| IUPAC name
| Other names
|Molar mass|| 158.36 g/mol (anhydrous)|
266.45 g/mol (hexahydrate)
|Appearance|| Purple (anhydrous)|
Dark green (hexahydrate)
|Density|| 2.87 g/cm3 (anhydrous)|
1.76 g/cm3 (hexahydrate)
|Melting point|| 1,152 °C (2,106 °F; 1,425 K) (anhydrous)|
83 °C (181 °F; 356 K) (hexahydrate)
|Boiling point||1,300 °C (2,370 °F; 1,570 K) (decomposes)|
58.5 g/100 ml (20 °C)
|Solubility||Insoluble in acetone, diethyl ether, ethanol|
|Safety data sheet|| Sigma-Aldrich (anhydrous)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|1,870 mg/kg (rat, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Chromium(III) chloride (CrCl3) is a compound of chromium. It is available in two forms, anhydrous and hydrated.
Chromium(III) chloride will react with bases to give chromium hydroxide.
Chromium(III) chloride is a purple (anhydrous) or dark green (hydrated) solid.
Chromium chloride is sold by chemical suppliers.
Chromium chloride hexahydrate can be obtained by reacting chromium oxide, hydroxide or plain chromium metal with conc. hydrochloric acid.
A more energetic route involves the carbothermic chlorination of chromium(III) oxide between 650–800 °C.
Reacting chlorine gas with hot chromium metal will also give anhydrous CrCl3.
Heating chromium(III) chloride hexahydrate in air will cause some of it to oxidize, resulting in CrCl3 contaminated with oxide and oxychloride. To obtain the anhydrous form from the hexahydrate, you must heat the CrCl3 in the presence of a chlorine or chloride source, like thionyl chloride or dry hydrogen chloride gas.
- Make chromates and dichromates
- Make chromium(II) chloride
- Make Cr coordination complexes and adducts
- Make organochromium compounds
While less toxic than Cr(VI) compounds, chromium chloride is less toxic, although it's still quite harmful.
In closed bottles, air-tight for the anhydrous form.
Should be converted to less soluble forms and sent to disposal facilities. You can also recycle it.