Cobalt(II) nitrate
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| Names | |
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| Other names
Cobaltous nitrate
Nitric acid, cobalt(2+) salt |
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.030.353 |
| EC Number | 233-402-1 |
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PubChem CID
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| RTECS number | GG1109000 |
| UNII | |
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| Properties | |
| Co(NO3)2 | |
| Molar mass | 182.943 g/mol (anhydrous) 291.03 g/mol (hexahydrate) |
| Appearance | pale red powder (anhydrous) red crystalline (hexahydrate) |
| Odor | odorless (hexahydrate) |
| Density | 2.49 g/cm3 (anhydrous) 1.87 g/cm3 (hexahydrate) |
| 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) |
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| Solubility | soluble in alcohol, acetone, ethanol, ammonia (hexahydrate) |
| Structure | |
| monoclinic (hexahydrate) | |
| Hazards | |
| Safety data sheet | Cobalt (II) Nitrate MSDS |
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EU classification (DSD) (outdated)
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Carc. Cat. 2 Muta. Cat. 3 Repr. Cat. 2 Toxic (T) Dangerous for the environment (N) |
| R-phrases (outdated) | R49, R60, R42/43, R68, R50/53 |
| S-phrases (outdated) | S53, S45, S60, S61 |
| NFPA 704 | |
| Lethal dose or concentration (LD, LC): | |
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LD50 (median dose)
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434 mg/kg; rat, oral (anhydrous) 691 mg/kg; rat, oral (hexahydrate) |
| Related compounds | |
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Other anions
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Cobalt(II) sulfate Cobalt(II) chloride Cobalt oxalate |
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Other cations
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Iron(III) nitrate Nickel(II) nitrate |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Cobalt Nitrate is the inorganic cobalt(II) salt of nitric acid, often with various amounts of water. It is more commonly found as a hexahydrate, Co(NO3)2·6H2O, which is a red-brown deliquescent salt that is soluble in water and other polar solvents.[2]
Composition and structures[edit]
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. 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.[4] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate.[2]
Uses[edit]
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.[5] It is used in the preparation of dyes and inks.[6]
Production[edit]
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
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References[edit]
- ^ Perrys' Chem Eng Handbook, 7th Ed
- ^ 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
- ^ 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.
- ^ Prelesnik, P. V.; Gabela, F.; Ribar, B.; Krstanovic, I. (1973). "Hexaaquacobalt(II) nitrate". Cryst. Struct. Commun. 2 (4): 581–583.
- ^ Ernst B, Libs S, Chaumette P, Kiennemann A. Appl. Catal. A 186 (1-2): 145-168 1999
- ^ 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
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Salts and covalent derivatives of the Nitrate ion
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| HNO3 | He | ||||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO3)4− | C | N | O | 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)3, Fe(NO3)2 |
Co(NO3)2, Co(NO3)3 |
Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | Br | Kr | ||
| RbNO3 | Sr(NO3)2 | Y | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | Te | I | Xe(NO3)2 | ||
| CsNO3 | Ba(NO3)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(NO3)2, Hg(NO3)2 |
Tl(NO3)3, TlNO3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |||
| FrNO3 | Ra(NO3)2 | 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 | Nd | Pm | Sm | Eu | Gd(NO3)3 | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
| Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
