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Cobalt(II) acetate
Cobalt(II) acetate
| Names | |
|---|---|
| IUPAC name
Cobalt(II) acetate
| |
| Identifiers | |
| 3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.000.687 |
| 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 (anhydrous) intense red crystals (tetrahydrate) |
| 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)
|
1.542 (tetrahydrate) |
| Hazards | |
| Safety data sheet | J.T. Baker MSDS |
| NFPA 704 | |
| Lethal dose or concentration (LD, LC): | |
| LD50 (median dose)
|
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 ?) | |
| Infobox references | |
Cobalt(II) acetate is the cobalt(II) salt of acetic acid. It is commonly found as the tetrahydrate Co(C2H3O2)2·4 H2O or Co(CH3COO)2·4 H2O also abbreviated Co(OAc)2·4 H2O. It is used as an industrial catalyst.
Synthesis and structure
It may be formed by the reaction between cobalt oxide or hydroxide and acetic acid:
- CoO + 2 HC2H3O2 + 3 H2O → Co(C2H3O2)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]
Reactions and uses
Cobalt acetate is a precursor to various oil drying agents, catalysts that allow paints and varnishes to harden.[2] Cobalt(II) acetate reacts with salenH2 to give salcomine, a transition metal dioxygen complex:[3]
- Co(OAc)2 + salenH2 → Co(salen) + 2 HOAc
Safety
Cobalt salts are poisonous.[4]
- ^ 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.
- ^ 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
- ^ Appleton, T. G. (1977). "Oxygen Uptake by a Cobalt(II) Complex". J. Chem. Ed. 54 (7): 443. doi:10.1021/ed054p443.
- ^ MallBaker MSDS[permanent dead link]
| Salts and the ester of the acetate ion
| |||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| AcOH | He | ||||||||||||||||||
| LiOAc | Be(OAc)2 BeAcOH |
B(OAc)3 | ROAc | NH4OAc | AcOAc | 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 | 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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