]²⁺ ions associated with sulfate anions.[2]

Uses

Cobalt is obtained from ores via the sulfate in many cases.[1][3]

Hydrated cobalt(II) sulfate is used in the preparation of pigments, as well as in the manufacture of other cobalt salts. Cobalt pigment is used in porcelains and glass. Cobalt(II) sulfate is used in storage batteries and electroplating baths, sympathetic inks, and as an additive to soils and animal feeds. For these purposes, the cobalt sulfate is produced by treating cobalt oxide with sulfuric acid.[1]

Health issues

Cobalt is an essential mineral for mammals, but more than a few milligrams each day is harmful. Although poisonings have rarely resulted from cobalt compounds, their chronic ingestion has caused serious health problems at doses far less than the lethal dose. In 1966, the addition a cobalt compound to stabilize beer foam in Canada led to a peculiar form of toxin-induced cardiomyopathy, which came to be known as beer drinker's cardiomyopathy.[4][5][6]

Furthermore, cobalt(II) sulfate is suspected of causing cancer (i.e., possibly carcinogenic, IARC Group 2B) as per the International Agency for Research on Cancer (IARC) Monographs. [PDF]

See also

• Chalcanthum

References

1. John D. Donaldson, Detmar Beyersmann "Cobalt and Cobalt Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a07_281.pub2
2. Elerman, Y. "Refinement of the crystal structure of CoSO₄*6H₂O" Acta Crystallographica Section C 1988, volume 44, p599-p601. doi:10.1107/S0108270187012447
3. Rarely, cobalt(II) sulfate is found in form of few crystallohydrate minerals, occurring among oxidation zones containing primary Co minerals (like skutterudite or cobaltite). These minerals are: biebierite (heptahydrate), moorhouseite (Co,Ni,Mn)SO₄^.6H₂O, aplowite (Co,Mn,Ni)SO₄^.4H₂O and cobaltkieserite (monohydrate).
4. Morin Y; Tětu A; Mercier G (1969). "Quebec beer-drinkers' cardiomyopathy: Clinical and hemodynamic aspects". Annals of the New York Academy of Sciences. 156 (1): 566–576. Bibcode:1969NYASA.156..566M. doi:10.1111/j.1749-6632.1969.tb16751.x. PMID 5291148.
5. Barceloux, Donald G. & Barceloux, Donald (1999). "Cobalt". Clinical Toxicology. 37 (2): 201–216. doi:10.1081/CLT-100102420. PMID 10382556.
6. 11.1.5 The unusual type of myocardiopathy recognized in 1965 and 1966 in Quebec (Canada), Minneapolis (Minnesota), Leuven (Belgium), and Omaha (Nebraska) was associated with episodes of acute heart failure (e/g/, 50 deaths among 112 beer drinkers).