Anhydrous cobalt chloride.
| Other names
Muriate of cobalt
|Molar mass|| 129.839 g/mol (anhydrous)|
165.87 g/mol (dihydrate)
237.93 g/mol (hexahydrate)
|Appearance|| Blue crystals (anhydrous)|
Rose-red crystals (hexahydrate)
|Density|| 3.356 g/cm3 (anhydrous)|
2.477 g/cm3 (dihydrate)
1.924 g/cm3 (hexahydrate)
|Melting point|| anhydrous|
735 °C (1,355 °F; 1,008 K)
140 °C (284 °F; 413 K)
100 °C (212 °F; 373 K)
86 °C (187 °F; 359 K)
| 43.6 g/100 ml (0 °C)|
45 g/100 ml (7 °C)
52.9 g/100 ml (20 °C)
105 g/100 ml (96 °C)
|Solubility||Soluble in ethanol, glycerol, pyridine|
|Solubility in acetone||8.6 g/100 ml|
|Solubility in methanol||38.5 g/100 ml|
|Safety data sheet|| Sigma-Aldrich (anhydrous)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|766 mg/kg (rat)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Cobalt(II) chloride is a colorful compound with the formula CoCl2. Three hydrates of cobalt chloride exist, anhydrous, dihydrate, and hexahydrate. All three hydrates are hygroscopic, with the anhydrous a light blue color, and the di and heptahydrate violet. All three are useful reagents which are commonly used as starting points for reactions involving cobalt.
In the presence of ammonia or amines, cobalt(II) is readily oxidized by atmospheric oxygen to give a variety of cobalt(III) complexes, such as hexamminecobalt(III) chloride:
- 4 CoCl2•6H2O + 4 NH4Cl + 20 NH3 + O2 → 4 [Co(NH3)6]Cl3 + 26 H2O
Cobalt(II) chloride is a salt that is blue when anhydrous and pink-purple when hydrated. The compound melts at 735 °C (anhydrous), 100 °C (dihydrate), 86 °C (hexahydrate). It boils at 1049 °C. CoCl2 is soluble in water (52.9 g/100 mL at 20 °C) methanol (38.5 g/100 mL), and slightly soluble in acetone, diethyl ether. The density for the three forms is 3.356 g/cm3 (anhydrous), 2.477 g/cm3 (dihydrate), 1.924 g/cm3 (heptahydrate).
Cobalt chloride heptahydrate can be synthesized by reacting two moles of hydrochloric acid with one mole of cobalt carbonate. Add a small amount of acid and then stir the mixture before adding another small portion, as the CO2 created can cause the mixture to overflow. Usually, there will be a layer of unreacted cobalt carbonate/other contaminants that must be filtered out using either vacuum or gravity filtration in order to receive a pure product.
- CoCO3 + 2 HCl → CoCl2 + CO2+ H2O
By heating this solution to dryness a light blue powder will be formed which is anhydrous cobalt chloride.
If heptahydrate crystals are desired the solution may be dried in a desiccator.
Cobalt(II) chloride can be purchased from chemical suppliers, both as a solid and as a solution.
It can also be found in some types of colored silica gel, though the amount is small.
Cobalt(II) chloride, along with other cobalt(II) compounds is classified as "Substance of very high concern" in the EU and its sale is regulated.
- Cobalt chloride can be used for the synthesis of many complexes, such as Hexamminecobalt (III) chloride and Potassium cobaltinitrite.
- Invisible ink
- Electroplating cobalt metal
- Water indicator, especially in desiccants
- Make cobalt coordination complexes
Cobalt dichloride is a strong allergen, with a LD50 of 80 mg/kg (rats).
Eye and hand protection should be worn while handling this compound.
Cobalt(II) chloride should be stored in an airtight container or bag to counter its strong hygroscopic nature.
Cobalt dichloride should be converted to an insoluble form before disposal.