Potassium alum
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| ChEBI | |
| ECHA InfoCard | 100.030.116 |
| E number | E522 (acidity regulators, ...) |
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| Properties | |
| KAl(SO4)2·12H2O | |
| Molar mass | 474.3884 g/mol |
| Appearance | white small crystals |
| Odor | watery metallic |
| Density | 1.725 g/cm3 |
| Melting point | 92 to 95 °C (198 to 203 °F; 365 to 368 K) |
| Boiling point | 200 °C (392 °F; 473 K) |
| 14.00 g/100 mL (20 °C) 36.80 g/100 mL (50 °C) | |
| Solubility | insoluble in acetone |
| Refractive index (nD) |
1.4564 |
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| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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Potassium alum, potash alum, or potassium aluminum sulfate is a chemical compound: the potassium double sulfate of aluminium. Its chemical formula is KAl(SO4)2 and it is commonly found in its dodecahydrate form as KAl(SO4)2·12H2O. Alum is the common name for this chemical compound, given the nomenclature of potassium aluminum sulfate dodecahydrate. It is commonly used in water purification, leather tanning, dyeing,[4] fireproof textiles, and baking powder. It also has cosmetic uses as a deodorant, as an aftershave treatment and as a styptic for minor bleeding from shaving.[5]
Characteristics
Potassium alum crystallizes in regular octahedra with flattened corners and is very soluble in water. The solution reddens litmus and is an astringent. When heated to nearly a red heat, it gives a porous, friable mass, which is known as "burnt alum". It fuses at 92 °C (198 °F) in its own water of crystallization. "Neutral alum" is obtained by the addition of as much sodium carbonate to a solution of alum as will begin to cause the separation of alumina.
Mineral form and occurrence
Potassium alum or alum-(K) is a naturally occurring sulfate mineral, which typically occurs as encrustations on rocks in areas of weathering and oxidation of sulfide minerals and potassium-bearing minerals. In the past, alum was obtained from alunite, a mineral mined from sulfur-containing volcanic sediments source.[6] Alunite is an associate and likely potassium and aluminium source.[3][7] It has been reported at Vesuvius, Italy; east of Springsure, Queensland; Alum Cave, Tennessee; Alum Gulch, Santa Cruz County, Arizona and the Philippine island of Cebu. A related mineral is kalinite, a fibrous mineral with formula KAl(SO4)2·11H2O.[8]
Uses
Chemical
- in tanning of leather to prepare the hide
- as a mordant for dyes
- in the clarifying of turbid liquids, including post-storm treatment of lakes to precipitate contaminants[9]
- as a fire retardant in textile products
- (historically) as a hardener for photographic emulsions (films and papers), usually as part of the fixer. Modern alternatives are superior.
Medicinal
- as an astringent/styptic and antiseptic.
- as a natural deodorant by inhibiting the growth of the bacteria responsible for body odor.[5]
- after shaving to prepare the skin
- to reduce bleeding in minor cuts and abrasions, nosebleeds, and hemorrhoids.
- to remove pimples and acne.
Culinary
- As an additive to baking powder to provide a second leavening phase at high temperatures.
- To preserve and add crispness to fruit and vegetable especially when pickling.
Traditional
- In Ayurveda, where it is called phitkari or saurashtri
- In traditional Chinese medicine it is called mingfan 明礬.
Toxicology and safety
Potassium alum may be a weak irritant to the skin.[10]
See also
References
- ↑ International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN 0-85404-438-8. Electronic version.
- ↑ "Aluminium potassium sulfate dodecahydrate". ChemExper. Retrieved 2013-04-19.
- 1 2 "Alum-(K) Mineral Data". Mineralogy Database. Retrieved 2013-04-19.
- ↑ Editors, The. "alum | chemical compound". Britannica.com. Retrieved 2016-01-18.
- 1 2 Helmenstine, Anne Marie. "What is Alum?". About.com. Retrieved 2013-04-19.
- ↑ Bottomley (2010) p. 35.
- ↑ "Alum-(K) mineral data and information". MinDat. Retrieved 2013-04-19.
- ↑ "Kalinite Mineral Data". MinDat. Retrieved 2013-04-19.
- ↑ "Storm water treatment will strip phosphorus from Arboretum pond, College of Engineering @ The University of Wisconsin-Madison, initiatives in energy, health, nanotechnology, security, and information technology". Engr.wisc.edu. Retrieved 2016-01-18.
- ↑ Gallego H, Lewis EJ, Crutchfield CE 3rd (July 1999). "Crystal deodorant dermatitis: irritant dermatitis to alum-containing deodorant". Cutis. 64 (1): 65–6. PMID 10431678.
Further reading
- Bottomley, L.; Bottomley, L.A. (2010). School of Chemistry & Biochemistry, Georgia Institute of Technology, Chemistry 1310: Laboratory Manual. Plymouth, MI: Hayden-McNeil Publishing. ISBN 978-0-7380-3819-3.