Open main menu

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
Calcium-carbonate-xtal-3D-SF.png
Cobalt(II) carbonate powder
Names
IUPAC name
Cobalt(II) carbonate
Other names
Cobaltous carbonate; cobalt(II) salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.007.428
Properties
CoCO3
Appearance red/ pink crystals (anhydrous)
pink, violet, red crystalline powder (hexahydrate)
Density 4.13 g/cm3
Melting point 427 °C (801 °F; 700 K) [2]
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[1]
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[2]
−722.6 kJ/mol[2]
-651 kJ/mol[2]
Hazards
GHS pictograms GHS07: HarmfulGHS08: Health hazard[3]
GHS signal word Warning
H302, H315, H317, H319, H335, H351[3]
P261, P280, P305+351+338[3]
NFPA 704
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 codeNFPA 704 four-colored diamond
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 ☑Y☒N ?)
Infobox references

Preparation and structureEdit

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]

ReactionsEdit

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

UsesEdit

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 occurrenceEdit

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]

SafetyEdit

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

ReferencesEdit

  1. ^ "Archived copy". Archived from the original on 2012-06-15. Retrieved 2012-05-17.CS1 maint: archived copy as title (link)
  2. ^ a b c d http://chemister.ru/Database/properties-en.php?dbid=1&id=573
  3. ^ a b c 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. ^ a b "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

External linksEdit

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 Cr MnCO3 FeCO3 CoCO3 NiCO3 CuCO3 ZnCO3 Ga Ge As Se Br Kr
Rb2CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh Pd Ag2CO3 CdCO3 In Sn Sb Te I Xe
Cs2CO3,
CsHCO3
BaCO3   Hf Ta W Re Os Ir Pt Au Hg Tl2CO3 PbCO3 (BiO)2CO3 Po 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 Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2CO3 Np Pu Am Cm Bk Cf Es Fm Md No Lr