View source for Chemistry:Aluminium hydroxide

{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 476993259
| ImageFile = Gibbsite-crystal-3D-balls.png
| ImageName = Unit cell ball and stick model of aluminium hydroxide
| ImageFile1 = Hydroxid hlinitý.PNG
| ImageName1 = Sample of aluminium hydroxide in a vial
| PIN = Aluminium hydroxide
| SystematicName = Trihydroxidoaluminium
| OtherNames = {{ubl|Aluminic acid|Aluminic hydroxide|Alumanetriol|Aluminium(III) hydroxide|Aluminium hydroxide|Aluminium trihydroxide|<!--See Pubchem-->Hydrated alumina|Orthoaluminic acid}}
|Section1={{Chembox Identifiers
| InChI = 1/Al.3H2O/h;3*1H2/q+3;;;/p-3
| InChIKey = WNROFYMDJYEPJX-DFZHHIFOAJ
| CASNo = 21645-51-2
| CASNo_Ref = {{cascite|correct|CAS}}
| DrugBank = DB06723
| KEGG = D02416
| PubChem = 10176082
| ChemSpiderID = 8351587
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| ChEMBL = 1200706
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 5QB0T2IUN0
| RTECS = BD0940000
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 33130
| SMILES = [OH-].[OH-].[OH-].[Al+3]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Al.3H2O/h;3*1H2/q+3;;;/p-3
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = WNROFYMDJYEPJX-UHFFFAOYSA-K<br />{{ATC|A02|AB02}} (algeldrate)
}}
|Section2={{Chembox Properties
| Properties_ref =<ref>For solubility product: {{cite web|url=http://www.ktf-split.hr/periodni/en/abc/kpt.html |title=Solubility product constants |access-date=2012-05-17 |url-status=dead |archive-url=https://web.archive.org/web/20120615020049/http://www.ktf-split.hr/periodni/en/abc/kpt.html |archive-date=15 June 2012 }}</ref><ref>For isoelectric point: {{Cite journal | last1=Gayer | first1=K. H. | last2=Thompson | first2=L. C. | last3=Zajicek | first3=O. T. | title=The solubility of aluminum hydroxide in acidic and basic media at 25 ?c | journal=Canadian Journal of Chemistry | date=September 1958 | doi=10.1139/v58-184 | issn=0008-4042 | volume=36 | issue=9 | pages=1268–1271| doi-access=free }}</ref>
| Formula = {{chem2|Al(OH)3}}
| Al=1|O=3|H=3
| Appearance = White [[Physics:Amorphous|amorphous]] powder
| Density = 2.42 g/cm<sup>3</sup>, solid
| Solubility = 0.0001 g/(100 mL)
| SolubleOther = soluble in [[Chemistry:Acid|acid]]s and [[Chemistry:Alkali|alkali]]s
| SolubilityProduct = 3×10<sup>−34</sup>
| MeltingPtC = 300
| BoilingPt =
| pKa = >7
| IsoelectricPt = 7.7
  }}
|Section5={{Chembox Thermochemistry
| Thermochemistry_ref = <ref>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles |edition=6th| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7}}</ref>
| DeltaHf = −1277&nbsp;kJ·mol<sup>−1</sup>
 }}
|Section6={{Chembox Pharmacology
| Pharmacology_ref = <ref>{{Cite journal | last1=Black | first1=Ronald A. | last2=Hill | first2=D. Ashley | title=Over-the-Counter Medications in Pregnancy | journal=American Family Physician | access-date=2017-07-01 | date=2003-06-15 | url=http://www.aafp.org/afp/2003/0615/p2517.html | issn=0002-838X | volume=67 | issue=12 | pages=2517–2524| pmid=12825840 }}</ref>
| ATCCode_prefix = A02
| ATCCode_suffix = AB01
| ATC_Supplemental =
}}
|Section7={{Chembox Hazards
| GHSPictograms = no GHS pictograms
| HPhrases = no hazard statements
| PPhrases = {{P-phrases|264|261|280|271|312|304+340|305+351+338|337+313}}
| FlashPt = Non-flammable
| NFPA-H = 1 | NFPA-F = 0 | NFPA-R = 0
| ExternalSDS = [https://www.fishersci.com/shop/msdsproxy?productName=AC219130250&productDescription=ALUMINUM+HYDROXIDE+POWDER+25G&catNo=AC219130250&vendorId=VN00032119&storeId=10652 External MSDS]
 | LD50 = >5000&nbsp;mg/kg (rat, oral)
}}
|Section8={{Chembox Related
| OtherAnions = None
| OtherCompounds = {{ubl|[[Chemistry:Boric acid|Boric acid]]|[[Chemistry:Gallium(III) hydroxide|Gallium(III) hydroxide]]|[[Chemistry:Indium(III) hydroxide|Indium(III) hydroxide]]|[[Chemistry:Thallium(III) hydroxide|Thallium(III) hydroxide]]|[[Chemistry:Scandium(III) hydroxide|Scandium(III) hydroxide]]|[[Chemistry:Sodium oxide|Sodium oxide]]|Aluminium oxide hydroxide}}
  }}
}}

'''Aluminium hydroxide''', {{chem2|Al([[Chemistry:Hydroxide|OH]])3}}, is found in nature as the mineral [[Chemistry:Gibbsite|gibbsite]] (also known as hydrargillite) and its three much rarer [[Physics:Polymorphism (materials science)|polymorphs]]: bayerite, [[Chemistry:Doyleite|doyleite]], and nordstrandite. Aluminium hydroxide is [[Chemistry:Amphoterism|amphoteric]], i.e., it has both [[Chemistry:Base|basic]] and acidic properties. Closely related are aluminium oxide hydroxide, AlO(OH), and [[Chemistry:Aluminium oxide|aluminium oxide]] or alumina ({{chem2|Al2O3}}), the latter of which is also amphoteric. These compounds together are the major components of the aluminium [[Earth:Ore|ore]] [[Earth:Bauxite|bauxite]]. Aluminium hydroxide also forms a gelatinous precipitate in water.

==Structure==
{{chem2|Al(OH)3}} is built up of double layers of hydroxyl groups with aluminium ions occupying two-thirds of the octahedral holes between the two layers.<ref>{{Wells4th}}</ref><ref name="properties">{{Cite book | editor=A. J. Downs | last=Evans | first=K. A. | title=Chemistry of aluminium, gallium, indium, and thallium | chapter=Properties and uses of aluminium oxides and aluminium hydroxides | location=London; New York | date=1993 | edition=1st | publisher=Blackie Academic & Professional | isbn=9780751401035}}</ref> Four [[Physics:Polymorphism (materials science)|polymorph]]s are recognized.<ref name = Karamalidis>{{cite book | last = Karamalidis | first = A. K. |author2=Dzombak D. A. | year = 2010 | publisher = {{wipe|John Wiley & Sons}} | url = https://books.google.com/books?id=XULsOFSipsgC&pg=PA15 | pages=15–17 | title = Surface Complexation Modeling: Gibbsite | isbn = 978-0-470-58768-3 }}</ref> All feature layers of [[Octahedron|octahedral]] aluminium hydroxide units, with [[Chemistry:Hydrogen bond|hydrogen bond]]s between the layers. The polymorphs differ in terms of the stacking of the layers. All forms of {{chem2|Al(OH)3}} crystals are hexagonal {{Disputed inline|date=October 2020}}:
* [[Chemistry:Gibbsite|gibbsite]] is also known as γ-{{chem2|Al(OH)3}} <ref name=":1">{{Cite book|last1=Wefers|first1=Karl|url=http://worldcat.org/oclc/894928306|title=Oxides and hydroxides of aluminum|last2=Misra|first2=Chanakya|date=1987|publisher=Alcoa Research Laboratories|pages=2|oclc=894928306}}</ref> or α-{{chem2|Al(OH)3}} {{Citation needed|date=October 2020}}
* bayerite is also known as α-{{chem2|Al(OH)3}}<ref name=":1" /> or ''β-alumina trihydrate''{{citation needed|date=March 2021}}
* nordstrandite is also known as {{chem2|Al(OH)3}}<ref name=":1" />
* [[Chemistry:Doyleite|doyleite]]

''Hydrargillite'', once thought to be aluminium hydroxide, is an [[Chemistry:Aluminium phosphate|aluminium phosphate]]. Nonetheless, both ''gibbsite'' and ''hydrargillite'' refer to the same polymorphism of aluminium hydroxide, with ''gibbsite'' used most commonly in the United States and ''hydrargillite'' used more often in Europe. Hydrargillite is named after the [[Social:Greek language|Greek]] words for water (''{{lang|grc-Latn|hydra}}'') and clay (''{{lang|grc-Latn|argylles}}'').

==Properties==
Aluminium hydroxide is amphoteric. In [[Chemistry:Acid|acid]], it acts as a Brønsted–Lowry base. It neutralizes the acid, yielding a salt:<ref name=":0">{{Cite web |url=https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/acids-and-bases-15/acid-base-properties-of-oxides-114/basic-and-amphoteric-hydroxides-469-6403/ |title=Basic and Amphoteric Hydroxides |last=Boundless |date=2016-07-26 |work=Boundless Chemistry |access-date=2017-07-02 |archive-url=https://web.archive.org/web/20170822135614/https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/acids-and-bases-15/acid-base-properties-of-oxides-114/basic-and-amphoteric-hydroxides-469-6403/ |archive-date=22 August 2017 |url-status=dead }}</ref>
:{{chem2|3 HCl + Al(OH)3 → AlCl3 + 3 H2O}}

In bases, it acts as a [[Chemistry:Lewis acids and bases|Lewis acid]] by binding hydroxide ions:<ref name=":0" />
:{{chem2|Al(OH)3 + OH− → [Al(OH)4]−}}

==Production==
[[File:Bützflethermoor Rotschlammdeponie Luftaufnahmen 2012-05-by-RaBoe-478-1.jpg|thumb|left|upright=1.25|[[Earth:Red mud|Red mud]] reservoirs (this one in Stade, Germany) contain the corrosive residues from the production of aluminium hydroxide.]]
Virtually all the aluminium hydroxide used commercially is manufactured by the [[Chemistry:Bayer process|Bayer process]]<ref>{{cite journal|last=Hind|first=AR|author2=Bhargava SK|author3=Grocott SC|title=The Surface Chemistry of Bayer Process Solids: A Review|journal=Colloids Surf Physiochem Eng Aspects|year=1999|volume=146|issue=1–3|pages=359–74|doi=10.1016/S0927-7757(98)00798-5}}</ref> which involves dissolving [[Earth:Bauxite|bauxite]] in sodium hydroxide at temperatures up to {{convert|270|C}}. The waste solid, [[Earth:Bauxite tailings|bauxite tailings]], is removed and aluminium hydroxide is precipitated from the remaining solution of [[Chemistry:Sodium aluminate|sodium aluminate]]. This aluminium hydroxide can be converted to [[Chemistry:Aluminium oxide|aluminium oxide]] or alumina by [[Chemistry:Calcination|calcination]].

The residue or [[Earth:Bauxite tailings|bauxite tailings]], which is mostly iron oxide, is highly caustic due to residual sodium hydroxide. It was historically stored in lagoons; this led to the Ajka alumina plant accident in 2010 in Hungary, where a dam bursting led to the drowning of nine people. An additional 122 sought treatment for chemical burns. The mud contaminated {{convert|40|km2}} of land and reached the [[Place:Danube|Danube]]. While the mud was considered non-toxic due to low levels of heavy metals, the associated slurry had a pH of 13.<ref>{{cite news|title=Hungary Battles to Stem Torrent of Toxic Sludge|url=https://www.bbc.co.uk/news/world-europe-11475361|newspaper=BBC News Website | date=5 October 2010}}</ref>

==Uses==
===Filler and fire retardant ===
Aluminium hydroxide finds use as a fire retardant filler for polymer applications. It is selected for these applications because it is colorless (like most polymers), inexpensive, and has good fire retardant properties.<ref name=Ullmann>{{Ullmann |doi=10.1002/14356007.a01_557|title=Aluminum Oxide|year=2000|last1=Hudson|first1=L. Keith|last2=Misra|first2=Chanakya|last3=Perrotta|first3=Anthony J.|last4=Wefers|first4=Karl|last5=Williams|first5=F. S.|isbn=3527306730}}</ref> [[Chemistry:Magnesium hydroxide|Magnesium hydroxide]] and mixtures of [[Chemistry:Huntite|huntite]] and [[Chemistry:Hydromagnesite|hydromagnesite]] are used similarly.<ref>{{cite journal | last = Hollingbery | first = LA |author2=Hull TR | url = http://clok.uclan.ac.uk/1432/1/2._The_fire_retardant_behaviour_of_huntite_and_hydromagnesite_-_A_review.pdf | title = The Fire Retardant Behaviour of Huntite and Hydromagnesite - A Review | journal = Polymer Degradation and Stability | volume = 95 | issue = 12 | year = 2010 | pages = 2213–2225 | doi=10.1016/j.polymdegradstab.2010.08.019}}</ref><ref>{{cite journal | last = Hollingbery | first = LA |author2=Hull TR | url = http://clok.uclan.ac.uk/1139/1/1._The_thermal_decomposition_of_huntite_and_hydromagnesite_-_A_review.pdf | title = The Thermal Decomposition of Huntite and Hydromagnesite - A Review | journal = Thermochimica Acta | volume = 509 | issue = 1–2 | year = 2010 | pages = 1–11 | doi=10.1016/j.tca.2010.06.012}}</ref><ref>{{cite journal | last = Hollingbery | first = LA |author2=Hull TR | url = http://clok.uclan.ac.uk/3420/1/Fire%20retardant%20effect%20of%20huntite%20and%20hydromagnesite.pdf | title = The Fire Retardant Effects of Huntite in Natural Mixtures with Hydromagnesite | journal = Polymer Degradation and Stability | volume = 97 | issue = 4 | year = 2012 | pages = 504–512 | doi=10.1016/j.polymdegradstab.2012.01.024}}</ref><ref>{{cite journal | last = Hollingbery | first = LA |author2=Hull TR | url = http://clok.uclan.ac.uk/3414/1/The%20Thermal%20Decomposition%20of%20Natural%20Turkish%20Huntite%20and%20Hydromagnesite.pdf | title = The Thermal Decomposition of Natural Mixtures of Huntite and Hydromagnesite | journal = Thermochimica Acta | volume = 528 | year = 2012 | pages = 45–52 | doi=10.1016/j.tca.2011.11.002}}</ref><ref>{{cite journal | last = Hull | first = TR |author2=Witkowski A |author3=Hollingbery LA | url = http://clok.uclan.ac.uk/2963/1/Hull_MineralFillersPDSAcceptedManuscript.pdf | title = Fire Retardant Action of Mineral Fillers | journal = Polymer Degradation and Stability | volume = 96 | issue = 8 | year = 2011 | pages = 1462–1469 | doi=10.1016/j.polymdegradstab.2011.05.006| s2cid = 96208830 }}</ref> It decomposes at about {{convert|180|C}}, absorbing a considerable amount of heat in the process and giving off water vapour. 

In addition to behaving as a fire retardant, it is very effective as a smoke suppressant in a wide range of polymers, most especially in [[Chemistry:Polyester|polyester]]s, [[Chemistry:Poly(methyl methacrylate)|acrylics]], [[Chemistry:Ethylene-vinyl acetate|ethylene vinyl acetate]], [[Chemistry:Epoxy|epoxies]], [[Chemistry:Polyvinyl chloride|polyvinyl chloride]] (PVC) and [[Chemistry:Natural rubber|rubber]].<ref>{{Cite web|url=https://www.hubermaterials.com/userfiles/files/PFDocs/Huber%20Non-Halogen%20Fire%20Retardant%20Additives.pdf|title=Huber Non-Halogen Fire Retardant Additives|author=Huber Engineered Materials|access-date=2017-07-03}}</ref>

Aluminium hydroxide is used as filler in some [[Engineering:Artificial stone|artificial stone]] compound material, often in [[Chemistry:Acrylic resin|acrylic resin]].<!-- see e.g. https://www.kerrock.eu -->

===Precursor to Al compounds===
Aluminium hydroxide is a feedstock for the manufacture of other aluminium compounds: calcined aluminas, [[Chemistry:Aluminium sulfate|aluminium sulfate]], polyaluminium chloride, [[Chemistry:Aluminium chloride|aluminium chloride]], [[Chemistry:Zeolite|zeolite]]s, [[Chemistry:Sodium aluminate|sodium aluminate]], activated alumina, and [[Chemistry:Aluminium nitrate|aluminium nitrate]].<ref name="properties" />

Freshly precipitated aluminium hydroxide forms [[Physics:Gel|gel]]s, which are the basis for the application of aluminium salts as [[Chemistry:Flocculation|flocculants]] in water purification. This gel crystallizes with time. Aluminium hydroxide gels can be dehydrated (e.g. using water-miscible non-aqueous solvents like [[Chemistry:Ethanol|ethanol]]) to form an amorphous aluminium hydroxide powder, which is readily soluble in acids. Heating converts it to activated aluminas, which are used as [[Chemistry:Desiccant|desiccant]]s, adsorbent in gas purification, and [[Chemistry:Catalyst support|catalyst support]]s.<ref name=Ullmann/>

===Pharmaceutical===
Under the generic name "algeldrate", aluminium hydroxide is used as an [[Chemistry:Antacid|antacid]] in humans and animals (mainly cats and dogs). It is preferred over other alternatives such as [[Chemistry:Sodium bicarbonate|sodium bicarbonate]] because {{chem2|Al(OH)3}}, being insoluble, does not increase the pH of stomach above 7 and hence, does not trigger secretion of excess acid by the stomach. Brand names include Alu-Cap, Aludrox, Gaviscon or Pepsamar. It reacts with excess acid in the stomach, reducing the acidity of the stomach content,<ref>{{cite book |author1=Galbraith, A |author2=Bullock, S |author3=Manias, E |author4=Hunt, B |author5=Richards, A | year = 1999 | title = Fundamentals of pharmacology: a text for nurses and health professionals | location = Harlow | publisher = Pearson | pages = 482}}</ref><ref name=papich>{{Cite book | last=Papich | first=Mark G. | title=Saunders Handbook of Veterinary Drugs | chapter=Aluminum Hydroxide and Aluminum Carbonate | location=St. Louis, Mo | date=2007 | edition=2nd | publisher=Saunders/Elsevier | isbn=9781416028888 | pages=15–16}}</ref> which may relieve the symptoms of ulcers, heartburn or dyspepsia. Such products can cause [[Medicine:Constipation|constipation]], because the aluminium ions inhibit the contractions of [[Biology:Smooth muscle|smooth muscle]] cells in the gastrointestinal tract, slowing [[Biology:Peristalsis|peristalsis]] and lengthening the time needed for stool to pass through the [[Biology:Large intestine|colon]].<ref name="Washington1991">{{cite book|last1=Washington|first1=Neena|title=Antacids and Anti Reflux Agents|date=2 August 1991|publisher=CRC Press|location=Boca Raton, FL|isbn=978-0-8493-5444-1|page=10}}</ref> Some such products are formulated to minimize such effects through the inclusion of equal concentrations of [[Chemistry:Magnesium hydroxide|magnesium hydroxide]] or [[Chemistry:Magnesium carbonate|magnesium carbonate]], which have counterbalancing [[Chemistry:Laxative|laxative]] effects.<ref>{{Cite book | last=Bill | first=Robert L. | title=Clinical Pharmacology and Therapeutics for Veterinary Technicians - E-Book | date=2016-09-01 | publisher=Elsevier Health Sciences | isbn=9780323444026 | page=105 | url=https://books.google.com/books?id=0Hf2DAAAQBAJ&pg=PA105}}</ref>

This compound is also used to control [[Medicine:Hyperphosphatemia|hyperphosphatemia]] (elevated [[Chemistry:Phosphate|phosphate]], or phosphorus, levels in the blood) in people and animals suffering from kidney failure. Normally, the kidneys filter excess phosphate out from the blood, but kidney failure can cause phosphate to accumulate. The aluminium salt, when ingested, binds to phosphate in the [[Chemistry:Intestine|intestine]]s and reduce the amount of phosphorus that can be absorbed.<ref name=plumb>{{Cite book | last=Plumb | first=Donald C. | title=Plumb's Veterinary Drug Handbook | chapter=Aluminum Hydroxide | location=Stockholm, Wisconsin; Ames, Iowa | date=2011 | edition=7th | publisher=Wiley | isbn=9780470959640 | pages=36–37}}</ref><ref>{{Cite web | author=Lifelearn Inc. | title=Aluminum Hydroxide | work=Know Your Pet | access-date=2017-06-30 | date=2010-11-01 | url=https://vcahospitals.com/know-your-pet/aluminum-hydroxide}}</ref>

[[Chemistry:Precipitation|Precipitated]] aluminium hydroxide is included as an adjuvant in some [[Biology:Vaccine|vaccine]]s (e.g. [[Social:Anthrax vaccine|anthrax vaccine]]). One of the well-known brands of aluminium hydroxide adjuvant is Alhydrogel, made by Brenntag Biosector.<ref>{{cite web|url=http://www.brenntag.com/biosector/en/biosector/about-brenntag-biosector/index.jsp|title=About Brenntag Biosector - Brenntag|website=brenntag.com|access-date=19 April 2018}}</ref>{{full citation needed|date=June 2017}}{{Dead link|date=January 2021}} Since it absorbs protein well, it also functions to stabilize vaccines by preventing the proteins in the vaccine from precipitating or sticking to the walls of the container during storage. Aluminium hydroxide is sometimes called "[[Chemistry:Alum|alum]]", a term generally reserved for one of several sulfates.{{citation needed|date=October 2018}}

Vaccine formulations containing aluminium hydroxide stimulate the [[Biology:Immune system|immune system]] by inducing the release of [[Chemistry:Uric acid|uric acid]], an immunological danger signal. This strongly attracts certain types of monocytes which differentiate into dendritic cells. The dendritic cells pick up the antigen, carry it to lymph nodes, and stimulate T cells and B cells.<ref>{{Cite journal | last = Kool | first = M |author2=Soullié T |author3=van Nimwegen M |author4=Willart MA |author5=Muskens F |author6=Jung S |author7=Hoogsteden HC |author8=Hammad H |author9=Lambrecht BN | title = Alum adjuvant boosts adaptive immunity by inducing uric acid and activating inflammatory dendritic cells| journal = J Exp Med | volume = 205 | issue = 4 | pages = 869–82 | date = 2008-03-24 | doi = 10.1084/jem.20071087| pmc=2807488 | pmid=18362170}}</ref> It appears to contribute to induction of a good [[Biology:T helper cell#Th1/Th2 model|Th2]] response, so is useful for immunizing against pathogens that are blocked by antibodies. However, it has little capacity to stimulate cellular (Th1) immune responses, important for protection against many pathogens,<ref>{{cite journal |vauthors=Petrovsky N, Aguilar JC | title = Vaccine adjuvants: current state and future trends | journal = Immunology & Cell Biology | year = 2004 | volume = 82 | issue = 5 | pages = 488–96 | doi = 10.1111/j.0818-9641.2004.01272.x | pmid = 15479434| s2cid = 154670 }}</ref> nor is it useful when the antigen is [[Chemistry:Peptide|peptide]]-based.<ref name = Cranage>{{cite book |title = Vaccine Protocols - Volume 87 of Methods in Molecular Medicine Biomed Protocols | last = Cranage | first = MP | editor = Robinson A |editor2=Hudson MJ |editor3=Cranage MP |author2=Robinson A | edition = 2nd | publisher = [[Company:Springer Science+Business Media|Springer]] | year = 2003 | isbn = 978-1-59259-399-6 | url = https://books.google.com/books?id=kCk9BUyEaLkC&pg=PA176|page= 176 }}</ref>

==Safety==
In the 1960s and 1970s it was speculated that aluminium was related to various [[Medicine:Neurological disorder|neurological disorder]]s, including [[Medicine:Alzheimer's disease|Alzheimer's disease]].<ref name=ALZ>{{cite web | url = http://www.alz.org/alzheimers_disease_myths_about_alzheimers.asp | title = Alzheimer's Myth's | access-date = 2012-07-29 | publisher = Alzheimer's Association }}</ref><ref name=AS>{{cite web | url = http://alzheimers.org.uk/site/scripts/documents_info.php?documentID=99 | title = Aluminium and Alzheimer's disease | access-date = 2012-03-08 | date = 2008-09-01 | publisher = Alzheimer's Society | last = Khan | first = A | archive-url = https://web.archive.org/web/20120311205419/http://alzheimers.org.uk/site/scripts/documents_info.php?documentID=99 | archive-date = 11 March 2012 | url-status = dead}}</ref> Since then, multiple [[Social:Epidemiology|epidemiological]] studies have found no connection between exposure to environmental or swallowed aluminium and neurological disorders, though injected aluminium was not looked at in these studies.<ref>{{cite journal | 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 | doi=10.1515/REVEH.2002.17.2.107 | pmc=4764671 }}</ref><ref>{{cite journal |vauthors=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 | date=May 1997 | pmid=9115023 | doi=10.1097/00001648-199705000-00009|jstor= 3702254| s2cid=32190038 | doi-access=free }}</ref><ref>{{cite journal |vauthors=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 | date=September 1998 | pmid=9861186 | pmc=1757634 | doi=10.1136/oem.55.9.627 }}</ref>

Neural disorders were found in experiments on mice motivated by Gulf War illness (GWI). Aluminium hydroxide injected in doses equivalent to those administered to the United States military, showed increased reactive astrocytes, increased [[Biology:Apoptosis|apoptosis]] of motor neurons and [[Biology:Microglia|microglia]]l proliferation within the spinal cord and cortex.<ref>{{Cite journal|last1=Shaw|first1=Christopher A.|last2=Petrik|first2=Michael S.|date=November 2009|title=Aluminum hydroxide injections lead to motor deficits and motor neuron degeneration|journal=Journal of Inorganic Biochemistry|volume=103|issue=11|pages=1555–1562|doi=10.1016/j.jinorgbio.2009.05.019|issn=1873-3344|pmc=2819810|pmid=19740540}}</ref>

==References==
{{Reflist|30em}}

==External links==
* [http://www.inchem.org/documents/icsc/icsc/eics0373.htm International Chemical Safety Card 0373]
* [http://pubs.aic.ca/doi/pdf/10.4141/cjss65-045 "Some properties of aluminum hydroxide precipitated in the presence of clays", Soil Research Institute, R C Turner, Department of Agriculture, Ottawa]{{Dead link|date=October 2022 |bot=InternetArchiveBot |fix-attempted=yes }}
* [http://www.nrcresearchpress.com/doi/abs/10.1139/v76-220 Effect of ageing on properties of polynuclear hydroxyaluminium cations]
* [http://www.nrcresearchpress.com/doi/abs/10.1139/v76-273 A second species of polynuclear hydroxyaluminium cation, its formation and some of its properties]

{{Hydroxides}}
{{Aluminium compounds}}
{{Antacids}}
{{Molecules detected in outer space}}

{{DEFAULTSORT:Aluminium Hydroxide}}
[[Category:Aluminium compounds]]
[[Category:Amphoteric compounds]]
[[Category:Antacids]]
[[Category:Hydroxides]]
[[Category:Inorganic compounds]]

{{Sourceattribution|Aluminium hydroxide}}