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Cobalt(II) nitrate

Summary

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

Cobalt(II) nitrate
Cobalt (II) Nitrate Hexahydrate Sample
Names
Other names
Cobaltous nitrate
Nitric acid, cobalt(2+) salt
Identifiers
  • 10026-22-9 hexahydrate checkY
  • 10141-05-6 anhydrous
  • 7697-37-2 dihydrate
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:86209 ☒N
ChemSpider
  • 23369 checkY
ECHA InfoCard 100.030.353 Edit this at Wikidata
EC Number
  • 233-402-1
  • 25000
RTECS number
  • GG1109000
UNII
  • 65W79BFD5V checkY
UN number 1477
  • DTXSID9064970 Edit this at Wikidata
  • InChI=1S/Co.2NO3/c;2*2-1(3)4/q+2;2*-1 checkY
    Key: UFMZWBIQTDUYBN-UHFFFAOYSA-N checkY
  • InChI=1/Co.2NO3/c;2*2-1(3)4/q+2;2*-1
    Key: UFMZWBIQTDUYBN-UHFFFAOYAS
  • [Co+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
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/cm3 (hexahydrate)
2.49 g/cm3 (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)[citation needed]
74 °C, decomposes (hexahydrate)
anhydrous:[1] 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
monoclinic (hexahydrate)
Hazards
GHS labelling:
GHS07: Exclamation markGHS09: Environmental hazardGHS09: Environmental hazard
Danger
H317, H334, H341, H350, H360, H410
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)
Lethal dose or concentration (LD, LC):
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 [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Infobox references

Composition and structuresEdit

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.[3] The dihydrate is a two-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding holding the layers together.[4] The tetrahydrate consists of discrete, octahedral [(H2O)4Co(NO3)2] molecules. The hexahydrate is better described as hexaaquacobalt(II) nitrate, [Co(OH2)6][NO3]2, as it consists of discrete [Co(OH2)6]2+ and [NO3]− ions.[5] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.[2]

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

Uses and reactionsEdit

It is commonly reduced to metallic high purity cobalt.[2] It can be absorbed on to various catalyst supports for use in Fischer–Tropsch catalysis.[6] It is used in the preparation of dyes and inks.[7]

Cobalt(II) nitrate is a common starting material for the preparation of coordination complexes such as cobaloximes,[8] carbonatotetraamminecobalt(III),[9] and others.[10]

ProductionEdit

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

ReferencesEdit

  1. ^ Perrys' Chem Eng Handbook, 7th Ed
  2. ^ a b c 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.
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Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)−4 RONO2 NO−3
NH4NO3 		HOONO2 FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 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 Se BrNO3 Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 NbO(NO3)3 MoO2(NO3)2 Tc Ru(NO3)3 Rh(NO3)3 Pd(NO3)2
Pd(NO3)4 		AgNO3
Ag(NO3)2 		Cd(NO3)2 In(NO3)3 Sn(NO3)4 Sb(NO3)3 Te INO3 Xe(NO3)2
CsNO3 Ba(NO3)2   Lu(NO3)3 Hf(NO3)4 TaO(NO3)3 W Re Os Ir Pt(NO3)2
Pt(NO3)4 		Au(NO3)3 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 PaO2(NO3)3 UO2(NO3)2 Np(NO3)4 Pu(NO3)4 Am(NO3)3 Cm(NO3)3 Bk(NO3)3 Cf Es Fm Md No

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