| IUPAC name
| Other names
Basic chromium sulfate
|Molar mass|| 392.16 g/mol|
608.363 g/mol (dodecahydrate)
716.45 g/mol (octadecahydrate)
|Appearance|| Reddish-brown crystals (anhydrous)|
Purple crystals (hydrated)
|Density|| 3.10 g/cm3 (anhydrous)|
1.86 g/cm3 (pentadecahydrate)
1.709 g/cm3 (octadecahydrate)
|Melting point||90 °C (194 °F; 363 K) (hydrated)|
|Boiling point||700 °C (1,292 °F; 973 K) (decomposes)|
|Solubility|| Reacts with bases|
Soluble in alcohols
Insoluble in mineral acids, organic solvents
|Vapor pressure||~0 mmHg|
|Safety data sheet||Sigma-Aldrich (hydrate)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Chromium(III) sulfate is the inorganic compound with chemical formula Cr2(SO4)3. It is a temperature-sensitive blue-grey solid and one of the principal compounds of chromium.
Solutions of chromium(III) sulfate turn from blue to green upon heating, indicating the formation of a less reactive "sulfato-complex" that may take days or weeks to revert. Freshly prepared chromium sulfate often contains traces of this coloration, with some samples even appearing green rather than blue, but is otherwise usable.
Treatment of chromium(III) sulfate with bases produces chromium(III) hydroxide. If the base used is a carbonate or bicarbonate, this reaction is accompanied with the release of carbon dioxide, in a manner similar to iron, which does not form carbonates.
Chromium(III) sulfate most often appears as a blue-grey or violet-grey amorphous solid. Recently prepared samples or those that have been subjected to heat may contain a deep green-colored sulfato complex and are hygroscopic as a result. Purer samples can be dried to form a lighter-colored powder.
Chromium(III) sulfate is readily soluble in water and some lower alcohols.
Chromium sulfate, for the most part, can only be purchased from online suppliers. Its use as a tanning chemical has largely been superseded by chrome alum and other agents.
The Jones oxidation, which uses a solution of potassium dichromate or sodium dichromate acidified with sulfuric acid to oxidize alcohols, produces chromium(III) sulfate as a byproduct, along with sodium or potassium sulfate. If the temperature of the reaction is kept low enough, the presence of chromium(III) sulfate will be indicated by a blue or blue-violet color to the end product, rather than a green color produced when the temperature is too high. To extract the chromium(III) from solution, the reaction products must be treated with bases to precipitate chromium(III) hydroxide.
Chromium(III) sulfate can be more directly produced by the action of cold, dilute sulfuric acid on chromium(III) hydroxide or chromium(III) oxide. It should be noted, however, that many grades of chromium(III) oxide are not reactive enough, often as a result of being calcined, to respond to treatment with acid.
- Grow crystals of chrome alum, a double salt
- Compound collecting (colored salts)
- Make chromates and dichromates
Contact with solutions of chromium(III) sulfate or inhalation of particles may cause irritation, but overall this compound is relatively non-toxic.
Chromium(III) sulfate is relatively stable and has low reactivity, but should be kept away from temperatures greater than 40 °C when in the presence of moisture to avoid complex formation. A clean plastic bottle is a good storage bottle.
Chromium(III) can be harmful to marine life, so water-soluble compounds of trivalent chromium should be precipitated as chromium(III) hydroxide before being disposed of in the trash. You can also recycle the chromium ions.