Chemistry:Cobalt(II) acetate
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| Names | |
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| IUPAC name
Cobalt(II) acetate
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| UNII |
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| Properties | |
| Co(C2H3O2)2 | |
| Molar mass | 177.02124 g/mol (anhydrous) 249.08 g/mol (tetrahydrate) |
| Appearance | Pink crystals (tetrahydrate) intense red crystals (anhydrous) |
| Odor | vinegar (tetrahydrate) |
| Density | 1.705 g/cm3 (tetrahydrate) |
| Melting point | 140 °C (284 °F; 413 K) (tetrahydrate) |
| Soluble | |
| Solubility | soluble in alcohol, dilute acids, pentyl acetate (tetrahydrate) |
| +11,000·10−6 cm3/mol | |
Refractive index (nD)
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1.542 (tetrahydrate) |
| Hazards | |
| Safety data sheet | J.T. Baker MSDS |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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503 mg/kg (oral, rat) |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Cobalt(II) acetate is the cobalt salt of acetic acid. It is commonly found as the tetrahydrate Co(CH3CO2)2·4 H2O, abbreviated Co(OAc)2·4 H2O. It is used as a catalyst.
Synthesis and structure
Like many other transition metal acetates, cobalt(II) acetate forms by the reaction of cobalt oxide or hydroxide and acetic acid:
- CoO + 2 CH3CO2H + 3 H2O → Co(CH3CO2)2·4 H2O
The tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central cobalt centre being coordinated by four water molecules and two acetate ligands.[1] The analogous nickel acetate is isostructural.[2]
Various hydrates are known including Co(CH3CO2)2·H2O and [Co(CH3CO2)2]5·0.5 H2O.[3]
Reactions and uses
Cobalt acetate is a precursor to various oil drying agents, catalysts that allow paints and varnishes to harden.[4]
Anhydrous cobalt acetate is a widely used source of cobalt in the synthesis of materials,[5] catalyst,[6] and complexes.[7]
Safety
Cobalt salts are poisonous.[8]
References
- ↑ Sobolev, Alexandre N.; Miminoshvili, Elguja B.; Miminoshvili, Ketevan E.; Sakvarelidze, Tamara N. (2003). "Cobalt diacetate tetrahydrate". Acta Crystallographica Section E 59 (10): m836–m837. doi:10.1107/S1600536803019093.
- ↑ Van Niekerk, J. N.; Schoening, F. R. L. (1953). "The crystal structures of nickel acetate, Ni(CH3COO)2·4H2O, and cobalt acetate, Co(CH3COO)2·4H2O". Acta Crystallogr. 6 (7): 609–612. doi:10.1107/S0365110X5300171X.
- ↑ Zhang, Gao; Lin, Jian; Guo, Dong-Wei; Yao, Shi-Yan; Tian, Yun-Qi (2010). "Infinite Coordination Polymers of One- and Two-dimensional Cobalt Acetates". Zeitschrift für Anorganische und Allgemeine Chemie 636 (7): 1401–1404. doi:10.1002/zaac.200900457.
- ↑ 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
- ↑ Rodenas, Tania; Luz, Ignacio; Prieto, Gonzalo; Seoane, Beatriz; Miro, Hozanna; Corma, Avelino; Kapteijn, Freek; Llabrés i Xamena, Francesc X. et al. (2015). "Metal–organic framework nanosheets in polymer composite materials for gas separation". Nature Materials 14 (1): 48–55. doi:10.1038/nmat4113. PMID 25362353. Bibcode: 2015NatMa..14...48R.
- ↑ Schultz, Mitchell J.; Sigman, Matthew S. (2006). "Recent advances in homogeneous transition metal-catalyzed aerobic alcohol oxidations". Tetrahedron 62 (35): 8227–8241. doi:10.1016/j.tet.2006.06.065.
- ↑ Appleton, T. G. (1977). "Oxygen Uptake by a Cobalt(II) Complex". J. Chem. Educ. 54 (7): 443. doi:10.1021/ed054p443.
- ↑ MallBaker MSDS[yes|permanent dead link|dead link}}]
Acetyl halides and salts of the acetate ion
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| AcOH | He | ||||||||||||||||||
| LiOAc | Be(OAc)2 BeAcOH |
B(OAc)3 | AcOAc ROAc |
NH4OAc | AcOOH | FAc | Ne | ||||||||||||
| NaOAc | Mg(OAc)2 | Al(OAc)3 ALSOL Al(OAc)2OH Al2SO4(OAc)4 |
Si | P | S | ClAc | Ar | ||||||||||||
| KOAc | Ca(OAc)2 | Sc(OAc)3 | Ti(OAc)4 | VO(OAc)3 | Cr(OAc)2 Cr(OAc)3 |
Mn(OAc)2 Mn(OAc)3 |
Fe(OAc)2 Fe(OAc)3 |
Co(OAc)2, Co(OAc)3 |
Ni(OAc)2 | Cu(OAc)2 | Zn(OAc)2 | Ga(OAc)3 | Ge | As(OAc)3 | Se | BrAc | Kr | ||
| RbOAc | Sr(OAc)2 | Y(OAc)3 | Zr(OAc)4 | Nb | Mo(OAc)2 | Tc | Ru(OAc)2 Ru(OAc)3 Ru(OAc)4 |
Rh2(OAc)4 | Pd(OAc)2 | AgOAc | Cd(OAc)2 | In | Sn(OAc)2 Sn(OAc)4 |
Sb(OAc)3 | Te | IAc | Xe | ||
| CsOAc | Ba(OAc)2 | Hf | Ta | W | Re | Os | Ir | Pt(OAc)2 | Au | Hg2(OAc)2, Hg(OAc)2 |
TlOAc Tl(OAc)3 |
Pb(OAc)2 Pb(OAc)4 |
Bi(OAc)3 | Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La(OAc)3 | Ce(OAc)x | Pr | Nd | Pm | Sm(OAc)3 | Eu(OAc)3 | Gd(OAc)3 | Tb | Dy(OAc)3 | Ho(OAc)3 | Er | Tm | Yb(OAc)3 | Lu(OAc)3 | |||||
| Ac | Th | Pa | UO2(OAc)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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