Difference between revisions of "Aluminium hydroxide"

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{{chembox
 
{{chembox
 
| verifiedrevid = 322319835
 
| verifiedrevid = 322319835
−
|   Name = Aluminium hydroxide
+
| Name = Aluminium hydroxide
−
|   ImageFile = Gibbsite-crystal-3D-balls.png
+
| ImageFile = Gibbsite-crystal-3D-balls.png
−
|   ImageFile2 = Hydroxid hlinitý.PNG
+
| ImageFile2 = Hydroxid hlinitý.PNG
−
|   IUPACName = Aluminium hydroxide
+
| IUPACName = Aluminium hydroxide
−
|  OtherNames = Aluminium(III) hydroxide,<br />Hydrated alumina
+
|  OtherNames = Hydrated alumina<br/>[[Gibbsite]]
 
| Section1 = {{Chembox Identifiers
 
| Section1 = {{Chembox Identifiers
 
|  ChemSpiderID = 8351587
 
|  ChemSpiderID = 8351587
−
| InChI = 1/Al.3H2O/h;3*1H2/q+3;;;/p-3
+
|   InChI = 1/Al.3H2O/h;3*1H2/q+3;;;/p-3
−
| SMILES = [Al+3].[OH-].[OH-].[OH-]
+
|   InChIKey = WNROFYMDJYEPJX-DFZHHIFOAJ
−
| InChIKey = WNROFYMDJYEPJX-DFZHHIFOAJ
+
|  StdInChI = 1S/Al.3H2O/h;3*1H2/q+3;;;/p-3
−
| CASNo = 21645-51-2
+
|   StdInChIKey = WNROFYMDJYEPJX-UHFFFAOYSA-K
−
|   CASNo_Ref = {{cascite}}
+
|   CASNo = 21645-51-2
 +
|   CASNo_Ref = {{cascite}}
 
|  RTECS = BD0940000
 
|  RTECS = BD0940000
 +
|  EC-number = 244-492-7
 +
|  ATCCode_prefix = A02
 +
|  ATCCode_suffix = AB01
 
   }}
 
   }}
 
| Section2 = {{Chembox Properties
 
| Section2 = {{Chembox Properties
 
|  Formula = Al(OH)<sub>3</sub>
 
|  Formula = Al(OH)<sub>3</sub>
 
|  MolarMass = 78.00 g/mol
 
|  MolarMass = 78.00 g/mol
−
|  Appearance = White [[amorphous]] powder
+
|  Appearance = White amorphous powder
−
|  Density = 2.42 g/cm³, solid
+
|  Density = 2.42 g/cm<sup>3</sup>, solid
−
|  Solubility = 0.0001 g/100 mL (20 °C)
+
|  Solubility = 0.0001 g/100 ml (20 °C)
−
|  SolubleOther = soluble in [[acid]]s, [[alkali]]es, [[hydrochloric acid|HCl]], [[sulfuric acid|HSO<sub>4</sub>]]
+
|  SolubleOther = soluble in [[acid]]s, [[alkali]]s
−
|  MeltingPtC = 300
+
|  MeltingPt = 300 °C ''dehydr.''
−
|  BoilingPt =
 
−
|  pKa = >7
 
 
   }}
 
   }}
 
| Section7 = {{Chembox Hazards
 
| Section7 = {{Chembox Hazards
−
|  EUClass = Irritant ('''I''') Xi
+
|  EUIndex = not listed
−
|  RPhrases = {{R36}} {{R37}} {{R38}}
+
|  FlashPt = non-flammable
−
|  SPhrases = {{S26}} {{S36}}
+
|  ExternalMSDS = {{ICSC-small|0373}}
−
|  FlashPt = Non-flammable
+
   }}
−
|  NFPA-H = 1 | NFPA-F = 0 | NFPA-R = 0
 
−
|   ExternalMSDS = [http://physchem.ox.ac.uk/MSDS/AL/aluminium_hydroxide.html External MSDS]  }}
 
 
| Section8 = {{Chembox Related
 
| Section8 = {{Chembox Related
−
|  OtherAnions = None
+
|  OtherAnions = [[Aluminium oxide hydroxide]]<br/>[[Aluminium oxide]]
−
|  OtherCpds = [[Sodium oxide]],<br />[[aluminium oxide hydroxide]]
+
|  OtherCations = [[Boric acid]]<br/>[[Gallium hydroxide]]
 
   }}
 
   }}
 
}}
 
}}
  
−
'''Aluminium hydroxide''', Al(OH)<sub>3</sub>, Alum, is the most stable form of [[aluminium]] in normal conditions. It is found in nature as the mineral [[gibbsite]] (also known as hydrargillite) and its three, much more rare, polymorphs: bayerite, doyleite and nordstrandite. Closely related are [[aluminium oxide hydroxide]], AlO(OH), and [[aluminium oxide]], Al<sub>2</sub>O<sub>3</sub>, differing only by loss of water. These compounds together are the major components of the aluminium [[ore]] [[bauxite]].  Freshly precipitated aluminium hydroxide forms [[gel]]s, which is the basis for application of aluminium salts as [[flocculation|flocculants]] in water purification. This gel crystallizes with time. Aluminium hydroxide gels can be dehydrated (e.g., with the utility of water-miscible non-aqueous solvents like ethanol) to form an amorphous aluminium hydroxide powder, which is readily soluble in acids. Heat-dried aluminium hydroxide powder is known as activated alumina and is used in gas purification, as a catalyst support and an abrasive.
+
'''Aluminium hydroxide''', Al(OH)<sub>3</sub>, is a common form of [[aluminium]] in normal conditions. It is found in nature as the mineral [[gibbsite]] (also known as hydrargillite) and its three, much more rare, polymorphs: bayerite, doyleite and nordstrandite. Closely related are [[aluminium oxide hydroxide]], AlO(OH), and [[aluminium oxide]], Al<sub>2</sub>O<sub>3</sub>, differing only by loss of water. These compounds together are the major components of the aluminium [[ore]] [[bauxite]].  Freshly precipitated aluminium hydroxide forms [[gel]]s, which is the basis for application of aluminium salts as [[flocculation|flocculants]] in water purification. This gel crystallizes with time. Aluminium hydroxide gels can be dehydrated (e.g., with the utility of water-miscible non-aqueous solvents like ethanol) to form an amorphous aluminium hydroxide powder, which is readily soluble in acids. Heat-dried aluminium hydroxide powder is known as activated alumina and is used in gas purification, as a catalyst support and an abrasive.
  
 
==Production==
 
==Production==
−
Aluminium hydroxide is an intermediate product in the [[Bayer process]]. In this process, [[bauxite]] is dissolved in hot [[sodium hydroxide]] solution, and insolubilities are filtered off. On cooling, aluminium hydroxide precipitates. The aluminium hydroxide is further calcined to give alumina, which may be smelted in the [[Hall-Héroult process]] in order to produce aluminium.
+
Aluminium hydroxide is an intermediate product in the [[Bayer process]]. In this process, [[bauxite]] is dissolved in hot [[sodium hydroxide]] solution, and insolubilities are filtered off. On cooling, aluminium hydroxide precipitates. The aluminium hydroxide is further calcined to give alumina, which may be smelted in the [[Hall–Héroult process]] in order to produce aluminium.
  
 
==Chemistry==
 
==Chemistry==
−
Gibbsite has a typical metal hydroxide structure with [[hydrogen bonds]]. It is built up of double layers of hydroxyl groups with aluminium ions occupying two-thirds of the octahedral holes between the two layers.<ref>A. F. Wells, ''Structural Inorganic Chemistry'', 4th. edition 1975, Oxford University Press.</ref>
+
Gibbsite has a typical metal hydroxide structure with [[hydrogen bonds]]. It is built up of double layers of hydroxyl groups with aluminium ions occupying two-thirds of the octahedral holes between the two layers.<ref>{{Wells5th}}.</ref>
  
−
Aluminium hydroxide is [[amphoteric]]. It dissolves in [[acid]], forming Al(H<sub>2</sub>O)<sub>6</sub><sup>3+</sup> (hexaaquaaluminate) or its [[hydrolysis]] products. It also dissolves in strong [[alkali]], forming Al(OH)<sub>4</sub><sup>-</sup> (tetrahydroxoaluminate).
+
Aluminium hydroxide is [[amphoteric]]. It dissolves in [[acid]], forming Al(H<sub>2</sub>O)<sub>6</sub><sup>3+</sup> (hexaaquaaluminate) or its [[hydrolysis]] products. It also dissolves in strong [[alkali]], forming Al(OH)<sub>4</sub><sup>-</sup> (tetrahydroxidoaluminate).
  
 
==Pharmacology==
 
==Pharmacology==
−
Pharmacologically, this compound is used as an [[antacid]] under names such as Alu-Cap, Aludrox or Pepsamar. The hydroxide reacts with excess acid in the stomach, reducing its acidity.<ref>{{cite book | author = Galbraith, A; Bullock, S; Manias, E. Hunt, B. & Richards, A. | year = 1999 | title =  Fundamentals of pharmacology: a text for nurses and health professionals | location = Harlow | publisher = Pearson | pages = 482}}</ref> This decrease of acidity of the contents of the stomach may in turn help to relieve the symptoms of [[peptic ulcer|ulcers]], [[heartburn]] or [[dyspepsia]]. It can also cause constipation and is therefore often used with [[magnesium hydroxide]] or [[magnesium carbonate]], which have counterbalancing [[laxative]] effects.  This compound is also used to control [[phosphate]] (phosphorus) levels in the blood of people suffering from kidney failure.
+
Pharmacologically, this compound is used as an [[antacid]] under names such as Alu-Cap, Aludrox or Pepsamar. The hydroxide reacts with excess acid in the stomach, reducing its acidity.<ref>{{citation | last1 = Galbraith | first1 = A. | last2 = Bullock | first2 = S. | last3 = Manias | first3 = E. | last4 = Hunt | first4 = B. | last5 = Richards | first5 = A. | year = 1999 | title =  Fundamentals of pharmacology: a text for nurses and health professionals | location = Harlow | publisher = Pearson | page = 482}}.</ref> This decrease of acidity of the contents of the stomach may in turn help to relieve the symptoms of [[peptic ulcer|ulcers]], [[heartburn]] or [[dyspepsia]]. It can also cause constipation and is therefore often used with [[magnesium hydroxide]] or [[magnesium carbonate]], which have counterbalancing [[laxative]] effects.  This compound is also used to control [[phosphate]] (phosphorus) levels in the blood of people suffering from kidney failure.
  
−
Aluminium hydroxide, alum, is included as an [[adjuvant]] in some [[vaccine]]s (e.g., ''[[Alhydrogel]]'', [[Anthrax Vaccine]]), since it appears to contribute to induction of a good [[antibody]] (Th2) response. Its pharmacological action is not known. However, it has little capacity to stimulate cellular (Th1) immune responses, important for protection against many pathogens.<ref>{{cite journal | author = Petrovsky N, Aguilar JC. | title = Vaccine adjuvants: current state and future trends | journal = [[Immunol Cell Biol.]] | year = 2004 | volume = 82 | issue = 5 | pages = 488–96 | doi = 10.1111/j.0818-9641.2004.01272.x}}</ref>
+
Aluminium hydroxide, alum, is included as an [[adjuvant]] in some [[vaccine]]s (e.g., ''[[Alhydrogel]]'', [[Anthrax vaccine]]), since it appears to contribute to induction of a good [[antibody]] (Th2) response. Its pharmacological action is not known. However, it has little capacity to stimulate cellular (Th1) immune responses, important for protection against many pathogens.<ref>{{citation | last1 = Petrovsky | first1 = Nikolai | last2 = Aguilar | first2 = Julio César | title = Vaccine adjuvants: current state and future trends | journal = Immunol. Cell Biol. | year = 2004 | volume = 82 | issue = 5 | pages = 488–96 | doi = 10.1111/j.0818-9641.2004.01272.x}}.</ref>
  
−
Because the brain lesions found in [[Alzheimer's disease]] sometimes contain traces of aluminium, there is concern that consumption of excess aluminium compounds may cause or contribute to the development of this and other [[neurodegenerative disease]]s.<ref>{{cite journal |author=Perl DP, Moalem S |title=Aluminum and Alzheimer's disease, a personal perspective after 25 years |journal=J. Alzheimers Dis. |volume=9 |issue=3 Suppl |pages=291–300 |year=2006 |pmid=17004365 |doi= |url=http://iospress.metapress.com/openurl.asp?genre=article&issn=1387-2877&volume=9&issue=3&spage=291}}</ref><ref>{{cite journal |author=Kawahara M |title=Effects of aluminum on the nervous system and its possible link with neurodegenerative diseases |journal=J. Alzheimers Dis. |volume=8 |issue=2 |pages=171–82; discussion 209–15 |year=2005 |month=November |pmid=16308486 |doi= |url=http://iospress.metapress.com/openurl.asp?genre=article&issn=1387-2877&volume=8&issue=2&spage=171}}</ref> However, multiple epidemiological studies have found no connection between exposure to aluminium and neurological disorders.<ref>{{cite journal
+
Because the brain lesions found in [[Alzheimer's disease]] sometimes contain traces of aluminium, there is concern that consumption of excess aluminium compounds may cause or contribute to the development of this and other [[neurodegenerative disease]]s.<ref>{{citation | last1 = Perl | first1 = Daniel P. | last2 = Moalem | first2 = Sharon | title = Aluminum and Alzheimer's disease, a personal perspective after 25 years | journal = J. Alzheimers Dis. | volume = 9 | issue = Suppl. 3 | pages = 291–300 | year = 2006 | pmid = 17004365 | doi = | url = http://iospress.metapress.com/content/arc12wra19tk8a9r/?p=ec09da7f1ac04920863f68bb00e5ca4f&pi=1&hl=u}}.</ref><ref>{{citation | last = Kawahara | first = Masahiro | title = Effects of aluminum on the nervous system and its possible link with neurodegenerative diseases | journal = J. Alzheimers Dis. | volume = 8 | issue = 2 | pages = 171–82; discussion 209–15 | year = 2005 | pmid = 16308486 | doi = | url = http://iospress.metapress.com/openurl.asp?genre=article&issn=1387-2877&volume=8&issue=2&spage=171}}.</ref> However, multiple epidemiological studies have found no connection between exposure to aluminium and neurological disorders.<ref>{{citation | last = Rondeau | first = V. | title = A review of epidemiologic studies on aluminum and silica in relation to Alzheimer's disease and associated disorders | journal = Rev. Environ. Health | volume = 17 | issue = 2 | pages = 107–21 | year = 2002 | pmid = 12222737}}.</ref><ref>{{citation | last1 = Martyn | first1 = C. N. | last2 = Coggon | first2 = D. N. | last3 = Inskip | first3 = H. | last4 = Lacey | first4 = R. F. | last5 = Young | first5 = W. F. | title = Aluminum concentrations in drinking water and risk of Alzheimer's disease | journal = Epidemiology | volume = 8 | issue = 3 | pages = 281–86 | year = 1997 | pmid = 9115023 | doi = 10.1097/00001648-199705000-00009}}.</ref><ref>{{citation | last1 = Graves | first1 = A. B. | last2 = Rosner | first2 = D. | last3 = Echeverria | first3 = D. | last4 = Mortimer | first4 = J. A. | last5 = Larson | first5 = E. B. | title = Occupational exposures to solvents and aluminium and estimated risk of Alzheimer's disease | journal = Occup. Environ. Med. | volume = 55 | issue = 9 | pages = 627–33 | year = 1998 | pmid = 9861186 | doi = 10.1136/oem.55.9.627}}.</ref>
−
|author=Rondeau V
 
−
|title=A review of epidemiologic studies on aluminum and silica in relation to Alzheimer's disease and associated disorders
 
−
|journal=Rev Environ Health
 
−
|volume=17
 
−
|issue=2
 
−
|pages=107–21
 
−
|year=2002
 
−
|pmid=12222737
 
−
}}</ref><ref>{{cite journal
 
−
|author=Martyn CN, Coggon DN, Inskip H, Lacey RF, Young WF
 
−
|title=Aluminum concentrations in drinking water and risk of Alzheimer's disease
 
−
|journal=Epidemiology
 
−
|volume=8
 
−
|issue=3
 
−
|pages=281–6
 
−
|year=1997
 
−
|month=May
 
−
|pmid=9115023
 
−
|doi=10.1097/00001648-199705000-00009
 
−
}}</ref><ref>{{cite journal
 
−
|author=Graves AB, Rosner D, Echeverria D, Mortimer JA, Larson EB
 
−
|title=Occupational exposures to solvents and aluminium and estimated risk of Alzheimer's disease
 
−
|journal=Occup Environ Med
 
−
|volume=55
 
−
|issue=9
 
−
|pages=627–33
 
−
|year=1998
 
−
|month=September
 
−
|pmid=9861186
 
−
|pmc=1757634
 
−
|doi=10.1136/oem.55.9.627
 
−
}}</ref>
 
  
−
In addition, elevated aluminium levels in blood, resulting from kidney dialysis with well water containing high aluminium, may result in [[dementia]] that is similar to but probably different from that of Alzheimer's disease.<ref>{{cite journal |author=Carpenter DO |title=Effects of metals on the nervous system of humans and animals |journal=Int J Occup Med Environ Health |volume=14 |issue=3 |pages=209–18 |year=2001 |pmid=11764847 |doi= |url=}}</ref>. However, this hypothesis is controversial.
+
In addition, elevated aluminium levels in blood, resulting from kidney dialysis with well water containing high aluminium, may result in [[dementia]] that is similar to but probably different from that of Alzheimer's disease.<ref>{{citation | last = Carpenter | first = D. O. | title = Effects of metals on the nervous system of humans and animals | journal = Int. J. Occup. Med. Environ. Health | volume = 14 | issue = 3 | pages = 209–18 | year = 2001 | pmid = 11764847 | doi = }}.</ref>. However, this hypothesis is controversial.
  
−
In 2007, tests with mice of the [[anthrax vaccine]] using aluminium hydroxide adjuvant were reported as resulting in adverse neuropathy symptoms.<ref>{{cite journal | author=Petrik MS, Wong MC, Tabata RC, Garry RF, Shaw CA. | title=Aluminum adjuvant linked to Gulf War illness induces motor neuron death in mice. | journal=Neuromolecular Med. | year=2007 | issue=9 | pages=83–100 |pmid= |doi= 10.1385/NMM:9:1:83|url= | volume=9 }}</ref>
+
In 2007, tests with mice of the [[anthrax vaccine]] using aluminium hydroxide adjuvant were reported as resulting in adverse neuropathy symptoms.<ref>{{citation | lat1 = Petrik | first1 = M. S. | last2 = Wong | first2 = M. C. | last3 = Tabata | first3 = R. C. | last4 = Garry | first4 = R. F. | last5 = Shaw | first5 = C. A. | title = Aluminum adjuvant linked to Gulf War illness induces motor neuron death in mice | journal = Neuromol. Med. | year = 2007 | volume = 9 | issue = 9 | pages = 83–100 | doi = 10.1385/NMM:9:1:83}}.</ref>
  
 
==Use as a fire retardant==
 
==Use as a fire retardant==
−
 
+
Aluminium hydroxide also finds use as a fire retardant filler for polymer applications in a similar way to [[magnesium hydroxide]] and [[hydromagnesite]]. It decomposes at about 180–200&nbsp;°C giving off water vapour.
−
Aluminium hydroxide also finds use as a fire retardant filler for polymer applications in a similar way to [[magnesium hydroxide]] and [[hydromagnesite]]. It decomposes at about 180 °C giving off water vapour.
 
  
 
==References==
 
==References==
−
<references/>
+
{{reflist}}
  
 
==External links==
 
==External links==
−
* [http://www.ilo.org/public/english/protection/safework/cis/products/icsc/dtasht/_icsc03/icsc0373.htm International Chemical Safety Card 0373]
+
*{{ICSC|0373}}
 +
*{{PGCH|0024}}
 +
*{{EHC|194|name=Aluminium}}
 +
*{{HSDB|name=Aluminum hydroxide}}
 +
*{{JEFCA-mono|url=http://www.inchem.org/documents/jecfa/jecmono/v024je07.htm | name=Aluminium | whoseries=24}}
 +
*{{EHC|192|name=Flame Retardants: A General Introduction}}
  
 
{{Antacids}}
 
{{Antacids}}
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[[Category:Aluminium compounds]]
 
[[Category:Aluminium compounds]]
 
[[Category:Hydroxides]]
 
[[Category:Hydroxides]]
−
[[Category:Phosphate binders]]
 
 
[[Category:Antacids]]
 
[[Category:Antacids]]
 +
[[Category:Flame retardants]]
  
 
{{Imported from Wikipedia|name=Aluminium hydroxide|id=327029915}}
 
{{Imported from Wikipedia|name=Aluminium hydroxide|id=327029915}}

Latest revision as of 05:33, 28 November 2009

Aluminium hydroxide
Gibbsite-crystal-3D-balls.png
Hydroxid hlinitý.PNG
IUPAC name Aluminium hydroxide
Other names Hydrated alumina
Gibbsite
Identifiers
InChI InChI=1/Al.3H2O/h;3*1H2/q+3;;;/p-3
InChIKey WNROFYMDJYEPJX-DFZHHIFOAJ
Standard InChI InChI=1S/Al.3H2O/h;3*1H2/q+3;;;/p-3
Standard InChIKey WNROFYMDJYEPJX-UHFFFAOYSA-K
CAS number [21645-51-2]
EC number 244-492-7
RTECS BD0940000
ATC code A02AB01
ChemSpider 8351587
Properties
Chemical formula Al(OH)3
Molar mass 78.00 g/mol
Appearance White amorphous powder
Density 2.42 g/cm3, solid
Melting point

300 °C dehydr.

Solubility in water 0.0001 g/100 ml (20 °C)
Solubility soluble in acids, alkalis
Hazards
Material safety data sheet (MSDS) ICSC 0373
EU index number not listed
Flash point non-flammable
Related compounds
Other anions Aluminium oxide hydroxide
Aluminium oxide
Other cations Boric acid
Gallium hydroxide
 Template:Tick(what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Aluminium hydroxide, Al(OH)3, is a common form of aluminium in normal conditions. It is found in nature as the mineral gibbsite (also known as hydrargillite) and its three, much more rare, polymorphs: bayerite, doyleite and nordstrandite. Closely related are aluminium oxide hydroxide, AlO(OH), and aluminium oxide, Al2O3, differing only by loss of water. These compounds together are the major components of the aluminium ore bauxite. Freshly precipitated aluminium hydroxide forms gels, which is the basis for application of aluminium salts as flocculants in water purification. This gel crystallizes with time. Aluminium hydroxide gels can be dehydrated (e.g., with the utility of water-miscible non-aqueous solvents like ethanol) to form an amorphous aluminium hydroxide powder, which is readily soluble in acids. Heat-dried aluminium hydroxide powder is known as activated alumina and is used in gas purification, as a catalyst support and an abrasive.

Production

Aluminium hydroxide is an intermediate product in the Bayer process. In this process, bauxite is dissolved in hot sodium hydroxide solution, and insolubilities are filtered off. On cooling, aluminium hydroxide precipitates. The aluminium hydroxide is further calcined to give alumina, which may be smelted in the Hall–Héroult process in order to produce aluminium.

Chemistry

Gibbsite has a typical metal hydroxide structure with hydrogen bonds. It is built up of double layers of hydroxyl groups with aluminium ions occupying two-thirds of the octahedral holes between the two layers.[1]

Aluminium hydroxide is amphoteric. It dissolves in acid, forming Al(H2O)63+ (hexaaquaaluminate) or its hydrolysis products. It also dissolves in strong alkali, forming Al(OH)4- (tetrahydroxidoaluminate).

Pharmacology

Pharmacologically, this compound is used as an antacid under names such as Alu-Cap, Aludrox or Pepsamar. The hydroxide reacts with excess acid in the stomach, reducing its acidity.[2] This decrease of acidity of the contents of the stomach may in turn help to relieve the symptoms of ulcers, heartburn or dyspepsia. It can also cause constipation and is therefore often used with magnesium hydroxide or magnesium carbonate, which have counterbalancing laxative effects. This compound is also used to control phosphate (phosphorus) levels in the blood of people suffering from kidney failure.

Aluminium hydroxide, alum, is included as an adjuvant in some vaccines (e.g., Alhydrogel, Anthrax vaccine), since it appears to contribute to induction of a good antibody (Th2) response. Its pharmacological action is not known. However, it has little capacity to stimulate cellular (Th1) immune responses, important for protection against many pathogens.[3]

Because the brain lesions found in Alzheimer's disease sometimes contain traces of aluminium, there is concern that consumption of excess aluminium compounds may cause or contribute to the development of this and other neurodegenerative diseases.[4][5] However, multiple epidemiological studies have found no connection between exposure to aluminium and neurological disorders.[6][7][8]

In addition, elevated aluminium levels in blood, resulting from kidney dialysis with well water containing high aluminium, may result in dementia that is similar to but probably different from that of Alzheimer's disease.[9]. However, this hypothesis is controversial.

In 2007, tests with mice of the anthrax vaccine using aluminium hydroxide adjuvant were reported as resulting in adverse neuropathy symptoms.[10]

Use as a fire retardant

Aluminium hydroxide also finds use as a fire retardant filler for polymer applications in a similar way to magnesium hydroxide and hydromagnesite. It decomposes at about 180–200 °C giving off water vapour.

References

  1. ↑ Wells, A. F. Structural Inorganic Chemistry, 5th ed.; Clarendon Press: Oxford, 1984. ISBN 0-19-855370-6.
  2. ↑ Galbraith, A.; Bullock, S.; Manias, E.; Hunt, B.; Richards, A. Fundamentals of pharmacology: a text for nurses and health professionals; Pearson: Harlow, 1999; p 482.
  3. ↑ Petrovsky, Nikolai; Aguilar, Julio César Vaccine adjuvants: current state and future trends. Immunol. Cell Biol. 2004, 82 (5), 488–96. DOI: 10.1111/j.0818-9641.2004.01272.x.
  4. ↑ Perl, Daniel P.; Moalem, Sharon Aluminum and Alzheimer's disease, a personal perspective after 25 years. J. Alzheimers Dis. 2006, 9 (Suppl. 3), 291–300. PMID 17004365, <http://iospress.metapress.com/content/arc12wra19tk8a9r/?p=ec09da7f1ac04920863f68bb00e5ca4f&pi=1&hl=u>.
  5. ↑ Kawahara, Masahiro Effects of aluminum on the nervous system and its possible link with neurodegenerative diseases. J. Alzheimers Dis. 2005, 8 (2), 171–82; discussion 209–15. PMID 16308486, <http://iospress.metapress.com/openurl.asp?genre=article&issn=1387-2877&volume=8&issue=2&spage=171>.
  6. ↑ Rondeau, V. A review of epidemiologic studies on aluminum and silica in relation to Alzheimer's disease and associated disorders. Rev. Environ. Health 2002, 17 (2), 107–21. PMID 12222737.
  7. ↑ Martyn, C. N.; Coggon, D. N.; Inskip, H.; Lacey, R. F.; Young, W. F. Aluminum concentrations in drinking water and risk of Alzheimer's disease. Epidemiology 1997, 8 (3), 281–86. PMID 9115023. DOI: 10.1097/00001648-199705000-00009.
  8. ↑ Graves, A. B.; Rosner, D.; Echeverria, D.; Mortimer, J. A.; Larson, E. B. Occupational exposures to solvents and aluminium and estimated risk of Alzheimer's disease. Occup. Environ. Med. 1998, 55 (9), 627–33. PMID 9861186. DOI: 10.1136/oem.55.9.627.
  9. ↑ Carpenter, D. O. Effects of metals on the nervous system of humans and animals. Int. J. Occup. Med. Environ. Health 2001, 14 (3), 209–18. PMID 11764847.
  10. ↑ Aluminum adjuvant linked to Gulf War illness induces motor neuron death in mice. Neuromol. Med. 2007, 9 (9), 83–100. DOI: 10.1385/NMM:9:1:83.

External links

Template:Antacids

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