Chemical Property of Cobalt chloride (CoCl2)
Chemical Property:
- Appearance/Colour:Blue crystalline powder
- Vapor Pressure:40 mm Hg ( 0 °C)
- Melting Point:724 °C(lit.)
- Boiling Point:1049 °C
- Flash Point:500 °C
- PSA：0.00000
- Density:3.35 g/cm3
- LogP:1.37900
- Storage Temp.:2-8°C
- Sensitive.:Hygroscopic
- Solubility.:585.9g/l soluble
- Water Solubility.:soluble
- Hydrogen Bond Donor Count:0
- Hydrogen Bond Acceptor Count:0
- Rotatable Bond Count:0
- Exact Mass:128.870899
- Heavy Atom Count:3
- Complexity:2.8
- Purity/Quality:
-
99% *data from raw suppliers
Cobalt(II) chloride
*data from reagent suppliers
Safty Information:
- Pictogram(s):
T, 
N
- Hazard Codes:T,N
- Statements:
49-42/43-52/53-50/53-22-68-41-60-51/53
- Safety Statements:
53-23-36/37-45-60-61-22-39-26
- MSDS Files:
-
SDS file from LookChem
Total 1 MSDS from other Authors
Useful:
- Canonical SMILES:Cl[Co]Cl
- Inhalation Risk:A harmful concentration of airborne particles can be reached quickly when dispersed.
- Effects of Short Term Exposure:The substance is irritating to the eyes.
- Effects of Long Term Exposure:Repeated or prolonged contact may cause skin sensitization. Repeated or prolonged inhalation may cause asthma. Ingestion may cause effects on the heart, bone marrow and thyroid. This substance is possibly carcinogenic to humans. Animal tests show that this substance possibly causes toxic effects upon human reproduction.
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Uses
Cobalt(II) chloride has several applications. It is used in hygrometers; as a
humidity indicator; as a temperature indicator in grinding; as a foam stabilizer in beer; in invisible ink; for painting on glass; in electroplating; and a catalyst in Grignard reactions, promoting coupling with an organic halide. It also is used to prepare several other cobalt salts; and in the manufacture of synthetic vitamin B12.
The vapor-phase co-reductions with other metal halides by hydrogen results in finely divided intermetallics with applications as structural materials or compounds with useful thermoelectric, magnetic, and oxidation-resistance properties. Cobalt(II) chloride is used in humidity indicator in weather instruments. In the anhydrous form, it finds use in electroplating of cobalt, in organic chemistry and is a precursor to cobaltocene, (bis(cyclopentadienyl)cobalt(II), which is a good reducing agent. It also serves as a Lewis acid. Cobalt chloride is an indicator for water in desiccants, owing to the reversible hydration/dehydration coupled with distinct color change. Cobalt chloride is useful for producing invisible ink as it turns blue when heated and becomes invisible once it gets cooled. Cobalt(II) chloride catalyzes cross coupling of aryl halides or vinyl halides with aryl grignard reagents in excellent yields. Cobalt chloride (CoCl2) is used to manufacture vitamin B12, even though the compound
itself can cause damage to red blood cells. It is also used as a dye mordant (to fix the dye to
the textile so that it will not run). It is also of use in manufacturing solid lubricants, as an
additive to fertilizers, as a chemical reagent in laboratories, and as an absorbent in gas masks,
electroplating, and the manufacture of vitamin B12. Absorbent for ammonia, gas masks, electroplating, sympathetic inks, hygrometers, manufacture of vitamin B
12, flux for magnesium refining,
solid lubricant, dye mordant, catalyst, barometers,
laboratory reagent, fertilizer additive.
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Description
blue crystals (anhydrous)
violet-blue (dihydrate)
rose red crystals (hexahydrate)
Sinks and mixes with water. Pale blue leaflets, turns pink upon exposure to moist air.
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Physical properties
Blue leaflets; turns pink in moist air; hygroscopic; the dihydrate is violet blue crystal; the hexahydrate is pink monoclinic crystal; density 3.36, 2.48 and 1.92 g/cm3 for anhydrous salt, dihydrate and hexahydrate, respectively; anhydrous salt melts at 740°C and vaporizes at 1,049°C; vapor pressure 60 torr at 801°C; the hexahydrate decomposes at 87°C; the anhydrous salt and the hydrates are all soluble in water, ethanol, acetone, and ether; the solubility of hydrates in water is greater than the anhydrous salt.
