Cobalt sulfate Chemical Properties
- Melting point:
- decomposes at 1140℃ [JAN85]
- d425 3.71
- H2O: soluble
- red orthorhombic crystals
- Water Solubility
- dissolves slowly in boiling H2O [MER06]; g/100g solution H2O: 19.7 ± 0.1 (0°C), 27.2 ± 0.1 (25°C), 27.8 (100°C); solid phase, CoSO4 · 7H2O (0°C, 25°C), CoSO4 ·H2O (100°C) [KRU93]
- CAS DataBase Reference
- 10124-43-3(CAS DataBase Reference)
- NIST Chemistry Reference
- Cobalt sulfate(10124-43-3)
- EPA Substance Registry System
- Cobalt(II) sulfate (10124-43-3)
- Language:EnglishProvider:Cobalt sulfate
Cobalt sulfate Usage And Synthesis
The anhydrous salt of cobalt(II) sulfate is a red orthogonal crystal; density 3.71g/cm3; melts above 700°C; the monohydrate is red orthogonal crystal having a density of 3.08 g/cm3; the heptahydrate is a pink salt, monoclinic prismatic crystals, density 2.03 g/cm3; heptahydrate dehydrates to hexahydrate at 41°C and converts to monohydrate at 74°C; the anhydrous salt and heptahydrates are soluble in water; monohydrate slowly dissolves in boiling water.
Cobalt(II) sulfate is used in storage batteries and electroplating baths for cobalt. It also is used as a dryer for lithographic inks; in pigments for decorating porcelains; in ceramics, glazes and enamels to protect from discoloring; and as a additive to soils.
Cobalt(II) sulfate is prepared by dissolving cobalt(II) oxide, hydroxide or carbonate in dilute sulfuric acid, followed by crystallization:
CoO + H2SO4 → CoSO4 + H2O
Co(OH)2 + H2SO4 → CoSO4 + 2H2O
CoCO3 + H2SO4 → CoSO4 + CO2 + H2O
Crystallization yields the commercial product, pink heptahydrate. Further oxidation of this salt in dilute H2SO4 with ozone or fluorine produces hydrated cobalt(III) sulfate, Co2(SO4)3•18H2O. This blue octadecahydrate, Co2(SO4)3•18H2O also is obtained by electrolytic oxidation of cobalt(II) chloride or any cobalt(II) salt solution in 8M sulfuric acid.
The blue, crystalline hydrate Co2(SO4)3.18H2O is prepared by the oxidation of cobalt(II) sulphate in 8N sulphuric acid either electrolytically or chemically with ozone or fluorine. It is stable in the dry state, but is decomposed by water with evolution of oxygen; it is fairly stable in solution in dilute sulphuric acid. Cobalt(III) alums MCo(SO4)2.12H2O (M = K, Rb, Cs or NH4) can be isolated as blue crystals from the mixed cooler solutions of the two sulphates in dilute sulphuric acid. The potassium alum is diamagnetic, the rubidium salt has a magnetic moment less than 1 B.M. and the ammonium alum has a moment of 2.1 B.M. at 304°K. The hydrated sulphate also has a small positive magnetic susceptibility. The sulphate is believed like the alums to contain the [Co(H2O)6]3+ ion.
Red powder or rose pink crystalline solid. Odorless.
Ceramics, pigments, glazes, in plating baths for cobalt, additive to soils, catalyst, paint and ink drier, storage batteries.
Odorless rose-pink solid. Sinks and mixes with water.
Air & Water Reactions
Acidic salts, such as Cobalt sulfate , are generally soluble in water. The resulting solutions contain moderate concentrations of hydrogen ions and have pH's of less than 7.0. They react as acids to neutralize bases. These neutralizations generate heat, but less or far less than is generated by neutralization of inorganic acids, inorganic oxoacids, and carboxylic acid. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible. Many of these compounds catalyze organic reactions.
May not be used in food products (FDA). Possible carcinogen.
Inhalation causes shortness of breath and coughing; permanent disability may occur. Ingestion causes pain and vomiting. Contact with eyes or skin causes irritation.
Special Hazards of Combustion Products: Toxic cobalt oxide fumes may form in fire.
Poison by intravenous and intraperitoneal routes. Moderately toxic by ingestion. Questionable carcinogen. When heated to decomposition it emits toxic fumes of SOx See also COBALT COMPOUNDS.
Many be used to catalyze organic reactions.
Cobalt sulfate is reasonably anticipated to be a human carcinogenbased on sufficient evidence of carcinogenicity from studies in experimental animals.
UN3288 Toxic solids, inorganic, n.o.s., Hazard Class: 6.1; Labels: 6.1-Poisonous materials, Technical Name Required.
Crystallise it three times from conductivity water (1.3mL/g) between 100o and 0o depending on which hydrate is required. The heptahydrate crystallises below 44o and is efflorescent with m 97o . Between 44o and 70o the monoclinic hexahydrate CoSO4.6H2O m 41.5o is formed, and above 70o the monohydrate CoSO4.H2O m 71o is obtained. The pale reddish or lavender-coloured anhydrous salt is obtained by heating the hydrate above 250o, boiling with conc H2SO4 or heating with (NH4)2SO4).
Aqueous solution reacts with bases, generating some heat. May react as either oxidizing agents or reducing agents
Use a licensed professional waste disposal service to dispose of this material. All federal, state, and local environmental regulations must be observed.
- Cobalt nitrate
- Manganese sulfate
- DAB Enhancer Solution Type ICobalt Sulfate (blue-black)
- COBALT SULFATE UN3077-III
- Ammonium cobalt(II) sulfate hexahydrate
- COBALT POTASSIUM SULFATE
- AMMONIUM COBALT SULFATE
- Cobalt sulfate
- Sodium sulfate
- Cobalt(Ⅱ) sulfate hydrate,COBALT SULFATE HYDRATE,COBALT SULFATE MONOHYDRATE,Cobalt(Ⅱ) sulfate anhydrous
- Cobalt sulfate heptahydrate: (Cobalt(II) sulfate(1:1), heptahydrate),Cobalt Sulfate, crystal,Tennant Cobalt Sulfate,COBALT SULFATE REAGENT,COBALT SULFATE HEPTAHYDRATE,COBALT SULFATE, 7-HYDRATE,COBALT SULFATE, 99.999%,Cobalt(Ⅱ) sulfate heptahydrate
- Dimethyl sulfate
- Barium sulfate
- Kanamycin sulfate
- Magnesium sulfate heptahydrate
- n-Dodecyl alcohol, sulfated
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