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Cobalt(II) nitrate

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Cobalt(II) nitrate
Cobalt (II) Nitrate Hexahydrate Sample
Cobalt (II) Nitrate Hexahydrate Sample
Hexahydrate
Names
Other names Cobaltous nitrate
Nitric acid, cobalt(2+) salt
Identifiers
CAS Number
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.353 Edit this at Wikidata
EC Number
  • 233-402-1
PubChem CID
RTECS number
  • GG1109000
UNII
UN number 1477
CompTox Dashboard (EPA)
InChI
  • InChI=1S/Co.2NO3/c;2*2-1(3)4/q+2;2*-1Key: UFMZWBIQTDUYBN-UHFFFAOYSA-N
  • InChI=1/Co.2NO3/c;2*2-1(3)4/q+2;2*-1Key: UFMZWBIQTDUYBN-UHFFFAOYAS
SMILES
  • .()=O.()=O
Properties
Chemical formula 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/cm (hexahydrate)
2.49 g/cm (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)
74 °C, decomposes (hexahydrate)
Solubility in water anhydrous: 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
Coordination geometry monoclinic (hexahydrate)
Hazards
GHS labelling:
Pictograms GHS07: Exclamation markGHS09: Environmental hazard
Signal word Danger
Hazard statements H317, H334, H341, H350, H360, H410
Precautionary statements 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)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2 0 0OX
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 , 100 kPa). ☒N verify (what is  ?) Infobox references
Chemical compound

Cobalt nitrate is the inorganic compound with the formula Co(NO3)2xH2O. 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.

Composition and structures

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. The dihydrate is a two-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding holding the layers together. The tetrahydrate consists of discrete, octahedral molecules. The hexahydrate is better described as hexaaquacobalt(II) nitrate, 2, as it consists of discrete and ions. Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.

  • Co(NO3)2 Co(NO3)2
  • Co(NO3)2·2H2O Co(NO3)2·2H2O
  • Co(NO3)2·4H2O Co(NO3)2·4H2O
  • Co(NO3)2·6H2O Co(NO3)2·6H2O

Uses and reactions

It is commonly reduced to metallic high purity cobalt. It can be absorbed on to various catalyst supports for use in Fischer–Tropsch catalysis. It is used in the preparation of dyes and inks.

Cobalt(II) nitrate is a common starting material for the preparation of coordination complexes such as cobaloximes, carbonatotetraamminecobalt(III), and others.

Production

The hexahydrate is prepared treating metallic cobalt or one of its oxides, hydroxides, or carbonate with nitric acid:

Co + 4 HNO3 + 4 H2O → Co(H2O)6(NO3)2 + 2 NO2
CoO + 2 HNO3 + 5 H2O → Co(H2O)6(NO3)2
CoCO3 + 2 HNO3 + 5 H2O → Co(H2O)6(NO3)2 + CO2

References

  1. Perrys' Chem Eng Handbook, 7th Ed
  2. ^ 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
  3. Tikhomirov, G. A.; Znamenkov, K. O.; Morozov, I. V.; Kemnitz, E.; Troyanov, S. I. (2002). "Anhydrous Nitrates and Nitrosonium Nitratometallates of Manganese and Cobalt, M(NO3)2, NO[Mn(NO3)3], and (NO)2[Co(NO3)4]: Synthesis and Crystal Structure". Z. anorg. allg. Chem. 628 (1): 269–273. doi:10.1002/1521-3749(200201)628:1<269::AID-ZAAC269>3.0.CO;2-P.
  4. Ribár, B.; Milinski, N.; Herak, R.; Krstanovič, I.; Djurič, S. (1976). "The Crystal Structure of Cobalt Nitrate Dihydrate, Co(NO3)2·2H2O". Zeitschrift für Kristallographie. 144 (1–6): 133–138. Bibcode:1976ZK....144..133R. doi:10.1524/zkri.1976.144.1-6.133.
  5. Prelesnik, P. V.; Gabela, F.; Ribar, B.; Krstanovic, I. (1973). "Hexaaquacobalt(II) nitrate". Cryst. Struct. Commun. 2 (4): 581–583.
  6. Ernst B, Libs S, Chaumette P, Kiennemann A. Appl. Catal. A 186 (1-2): 145-168 1999
  7. Lewis, Richard J., Sr. (2002). Hawley's Condensed Chemical Dictionary (14th Edition). John Wiley & Sons. http://www.knovel.com/knovel2/Toc.jsp?BookID=704&VerticalID=0
  8. Schrauzer, G. N. (1968). Bis(Dimethylglyoximato)Cobalt Complexes: ("Cobaloximes"). Inorganic Syntheses. pp. 61–70. doi:10.1002/9780470132425.ch12. ISBN 9780470132425.
  9. Schlessinger, G. (1960). "Carbonatotetramminecobalt(III) Nitrate". Inorganic Syntheses. 6: 173–175. doi:10.1002/9780470132371.ch55. ISBN 9780470132371.
  10. Hargens, Robert D.; Min, Woonza; Henney, Robert C. (1973). "Bis(ethylenediamine)sulfito Complexes of Cobalt(III)". Inorganic Syntheses. Inorganic Syntheses. pp. 77–81. doi:10.1002/9780470132456.ch15. ISBN 9780470132456.
Cobalt compounds
Cobalt(I)
Cobalt(II)
Cobalt(0,III)
Cobalt(II,III)
Cobalt(III)
Cobalt(III,IV)
Cobalt(IV)
Cobalt(V)
Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)−4 RONO2
+CO3
+C2O4 		NO3
NH4NO3 		HOONO2 FNO3
+F 		Ne
NaNO3 Mg(NO3)2 Al(NO3)3
Al(NO3)−4 		Si P +SO4 ClONO2
+Cl 		Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)2
Fe(NO3)3 		Co(NO3)2
Co(NO3)3 		Ni(NO3)2 CuNO3
Cu(NO3)2 		Zn(NO3)2 Ga(NO3)3 Ge As +SeO3 BrNO3
+Br 		Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 NbO(NO3)3 MoO2(NO3)2 Tc Ru Rh(NO3)3 Pd(NO3)2 AgNO3 Cd(NO3)2 In(NO3)3 Sn(NO3)4 Sb4O4(OH)2(NO3)2 Te INO3
+IO3 		Xe(NO3)2
CsNO3 Ba(NO3)2 * Lu(NO3)3 Hf(NO3)4 TaO(NO3)3 WO2(NO3)2 ReO3NO3 Os Ir3O(NO3)10 Pt Au(NO3)−4 Hg2(NO3)2
Hg(NO3)2 		TlNO3
Tl(NO3)3 		Pb(NO3)2 Bi(NO3)3
BiO(NO3) 		Po(NO3)4 At Rn
FrNO3 Ra(NO3)2 ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* La(NO3)3 Ce(NO3)3
Ce(NO3)4 		Pr(NO3)3 Nd(NO3)3 Pm(NO3)3 Sm(NO3)3 Eu(NO3)3 Gd(NO3)3 Tb(NO3)3 Dy(NO3)3 Ho(NO3)3 Er(NO3)3 Tm(NO3)3 Yb(NO3)3
** Ac(NO3)3 Th(NO3)4 PaO(NO3)3 UO2(NO3)2 Np(NO3)4 Pu(NO3)4 Am(NO3)3 Cm(NO3)3 Bk(NO3)3 Cf(NO3)3 Es Fm Md No
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