Chrome alum or Chromium(III) potassium sulfate is the potassium double sulfate of chromium. Its chemical formula is KCr(SO4)2 and it is commonly found in its dodecahydrate form as KCr(SO4)2·12(H2O). It is used in leather tanning.[1]
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| IUPAC name
Chromium potassium sulfate[citation needed]
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| Other names
Chromium alum[citation needed]
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.352 |
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| MeSH | chrome+alum |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| KCr(SO4)2 | |
| Molar mass | 283.220 g/mol |
| Appearance | dark purple needles or greyish-brown powder when anhydrous |
| Density | 1.83 g cm−3 |
| Melting point | 89 °C (192 °F; 362 K) |
| Boiling point | 400 °C (752 °F; 673 K) |
| 24 g/100mL (at 20 °C) | |
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| GHS labelling: | |
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| H315, H319 | |
| P305+P351+P338 | |
| Structure | |
| cubic | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Production and properties
edit_Potassium_Sulfate-crystals.jpg)
Chromium alum is produced from chromate salts or from ferrochromium alloys. Concentrated aqueous solutions of potassium dichromate can be reduced, usually with sulfur dioxide but also with alcohols or formaldehyde, in the presence of sulfuric acid at temperatures <40 °C. Alternatively and less commonly, ferrochromium alloys can be dissolved in sulfuric acid and, after precipitation of the ferrous sulfate, the chrome alum crystallizes upon addition of potassium sulfate. Chromium alum crystallizes in regular octahedra with flattened corners and is very soluble in water. The solution reddens litmus and is an astringent. Aqueous solutions are dark violet and turns green when it is heated above 50 °C.[1] In addition to the dodecahydrate, the hexahydrate KCr(SO4)2·6H2O, dihydrate KCr(SO4)2·2H2O, and the monohydrate KCr(SO4)2·H2O are known.[2]
Uses
editChromium alum is used in the tanning of leather[1] as chromium(III) stabilizes the leather by cross linking the collagen fibers within the leather.[3] However, this application is obsolete because the simpler chromium(III) sulfate is preferred.[2]
It was also used in gelatine emulsions in photographic film as hardener.[4]
References
edit- ^ a b c Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Chromium". Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.). Walter de Gruyter. pp. 1082–1095. ISBN 3-11-007511-3.
- ^ a b Gerd Anger, Jost Halstenberg, Klaus Hochgeschwender, Christoph Scherhag, Ulrich Korallus, Herbert Knopf, Peter Schmidt, Manfred Ohlinger, "Chromium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a07_067
- ^ Brown, E. M.; Dudley, R.L.; Elsetinow A. R. (1997). "A Conformational Study of Collagen as Affected by Tanning Procedures". Journal of the American Leather Chemists Association. 92: 225–233.
- ^ British Journal of Photography, vol 23 https://archive.org/details/britishjournalof35unse/page/478/mode/2up