Cobalt sulfate Property

Melting point:

decomposes at 1140℃ [JAN85]

Density 

d425 3.71

vapor pressure 

0Pa at 20℃

solubility 

H₂O: soluble

form 

red orthorhombic crystals

color 

red orthorhombic crystals, crystalline

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]

Merck 

13,2473

InChI

InChI=1S/Co.H2O4S.H2O/c;1-5(2,3)4;/h;(H2,1,2,3,4);1H2/q+2;;/p-2

InChIKey

BGORGFZEVHFAQU-UHFFFAOYSA-L

SMILES

S([O-])([O-])(=O)=O.O.[Co+2]

LogP

-1.031 (est)

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)

Safety

Hazard Codes 

T,N

Risk Statements 

49-42/43-51/53-50/53-22-68-60

Safety Statements 

53-23-36/37-45-61-60-22

RIDADR 

UN 3082 9/PG 3

WGK Germany 

2

Hazardous Substances Data

10124-43-3(Hazardous Substances Data)

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Danger

Hazard statements

H290May be corrosive to metals

H317May cause an allergic skin reaction

H319Causes serious eye irritation

H334May cause allergy or asthma symptoms or breathing difficulties if inhaled

H341Suspected of causing genetic defects

H410Very toxic to aquatic life with long lasting effects

Precautionary statements

P201Obtain special instructions before use.

P261Avoid breathing dust/fume/gas/mist/vapours/spray.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P284Wear respiratory protection.

P304+P340IF INHALED: Remove victim to fresh air and Keep at rest in a position comfortable for breathing.

P308+P313IF exposed or concerned: Get medical advice/attention.

Cobalt sulfate Chemical Properties,Usage,Production

Physical Properties

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.

Uses

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.

Preparation

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.

Description

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.

Chemical Properties

Red powder or rose pink crystalline solid. Odorless.

Uses

Ceramics, pigments, glazes, in plating baths for cobalt, additive to soils, catalyst, paint and ink drier, storage batteries.

Uses

Cobalt(II) Sulphate is used in batteries and fuel cells that display long-term stability.

Definition

ChEBI: Cobalt(2+) sulfate is a compound of cobalt and sulfate in which the ratio of cobalt (+2 oxidation state) to sulfate is 1:1. It contains a cobalt(2+).

General Description

Odorless rose-pink solid. Sinks and mixes with water.

Air & Water Reactions

Water soluble.

Reactivity Profile

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.

Hazard

May not be used in food products (FDA). Possible carcinogen.

Health Hazard

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

Fire Hazard

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

Flammability and Explosibility

Not classified

Safety Profile

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.

Potential Exposure

Many be used to catalyze organic reactions.

Carcinogenicity

Cobalt sulfate is reasonably anticipated to be a human carcinogenbased on sufficient evidence of carcinogenicity from studies in experimental animals.

Shipping

UN3288 Toxic solids, inorganic, n.o.s., Hazard Class: 6.1; Labels: 6.1-Poisonous materials, Technical Name Required.

Purification Methods

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).

Incompatibilities

Aqueous solution reacts with bases, generating some heat. May react as either oxidizing agents or reducing agents

Waste Disposal

Use a licensed professional waste disposal service to dispose of this material. All federal, state, and local environmental regulations must be observed.