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Potassium alum

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Potassium aluminium sulfate
Aluminium potassium sulfate
Names
IUPAC name
Aluminium potassium sulfate dodecahydrate[2][3]
Other names
Potassium alum
Potash alum
Alum-(K)[1]
phitkari
Identifiers
3D model (JSmol)
ChEBI
ECHA InfoCard 100.112.464 Edit this at Wikidata
E number E522 (acidity regulators, ...)
  • InChI=1S/Al.K.2H2O4S/c;;2*1-5(2,3)4/h;;2*(H2,1,2,3,4)/q+3;+1;;/p-4
  • [O-]S(=O)(=O)[O-].[O-]S(=O)(=O)[O-].[Al+3].[K+]
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
1.4564
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

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

Octahedral potassium alum crystal with unequal distribution of the face area.

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.[1][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

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

Toxicology and safety

Potassium alum may be a weak irritant to the skin.[11]

See also

References

  1. ^ a b "Alum-(K) Mineral Data". Mineralogy Database. Retrieved 19 April 2013.
  2. ^ 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.
  3. ^ "Aluminium potassium sulfate dodecahydrate". ChemExper. Retrieved 19 April 2013.
  4. ^ Editors, The. "alum | chemical compound". Britannica.com. Retrieved 18 January 2016. {{cite web}}: |last= has generic name (help)
  5. ^ a b Helmenstine, Anne Marie. "What is Alum?". About.com. Retrieved 19 April 2013.
  6. ^ Bottomley (2010) p. 35
  7. ^ "Alum-(K) mineral data and information". MinDat. Retrieved 19 April 2013.
  8. ^ "Kalinite Mineral Data". MinDat. Retrieved 19 April 2013.
  9. ^ "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 18 January 2016.
  10. ^ Uses of Alum in Traditional Chinese Medicine
  11. ^ 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.{{cite journal}}: CS1 maint: multiple names: authors list (link) CS1 maint: numeric names: authors list (link)

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.{{cite book}}: CS1 maint: multiple names: authors list (link)
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