71-48-7

Basic information

• Product Name: Cobalt acetate
• Synonyms: COBALT(II) ACETATE;COBALT ACETATE;acetatecobalteux;Aceticacid,cobalt(2+)salt;aceticacid,cobalt(2++)salt;bis(acetato)cobalt;cobalt(2+)acetate;cobaltacetate(co(oac)2)
• CAS NO: 71-48-7
• Molecular Formula: C₄H₆CoO₄
• Molecular Weight: 177.02
• EINECS: 200-755-8
• Product Categories: Organic-metal salt;Cobalt;Micro/Nanoelectronics;Solution Deposition Precursors;INORGANIC CHEMICAL ,cobalt, acetate
• Mol File: 71-48-7.mol

Chemical Properties

• Melting Point: 298 °C (dec.)(lit.)
• Boiling Point: 117.1 °C at 760 mmHg
• Flash Point: 40 °C
• Appearance: Pale pink to purple/Powder
• Density: 1.7043g/cm3
• Water Solubility: Soluble in waterSoluble in water, alcohol, dilute acids and pentyl acetate(tetrahydrate).
• Sensitive: Hygroscopic
• Merck: 14,2433
• CAS DataBase Reference: Cobalt acetate(CAS DataBase Reference)
• NIST Chemistry Reference: Cobalt acetate(71-48-7)
• EPA Substance Registry System: Cobalt acetate(71-48-7)

Safety Data

• Hazard Codes: Xn,N,T
• Statements: 22-36/37/38-40-43-53-68-50/53-42/43-60-49
• Safety Statements: 22-26-36/37/39-45-61-60-53
• RIDADR: UN 3077 9 / PGIII
• WGK Germany: 2
• RTECS: AG3150000
• TSCA: Yes
• HazardClass: 9
• Hazardous Substances Data: 71-48-7(Hazardous Substances Data)

Usage

Uses

Different sources of media describe the Uses of 71-48-7 differently. You can refer to the following data:
1. Cobalt(II) acetate is used for bleaching and drying varnishes and laquers. Other applications are: as a foam stabilizer for beverages; in sympathetic inks; as a mineral supplement in animal feed; and as a catalyst for oxidation. It also is used in aluminum anodizing solutions.
2. Cobalt(II) acetate is used as an industrial catalyst. It is used as a precursor to various oil drying agents. It finds application in ion exchange agents, lubricants, plating agents and surface treating agents, greases, ink, toner, and colorant products.
3. Sympathetic inks, paint and varnish driers, catalyst, anodizing, mineral supplement in feed additives, foam stabilizer.

Preparation

Cobalt(II) acetate is prepared by dissolving cobalt(II) carbonate or hydroxide in dilute acetic acid, followed by crystallization. Also, it may be prepared by oxidation of dicobalt octacarbonyl in the presence of acetic acid.

Chemical Properties

Violet Crystalline Powder or Pale pink to purple Powder. Catalyzer for oxidizing dimethylbenzene, desiccant for coating, mordant for printing, accelerant for solidifying glass. Cobalt(II) acetate is one of the compounds recommended for colouring the oxide layer formed on aluminium and its alloys by anodizing.

Physical properties

Red-to-violet monoclinic crystals (anhydrous acetate is light pink in color); density 1.705 g/cm3; becomes anhydrous when heated at 140°C; soluble in water, alcohols and acids.

Definition

ChEBI: A cobalt salt in which the cobalt metal is in the +2 oxidation state and the counter-anion is acetate.

General Description

Red-violet crystalline solid. Vinegar-like odor.

Air & Water Reactions

Water soluble. Deliquescent

Reactivity Profile

Salts, basic, such as Cobalt acetate, are generally soluble in water. The resulting solutions contain moderate concentrations of hydroxide ions and have pH's greater than 7.0. They react as bases to neutralize acids. These neutralizations generate heat, but less or far less than is generated by neutralization of the bases in reactivity group 10 (Bases) and the neutralization of amines. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible.

Hazard

May not be used in food products (FDA).

Health Hazard

Inhalation causes shortness of breath and coughing; permanent disability may occur. Ingestion causes pain and vomiting. Contact with eyes causes irritation. Contact with skin may cause dermatitis.

Fire Hazard

Special Hazards of Combustion Products: Toxic cobalt oxide fumes may form in fire.

Safety Profile

Poison by intravenous route. Moderately toxic by ingestion. Questionable carcinogen. Mutation data reported. See also COBALT COMPOUNDS. When heated to decomposition it emits acrid smoke and irritating fumes.

InChI:InChI=1/C2H4O2.Co/c1-2(3)4;/h1H3,(H,3,4);/q;+2/p-1

Upstream product

• 108-24-7 acetic anhydride 
• 64-19-7 acetic acid 
• 110-83-8 cyclohexene 
• 759403-02-6 cobalt(II) carbonate 
• 127-09-3 sodium acetate 
• 6147-53-1 cobalt(II) diacetate tetrahydrate 
• 7440-48-4 cobalt 
• 451-40-1 phenyl benzyl ketone 
• 998-40-3 tributylphosphine 
• 481711-41-5 Co(3,3',5,5'-tetramethyl-4,4'-dibutyldipyrrolylmethene-2,2'(-1H))2 
• 127-08-2 potassium acetate 
• 71-48-7 cobalt(II) acetate 

Downstream Products

• 629-15-2 ethylene glycol diformate 
• 14167-18-1 cobalt(II)(bis(salicylidene)ethylenediamine) 
• 802294-64-0 propionic acid 
• 107-92-6 butyric acid 
• 65-85-0 benzoic acid 
• 108-24-7 acetic anhydride 
• 71-48-7 cobalt(III) acetate 
• 100-52-7 benzaldehyde 
• 108-55-4 glutaric anhydride, 
• 62-23-7 4-nitro-benzoic acid 
• 26216-91-1 2-phenyl-2,3-dihydro-1H-indole 
• 25714-71-0 4-hydroxybutyraldehyde 

Relevant articles and documents

Co(II)-salen catalyzed stereoselective cyclopropanation of fluorinated styrenes

Three cis-selective Co(II)-salen complexes have been developed for the asymmetric cyclopropanation of para-fluorinated styrenes with ethyl diazoacetate. Increasing the steric reach of the C2-symmetric ligand side chains improved the enantiomeric ratio of the reaction from 28:1 to 66:1. The methodology was exemplified by the gram-scale synthesis of a lead compound for the treatment of castration-resistant prostate cancer (CRPC), as well as a structurally related analog.

The Role of Iodanyl Radicals as Critical Chain Carriers in Aerobic Hypervalent Iodine Chemistry

Selective O2 utilization remains a substantial challenge in synthetic chemistry. Biological small-molecule oxidation reactions often utilize aerobically generated high-valent catalyst intermediates to effect substrate oxidation. Available synthetic methods for aerobic oxidation catalysis are largely limited to substrate functionalization chemistry by low-valent catalyst intermediates (i.e., aerobically generated Pd(II) intermediates). Motivated by the need for new chemical platforms for aerobic oxidation catalysis, we recently developed aerobic hypervalent iodine chemistry. Here, we report that in contrast to the canonical two-electron oxidation mechanisms for the oxidation of organoiodides, the developed aerobic hypervalent iodine chemistry proceeds via a radical chain mechanism initiated by the addition of aerobically generated acetoxy radicals to aryl iodides. Despite the radical chain mechanism, aerobic hypervalent iodine chemistry displays substrate tolerance similar to that observed with traditional terminal oxidants, such as peracids. We anticipate that these insights will enable new sustainable oxidation chemistry via hypervalent iodine intermediates. O2 is routinely utilized in biological catalysis to generate high-valent catalyst intermediates that engage in substrate oxidation chemistry. Analogous synthetic chemistry via aerobically generated high-valent intermediates would enable new sustainable synthetic methods but is largely unknown because of the challenges in selective O2 utilization. We have developed aerobic hypervalent iodine chemistry as a platform for coupling O2 reduction with a diverse set of substrate functionalization mechanisms. Many of the synthetic applications of hypervalent iodine reagents rely on selective two-electron oxidation-reduction chemistry. Here, we report that one-electron oxidation reactions pathways via iodanyl radical intermediates are critical in aerobic hypervalent iodine chemistry. The new appreciation for the critical role that iodanyl radicals can play in the synthesis of hypervalent iodine compounds will provide new opportunities in sustainable oxidation catalysis. Aerobic hypervalent iodine chemistry provides a strategy for coupling the one-electron chemistry of O2 with two-electron processes typical of organic synthesis. We show that in contrast to the canonical two-electron oxidation of aryl iodides, aerobic synthesis proceeds by a radical chain process initiated by the addition of aerobically generated acetoxy radicals to aryliodides to generate iodanyl radicals. Robustness analysis reveals that the developed aerobic oxidation chemistry displays substrate tolerance similar to that observed in peracid-based methods and thus holds promise as a sustainable synthetic method.

The Kinetics of Growth of Metallo-supramolecular Polyelectrolytes in Solution

Several transition metal ions, like Fe2+, Co2+, Ni2+, and Zn2+ complex to the ditopic ligand 1,4-bis(2,2′:6′,2′′-terpyridin-4′-yl)benzene (L). Due to the high association constant, metal-ion induced self-assembly of Fe2+, Co2+, and Ni2+ leads to extended, rigid-rod like metallo-supramolecular coordination polyelectrolytes (MEPEs) even in aqueous solution. Here, we present the kinetics of growth of MEPEs. The species in solutions are analyzed by light scattering, viscometry and cryogenic transmission electron microscopy (cryo-TEM). At near-stoichiometric amounts of the reactants, we obtained high molar masses, which follow the order Ni-MEPE≈Co-MEPEa reversible step-growth mechanism. The forward polymerization rate constants follow the order Co-MEPEFe-MEPENi-MEPE and the growth of MEPEs can be accelerated by adding potassium acetate.

Kinetic stability of complexes of some d-metals with 3,3'- bis(dipyrrolylmethene) in the binary proton-donor solvent acetic acid-benzene

The kinetics of dissociation of Co(II), Ni(II), Cu(II), Zn(II), Cd(II), and Hg(II) binuclear homoleptic double-stranded helicates with bis(2,4,7,8,9- pentametyldipyrrolylmethen-3-yl)methane (H2L) of the [M 2L2] composition

Structural, spectral and magnetic properties of carboxylato cobalt(II) complexes with heterocyclic N-donor ligands: Reconstruction of magnetic parameters from electronic spectra

Heteroleptic cobalt(II) complexes with general formula of [Co(N-base) 2(car)2(H2O)2], have been synthesized and structurally characterized; the N-base stands for neutral N-donor ligands: iso-quinoline (iqu), [1]

Kinetics and products of the catalytic oxidation of acetamidotoluenes with ozone in acetic acid

The kinetics of acetamidotoluene oxidation in glacial acetic acid in the presence of cobalt acetate is reported. At 95°C and atmospheric pressure, acetamidotoluenes are oxidized by molecular oxygen very slowly: oxidation is complete in 10-12 h, and the major reaction products are acetamidobenzoic acids (27-36% yield). The introduction of ozone into the reactive gas increases the reaction rate by one order of magnitude. The main role of ozone is to generate the active form of the catalyst.

Factors affecting the selectivity of the oxidation of methyl p-toluate by cobalt(III)

The anaerobic oxidation of methyl p-toluate by cobalt(III) in acetic acid was investigated. Observed products were 4-carbomethoxybenzaldehyde (2), 4-carbomethoxybenzoic acid (3), 4-carbomethoxybenzyl acetate (1), 4,4′-dicarbomethoxybibenzyl (6), methyl 2,4-dimethylbenzoate (8), and methyl 3,4-dimethylbenzoate (9). Deuterium isotope labeling showed that 2 was not formed from 1, but appeared to be formed directly from methyl p-toluate via 4-carbomethoxybenzyl alcohol (5). The ratio of (2 + 3) to 1 was 0.5 with [Py3Co3O(OAc)5OH[PF6] and 1.0 with cobaltic acetate. Cobaltic acetate was generated in situ by the reaction of cobaltous acetate and peracetic acid. When the oxidation was carried out in the presence of chromium (0.05 equiv based on cobalt), the ratio increased dramatically and no 6 was observed. Other transition metals such as vanadium, molybdenum, and manganese had a similar effect, but were not as effective as chromium. Chromium was observed to form a mixed-metal cluster complex with cobalt. Treatment of an acetic acid solution of cobaltous acetate and methyl isonicotinate with K2CrO4 produced a solid tentatively identified as [(MIN)3Co2CrO(OAc)6][CrO 4H] (MIN = methyl isonicotinate). The selectivity for the oxidation of methyl p-toluate exhibited by the mixed-metal cluster complex was similar to that observed by the addition of chromium to oxidations using [py 3Co3O(OAc)5OH[PF6].

Synthesis and characterization of ternary carboxylato complexes of cobalt(II) with Schiff bases

Some novel mixed-ligand, ternary carboxylato complexes of cobalt(II) with Schiff bases (HSB) having general formula [Co(OOCR)(SB)] (where R = C 11H23, C13H27, C15H 31 or C17H35) have been synthesized by the substitution reactions of anhydrous cobalt(II) acetate. The isolated products have been characterized by elemental analyses, molar conductance and magnetic moment measurements and spectral (infrared, electronic and FAB mass) data. Models and coordination hypotheses for the complexes have been proposed and a peculiar structural characterization has been discussed on the basis of physicochemical studies. A sharp structural change has been noticed.

Synthesis and characterization of cobalt (II) complexes of chromen-2-one-3-carboxy hydrazide and 2-(chromen-2′-onyl)-5-(aryl) 1,3,4-oxadiazole derivatives

Cobalt(II) complexes of chromen-2-one-3-carboxy hydrazide and 2-(chromen 2′-onyl)-5-(aryl)-1,3,4-oxadiazole derivatives have been synthesized and characterized by elemental analysis, magnetic susceptibility, molar conductance, spectral studies [IR, UV-vis, and 1H NMR]. All the Co(II) complexes exhibit the composition M(Ln)2X2; where M = Co(II), L1 is chromen-2-one-3-carboxy hydrazide, L2 is 2-(chromen-2′-onyl)-5-(2″- hydroxylphenyl)1,3,4-oxadiazole, L3 2-(chromen-2′-onyl)-5-(4″- nitrophenyl)1,3,4-oxadiazole and L4 is 2-(chromen-2′-onyl)-5-(4″- chlorophenyl)1,3,4-oxadiazole. X = Cl-, Br-, NO 3-, CH3COO- , ClO4 -, CNS-, SO4-. The N,O donor ligands act as a bidentate ligand in all the complexes. Distorted octahedral geometry for all the Co(II) complexes is proposed. X-ray structure determination has been made for the exact definition of the coordination sphere. The newly synthesized Co(II) complexes have been screened for their antimicrobial activity against some bacterial species like E. coli, S. aureus, Pseudomonas aeruginosa and few fungal strains, C. albicans and Cryptococcus neoformans.

Racemic and chiral expanded salen-type complexes derived from biphenol and binaphthol: Salbip and salbin

The reaction of 2-fluoronitrobenzene with 2,2′-biphenol or (R)-binaphthol, followed by reduction and subsequent reaction of the resulting diamine with two equivalents of a salicylaldehyde, affords expanded salen-type ligands having backbones based on biphenol or binaphthol: salbipH2, (R)-salbinH2 and (R)-salbin(t-Bu)4H2. Deprotonation of these ligands with sodium methoxide or potassium hydride, followed by metallation with M(OAc)2 (M = Mn, Co, Ni, or Cu), affords the corresponding metal complexes in good yield (61-85%). The species containing Mn, Co, and Ni all have distorted octahedral geometry, as determined by X-ray crystallography. The ethereal oxygen atoms occupy two coordination sites with metal-oxygen distances ranging from 2.19 to 2.36 ?. The imine nitrogen atoms are trans to each other in the solid state, an impossible geometry in traditional salen-type complexes. The species containing Cu are distorted square planar and show much longer metal-ethereal oxygen distances ranging from 2.79 to 3.22 ?. The manganese complexes are competent catalysts for the epoxidation of olefins.