Cobalt(II) acetate

Names
IUPAC name

Cobalt(II) acetate

Identifiers

CAS Number

* 71-48-7 (anhydrous) Y
* 6147-53-1 (tetrahydrate) Y

3D model (JSmol)

* ionic form: Interactive image
* coordination form (anhydrate): Interactive image
* coordination form (tetrahydrate): Interactive image

ChemSpider |

* 6041 Y

PubChem CID

* 6277

UNII |

* 3XC4P44U7E Y
* 7648Z91O1N (tetrahydrate) Y

InChI

* InChI=1S/2C2H4O2.Co/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 Y

Key: QAHREYKOYSIQPH-UHFFFAOYSA-L Y

* InChI=1/2C2H4O2.Co/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2

Key: QAHREYKOYSIQPH-NUQVWONBAX

SMILES

* ionic form: [Co+2].[O-]C(=O)C.[O-]C(=O)C

* coordination form (anhydrate): O=C(C)O[Co]OC(C)=O

* coordination form (tetrahydrate): O=C(C)O[Co-4]([O+H2])([O+H2])([O+H2])([O+H2])OC(C)=O

Properties

Chemical formula

| 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)

Solubility in water

| Soluble
Solubility | soluble in alcohol, dilute acids, pentyl acetate (tetrahydrate)

Magnetic susceptibility (χ)

| +11,000·10−6 cm3/mol

Refractive index (nD)

| 1.542 (tetrahydrate)
Hazards
Safety data sheet | J.T. Baker MSDS
NFPA 704 (fire diamond)  |

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).

N verify (what is YN ?)
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.

## Contents

* 1 Synthesis and structure
* 2 Reactions and uses
* 3 Safety
* 4 References

## 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

1. ↑ 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.
2. ↑ 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.
3. ↑ 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.
4. ↑ 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
5. ↑ 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.
6. ↑ 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.
7. ↑ Appleton, T. G. (1977). "Oxygen Uptake by a Cobalt(II) Complex". J. Chem. Educ. 54 (7): 443. doi:10.1021/ed054p443.
8. ↑ MallBaker MSDS[yes|permanent dead link|dead link}}]

* v
* t
* e

Cobalt compounds

* CoBr2
* Co(CN)2
* CoCO3
* CoC2O4
* CoCl2
* CoCl3
* Co(ClO3)2
* CoF2
* CoF3
* CoI2
* Co(NO3)2
* Co(NO3)3
* CoO
* Co(OH)2
* CoS
* CoSO4
* CoSe
* Co2O3
* Co2P
* Co3O4
* Co3(PO4)2
* Co(Ac)2

* v
* t
* e

Acetyl halides and salts of the acetate ion

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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