Cobalt(II) carbonate

Cobalt(II) carbonate is the inorganic compound with the formula CoCO3. This reddish paramagnetic solid is an intermediate in the hydrometallurgical purification of cobalt from its ores. It is an inorganic pigment, and a precursor to catalysts.[4] Cobalt(II) carbonate also occurs as the rare red/pink mineral spherocobaltite.[5]

Cobalt(II) carbonate
Names
IUPAC name
Cobalt(II) carbonate
Other names
Cobaltous carbonate; cobalt(II) salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.007.428
UNII
Properties
CoCO3
Molar mass 118.941 g/mol
Appearance red/ pink crystals (anhydrous)
pink, violet, red crystalline powder (hexahydrate)
Density 4.13 g/cm3
Melting point 427 °C (801 °F; 700 K) [1]
decomposes before melting to cobalt(II) oxide (anhydrous)
140 °C (284 °F; 413 K)
decomposes (hexahydrate)
Cobalt (II) Carbonate is insoluble in distilled water.
1.0·10−10[2]
Solubility soluble in acid
negligible in alcohol, methyl acetate
insoluble in ethanol
1.855
Structure
Rhombohedral (anhydrous)
Trigonal (hexahydrate)
Thermochemistry
79.9 J/mol·K[1]
Std enthalpy of
formation (ΔfH⦵298)
 −722.6 kJ/mol[1]
-651 kJ/mol[1]
Hazards
GHS pictograms [3]
GHS Signal word Warning
GHS hazard statements
 H302, H315, H317, H319, H335, H351[3]
P261, P280, P305+351+338[3]
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
2
0
Lethal dose or concentration (LD, LC):
640 mg/kg (oral, rats)
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

Preparation and structure

It is prepared by combining solutions cobaltous sulfate and sodium bicarbonate:

CoSO4 + 2 NaHCO3 → CoCO3 + Na2SO4 + H2O + CO2

CoCO3 adopts a structure like calcite, consisting of cobalt in an octahedral coordination geometry.[6]

Reactions

Heating the carbonate, proceeds in a typical way for calcining, except that the material is partially oxidized:

6 CoCO3 + O2 → 2Co3O4 + 6 CO2

The resulting Co3O4 converts reversibly to CoO at high temperatures.[7] Like most transition metal carbonates, cobalt carbonate is insoluble in water, but is readily attacked by mineral acids:

CoCO3 + 2 HCl + 5 H2O → [Co(H2O)6]Cl2 + CO2

It is used to prepare many coordination complexes. The reaction of cobalt(II) carbonate and acetylacetone in the presence of hydrogen peroxide gives tris(acetylacetonato)cobalt(III).[8] These complexes are chiral and often can be resolved into the individual enantiomers.

Uses

Cobalt carbonate is a precursor to cobalt carbonyl and various cobalt salts. It is a component of dietary supplements since cobalt is an essential element. It is a precursor to blue pottery glazes, famously in the case of Delftware.

Natural occurrence

The moderately rare spherocobaltite is the natural form of cobalt carbonate, with good specimens coming especially from the Republic of Congo. Cobaltocalcite is a cobaltiferous calcite variety that is quite similar in habit to spherocobaltite.[5]

Safety

The compound is harmful if swallowed, and irritating to eyes and skin.

References
  1. http://chemister.ru/Database/properties-en.php?dbid=1&id=573
  2. "Archived copy". Archived from the original on 2012-06-15. Retrieved 2012-05-17.CS1 maint: archived copy as title (link)
  3. Sigma-Aldrich Co., Cobalt(II) carbonate. Retrieved on 2014-05-06.
  4. John Dallas Donaldson, Detmar Beyersmann, "Cobalt and Cobalt Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a07_281.pub2
  5. "Spherocobaltite: Spherocobaltite mineral information and data". www.mindat.org. Retrieved 7 August 2018.
  6. Pertlik, F. (1986). "Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate". Acta Crystallographica Section C. 42: 4–5. doi:10.1107/S0108270186097524.
  7. G.A. El-Shobaky, A.S. Ahmad, A.N. Al-Noaimi and H.G. El-Shobaky Journal of Thermal Analysis and Calorimetry 1996, Volume 46, Number 6 , pp.1801-1808. online abstract
  8. Bryant, Burl E.; Fernelius, W. Conard (1957). "Cobalt(III) Acetylacetonate". Inorganic Syntheses. pp. 188–189. doi:10.1002/9780470132364.ch53. ISBN 9780470132364.
Carbonates
H2CO3 He
Li2CO3,
LiHCO3		 BeCO3 B C (NH4)2CO3,
NH4HCO3		 O F Ne
Na2CO3,
NaHCO3,
Na3H(CO3)2		 MgCO3,
Mg(HCO3)2		 Al2(CO3)3 Si P S Cl Ar
K2CO3,
KHCO3		 CaCO3,
Ca(HCO3)2		 Sc Ti V CrCO3,
Cr2(CO3)3		 MnCO3 FeCO3 CoCO3,
Co2(CO3)3		 NiCO3 Cu2CO3,
CuCO3		 ZnCO3 Ga Ge As Se Br Kr
Rb2CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh PdCO3 Ag2CO3 CdCO3 In Sn Sb Te I Xe
Cs2CO3,
CsHCO3		 BaCO3   Hf Ta W Re Os Ir Pt Au HgCO3 Tl2CO3 PbCO3 (BiO)2CO3 Po(CO3)2 At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La2(CO3)3 Ce2(CO3)3 Pr2(CO3)3 Nd2(CO3)3 Pm2(CO3)3 Sm2(CO3)3 EuCO3,
Eu2(CO3)3		 Gd2(CO3)3 Tb2(CO3)3 Dy2(CO3)3 Ho2(CO3)3 Er2(CO3)3 Tm2(CO3)3 Yb2(CO3)3 Lu2(CO3)3
Ac Th(CO3)2 Pa UO2CO3 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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