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Lumina Health

Aluminium Sulfate

Preparation

Aluminium sulfate may be made by aluminium hydroxide, Al(OH)3, in sulfuric acid, H2SO4:

2 Al(OH)3 + 3 H2SO4 Al2(SO4)36H2O

Uses

Aluminium Sulfate is used in water purification and as a mordant in dyeing and printing textiles. In water purification, it causes impurities to coagulate which are removed as the particulate settles to the bottom of the container or more easily filtered. This process is called coagulation or flocculation.

When dissolved in a large amount of neutral or slightly-alkaline water, aluminium sulfate produces a gelatinous precipitate of aluminium hydroxide, Al(OH)3. In dyeing and printing cloth, the gelatinous precipitate helps the dye adhere to the clothing fibers by rendering the pigment insoluble.

Aluminium sulfate is sometimes used to reduce the pH of garden soil, as it hydrolyzes to form the aluminium hydroxide precipitate and a dilute sulfuric acid solution. An example of what changing the pH level of soil can do to plants is visible when looking at the Hydrangea macrophylla. The gardener can add Aluminum sulfate to the soil to reduce the pH level which in turn will result in the flowers of the Hydrangea turning a different color.

Aluminium sulfate is the active ingredient of some antiperspirants; however, beginning in 2005 the US Food and Drug Administration no longer recognized it as a wetness reducer.

Aluminium sulfate is usually found in baking powder, where there is controversy over its use due to concern regarding the safety of adding aluminum to the diet.

In construction industry it is used as waterproofing agent and accelerator in concrete. Another use is a foaming agent in fire fighting foam.

It is also used in styptic pencils, and pain relief from stings and bites; it is the active ingredient in popular pain relief products such as Stingose.

It can also be very effective as a molluscicide, killing spanish slugs.

Ahmed Ressam, the al-Qaeda Millenium Bomber, used aluminum sulfate as one of the components in the explosives that he prepared to bomb Los Angeles International Airport on New Year's Eve 1999/2000; the explosives could have produced a blast 40x greater than that of a devastating car bomb.

Chemical Reactions

The compound decomposes to lumina and sulfite when heated between 580 and 900C. It combines with water forming hydrated salts of various compositions.

Produces calcium aluminate with the evolution of sulfate when calcined with calcium sulfate:[citation needed]

Al2(SO4)3 + CaSO4 Ca(AlO2)2 + 4 SO3[citation needed]

Aluminium sulfate reacts with sodium bicarbonate to which foam stabilizer has been added, typically made from saponin, licorice root, or hydrolyzed animal protein in aqueous solution, forming fire-extinguishing foams, producing carbon dioxide

Al2(SO4)3 + 6 NaHCO3 2 Al(OH)3 + 3 Na2SO4 + 6 CO2

The carbon dioxide is trapped by the foam stabilizer and creates a thick foam which will float on top of hydrocarbon fuels and seal off access to atmospheric oxygen, smothering the fire. Chemical foam was unsuitable for use on polar solvents such as alcohol, as the fuel would mix with and break down the foam blanket. The carbon dioxide generated also served to propel the foam out of the container, be it a portable fire extinguisher or fixed installation using hoselines. Chemical foam is considered obsolete in the United States and has been replaced by synthetic mechanical foams, such as AFFF which have a longer shelf life, are more effective, and more versatile, although some counties such as Japan and India continue to use it.

References

Footnotes

^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398

^ Global Health and Education Foundation (2007). "Conventional Coagulation-Flocculation-Sedimentation". Safe Drinking Water is Essential. National Academy of Sciences. http://drinking-water.org/html/en/Treatment/Coagulation-Flocculation-technologies.html. Retrieved 2007-12-01. 

^ Kvech S, Edwards M (2002). "Solubility controls on aluminum in drinking water at relatively low and high pH". WATER RESEARCH 36 (17): 43564368. doi:10.1016/S0043-1354(02)00137-9. PMID 12420940. 

^ U.S. Court of Appeals for the Ninth Circuit (February 2, 2010). "U.S. v. Ressam". http://www.nefafoundation.org/miscellaneous/US_v_Ressam_9thcircuitappeals0210.pdf. Retrieved February 27, 2010. 

^ "Complaint; U.S. v. Ressam". NEFA Foundation. December 1999. http://nefafoundation.org/miscellaneous/FeaturedDocs/U.S._v_Ressam_Complaint.pdf. Retrieved February 26, 2010. 

Notations

Pauling, Linus (1970). General Chemistry. W.H. Freeman: San Francisco. ISBN 0-486-65622-5. 

External links

International Chemical Safety Card 1191

NIOSH Pocket Guide to Chemical Hazards

WHO Food Additive Series No. 12

Aluminum and health

v  d  e

  Aluminium compounds

AlAs  AlB2  AlB12  Al(BH4)3  AlBr3  AlCl  AlCl3  AlF  AlF3  AlH3  AlI3  AlN  Al(NO3)3  AlO  Al(OH)3  AlON  AlP  AlPO4  AlSb  Al2(MoO4)3  Al2O3  Al2S3  Al2(SO4)3  Al2Se3  Al2SiO5  Al4C3

Categories: Aluminium compounds | Sulfates | Molluscicides | Water treatmentHidden categories: Articles needing additional references from August 2009 | All articles needing additional references | Chemboxes which contain changes to watched fields | All articles with unsourced statements | Articles with unsourced statements from August 2009
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