| Revision as of 12:15, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 476564397 of page Aluminium_sulfate for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 04:23, 10 December 2024 edit Neko-chan (talk | contribs)Extended confirmed users, New page reviewers, Rollbackers20,609 edits →top: I think that's all the chemsTags: Mobile edit Mobile app edit Android app edit App full source |
| Line 1: |
Line 1: |
|
|
{{short description|Chemical compound}} |
|
{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
|
|
{{chembox |
|
{{chembox |
|
|
| Verifiedfields = changed |
|
| Watchedfields = changed |
|
| Watchedfields = changed |
|
| verifiedrevid = 455182564 |
|
| verifiedrevid = 476992891 |
|
| ImageFile = Aluminium sulfate.jpg |
|
| ImageFile = Aluminium sulfate.jpg |
|
| ImageSize = 200px |
|
| ImageSize = |
|
| ImageName = Aluminium sulfate hexadecahydrate |
|
| ImageName = Aluminium sulphate hexadecahydrate |
|
| IUPACName = Aluminium sulfate |
|
| IUPACName = Aluminium sulfate |
|
| OtherNames = Cake alum<br />Filter alum<br />Papermaker's alum<br />Alunogenite<br/>Sulfuric acid, aluminum salt (3:2) |
|
| OtherNames = {{Unbulleted list|Aluminum sulfate|Aluminium sulphate|Cake alum|Filter alum|Papermaker's alum|Alunogenite|aluminium salt (3:2)}} |
|
| Section1 = {{Chembox Identifiers |
|
|Section1={{Chembox Identifiers |
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|
| ChemSpiderID = 23233 |
|
| ChemSpiderID = 23233 |
|
| UNII_Ref = {{fdacite|correct|FDA}} |
|
| UNII_Ref = {{fdacite|correct|FDA}} |
|
| UNII = I7T908772F |
|
| UNII = I7T908772F |
|
|
| UNII1_Ref = {{fdacite|correct|FDA}} |
|
|
| UNII1 = TCS9L00G8F |
|
|
| UNII1_Comment = (octadecahydrate) |
|
|
|
|
| InChI = 1/2Al.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6 |
|
| InChI = 1/2Al.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6 |
|
| SMILES = ..S(=O)(=O).S()(=O)=O.S()(=O)=O |
|
| SMILES = ..S(=O)(=O).S()(=O)=O.S()(=O)=O |
| Line 21: |
Line 26: |
|
| StdInChIKey = DIZPMCHEQGEION-UHFFFAOYSA-H |
|
| StdInChIKey = DIZPMCHEQGEION-UHFFFAOYSA-H |
|
| CASNo = 10043-01-3 |
|
| CASNo = 10043-01-3 |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
| CASNo_Ref = {{cascite|correct|CAS}} |
|
|
| CASNo2_Ref = {{cascite|correct|CAS}} |
|
| CASOther = <br> 7784-31-8 (octadecahydrate) |
|
|
| PubChem = 24850 |
|
| CASNo2 = 7784-31-8 |
|
|
| CASNo2_Comment = (octadecahydrate) |
|
| EINECS = 233-135-0 |
|
|
| RTECS = BD1700000 |
|
| PubChem = 24850 |
|
|
| EINECS = 233-135-0 |
|
|
| RTECS = BD1700000 |
|
}} |
|
}} |
|
| Section2 = {{Chembox Properties |
|
|Section2={{Chembox Properties |
|
| Formula = Al<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
|
| Formula = Al<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> |
|
| MolarMass = 342.15 g/mol (anhydrous) <br> 666.42 g/mol (octadecahydrate) |
|
| MolarMass = 342.15 g/mol (anhydrous) <br> 666.44 g/mol (octadecahydrate) |
|
| Appearance = white crystalline solid <br> hygroscopic |
|
| Appearance = white crystalline solid <br> hygroscopic |
|
| Density = 2.672 g/cm<sup>3</sup> (anhydrous) <br> 1.62 g/cm<sup>3</sup> (octadecahydrate) |
|
| Density = 2.672 g/cm<sup>3</sup> (anhydrous) <br> 1.62 g/cm<sup>3</sup> (octadecahydrate) |
|
| Solubility = 31.2 g/100 mL (0 °C) <br> 36.4 g/100 mL (20 °C) <br> 89.0 g/100 mL (100 °C) |
|
| Solubility = 31.2 g/100 mL (0 °C) <br> 36.4 g/100 mL (20 °C) <br> 89.0 g/100 mL (100 °C) |
|
| SolubleOther = slightly soluble in ], dilute mineral ]s |
|
| SolubleOther = slightly soluble in ], dilute mineral ]s |
|
|
| MeltingPtC = 770 |
|
| MeltingPt = 770 °C (decomp, anhydrous) <br> 86.5 °C (]) |
|
|
|
| MeltingPt_notes = (decomposes, anhydrous) <br> 86.5 °C (]) |
|
| pKa = 3.3-3.6 |
|
|
|
| pKa = 3.3–3.6 |
|
| RefractIndex = 1.47 <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8</ref> |
|
|
|
| RefractIndex = 1.47<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> |
|
| enthalpy of formation Δ''H''<sup><s>o</s><sub>f</sub></sup><sub>solid</sub> = -3440 kJ/mol |
|
|
|
| MagSus = {{val|-93.0e-6|u=cm<sup>3</sup>/mol}} |
|
}} |
|
}} |
|
| Section3 = {{Chembox Structure |
|
|Section3={{Chembox Structure |
|
| Coordination = |
|
| Coordination = |
|
| CrystalStruct = ] (hydrate) |
|
| CrystalStruct = ] (hydrate) |
|
}} |
|
}} |
|
| Section8 = {{Chembox Related |
|
|Section4={{Chembox Thermochemistry |
|
|
| DeltaHf = -3440 kJ/mol |
|
| OtherCations = ]<br />] |
|
|
|
}} |
|
| OtherCpds = ''See'' ] |
|
|
|
|Section7={{Chembox Hazards |
|
|
| NFPA-H = 1 |
|
|
| NFPA-F = 0 |
|
|
| NFPA-R = 0 |
|
|
| NFPA-S = |
|
|
| IDLH = N.D.<ref name=PGCH>{{PGCH|0024}}</ref> |
|
|
| PEL = none<ref name=PGCH/> |
|
|
| REL = 2 mg/m<sup>3</sup><ref name=PGCH/> |
|
|
}} |
|
|
|Section8={{Chembox Related |
|
|
| OtherCations = ]<br />] |
|
|
| OtherCompounds = ''See'' ] |
|
}} |
|
}} |
|
}} |
|
}} |
|
|
|
|
|
'''Aluminium sulfate''' is a salt with the ] {{chem2|]2]3}}. It is soluble in water and is mainly used as a ] (promoting particle collision by neutralizing charge) in the purification of drinking water<ref>{{cite web | last = Global Health and Education Foundation | title = Conventional Coagulation-Flocculation-Sedimentation | work = Safe Drinking Water is Essential | publisher = National Academy of Sciences | year = 2007 | url = http://drinking-water.org/html/en/Treatment/Coagulation-Flocculation-technologies.html | access-date = 2007-12-01 | url-status = live | archive-url = https://web.archive.org/web/20071007195603/http://www.drinking-water.org/html/en/Treatment/Coagulation-Flocculation-technologies.html | archive-date = 2007-10-07 }}</ref><ref>{{cite journal | author=Kvech S, Edwards M | title=Solubility controls on aluminum in drinking water at relatively low and high pH | journal=Water Research | volume=36 | issue=17 | year=2002 | pages=4356–4368 | pmid=12420940 | doi=10.1016/S0043-1354(02)00137-9 | bibcode=2002WatRe..36.4356K }}</ref> and ]s, and also in paper manufacturing. |
|
|
|
|
|
The anhydrous form occurs naturally as a rare ] ], found for example in volcanic environments and on burning coal-mining waste dumps. Aluminium sulfate is rarely, if ever, encountered as the anhydrous salt. It forms a number of different ]s, of which the hexadecahydrate {{chem2|Al2(SO4)3*16H2O}} and octadecahydrate {{chem2|Al2(SO4)3*18H2O}} are the most common. The heptadecahydrate, whose formula can be written as {{chem2|2(SO4)3*5H2O}}, occurs naturally as the mineral ]. |
|
|
|
|
|
Aluminium sulfate is sometimes called '''alum''' or '''papermaker's alum''' in certain industries. However, the name "]" is more commonly and properly used for any double sulfate salt with the generic formula {{chem2|''X''Al(SO4)2*12H2O}}, where ''X'' is a ] ] such as ] or ].<ref name=shreve84>{{cite book|last=Austin|first=George T.|title=Shreve's Chemical process industries.|year=1984|publisher=McGraw-Hill|location=New York|isbn=9780070571471|pages=357|url=https://books.google.com/books?id=12ahTF69BAEC&q=alums&pg=PA357|edition=5th|url-status=live|archive-url=https://web.archive.org/web/20140103135350/http://books.google.com/books?id=12ahTF69BAEC&pg=PA357&lpg=PA357&dq=alums|archive-date=2014-01-03}}</ref> |
|
|
|
|
|
==Production== |
|
|
|
|
|
===In the laboratory=== |
|
|
Aluminium sulfate may be made by adding ], {{chem2|Al(OH)3}}, to ], {{chem2|H2SO4}}: |
|
|
:{{chem2|2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2O}} |
|
|
or by heating aluminium in a sulfuric acid solution: |
|
|
: {{chem2|2Al + 3H2SO4 → Al2(SO4)3 + 3H2↑}} |
|
|
|
|
|
===From alum schists=== |
|
|
The alum ]s employed in the manufacture of aluminium sulfate are mixtures of ], ] and various ] substances, and are found in upper ], ], ], and ]. These are either roasted or exposed to the ] action of the air. In the roasting process, ] is formed and acts on the clay to form aluminium sulfate, a similar condition of affairs being produced during weathering. The mass is now systematically extracted with water, and a solution of aluminium sulfate of ] 1.16 is prepared. This solution is allowed to stand for some time (in order that any ] and basic ] may separate), and is then evaporated until ] crystallizes on cooling; it is then drawn off and evaporated until it attains a specific gravity of 1.40. It is now allowed to stand for some time, and decanted from any sediment.{{sfn|Chisholm|1911|p=767}} |
|
|
|
|
|
===From clays or bauxite=== |
|
|
In the preparation of aluminium sulfate from ]s or from ], the material is gently ], then mixed with sulfuric acid and water and heated gradually to boiling; if concentrated acid is used no external heat is generally required as the formation of aluminium sulfate is ]. It is allowed to stand for some time, and the clear solution is drawn off. |
|
|
|
|
|
===From cryolite=== |
|
|
When ] is used as the ore, it is mixed with ] and heated. By this means, ] is formed; it is then extracted with water and ] either by ] or by passing a current of ] through the solution. The precipitate is then dissolved in sulfuric acid.{{sfn|Chisholm|1911|p=767}} |
|
|
|
|
|
==Uses== |
|
|
] |
|
|
Aluminium sulfate is sometimes used in the human food industry as a firming agent, where it takes on ] '''E520''', and in animal feed as a ]. In the United States, the ] lists it as "]" with no limit on concentration.<ref>{{citation |
|
|
| title = 21 CFR 182.1125 |
|
|
| url = https://www.accessdata.fda.gov/scripts/cdrh/cfdocs/cfcfr/CFRSearch.cfm?fr=182.1125 |
|
|
| publication-date = 2020-04-01 |
|
|
| access-date = 2021-02-22 |
|
|
}}</ref> Aluminium sulfate may be used as a ], an ], or as a ] for superficial shaving wounds.{{Citation needed|date=May 2023|reason=The previous source cited here was a dead link}} Aluminium sulfate is used as a ] in ] and ]. |
|
|
|
|
|
It is a common ] ] and works "by facilitating the slow release of ] from the vaccine depot formed at the site of ]."{{Citation needed|date=May 2023|reason=The previous source cited here was a dead link}} |
|
|
|
|
|
Aluminium sulfate is used in ] and for ] from ]. It causes suspended impurities to coagulate into larger particles and then settle to the bottom of the container (or be filtered out) more easily. This process is called ] or ]. Research suggests that in Australia, aluminium sulfate used in this way in drinking water treatment is the primary source of ] gas in ] systems.<ref>{{cite journal|title=Reducing sewer corrosion through integrated urban water management|journal=Science|volume=345|issue=6198|pages=812–814|author1=Ilje Pikaar |author2=Keshab R. Sharma |author3=Shihu Hu |author4=Wolfgang Gernjak |author5=Jürg Keller |author6=Zhiguo Yuan|bibcode=2014Sci...345..812P|year=2014|doi=10.1126/science.1251418|pmid=25124439|s2cid=19126381}}</ref> An improper and excess application incident in 1988 ] of ] in ]. |
|
|
|
|
|
Aluminium sulfate has been used as a method of ] remediation for shallow lakes. It works by reducing the ] load in the lakes.<ref name=":110">{{cite journal |last1=Kennedy |first1=Robert H. |last2=Cook |first2=G. Dennis |title=Control of Lake Phosphorus with Aluminum Sulfate: Dose Determination and Application Techniques |date=June 1982 |url=https://doi.org/10.1111/j.1752-1688.1982.tb00005.x |journal=Journal of the American Water Resources Association |volume=18 |issue=3 |pages=389–395 |doi=10.1111/j.1752-1688.1982.tb00005.x |bibcode=1982JAWRA..18..389K |issn=1093-474X}}</ref><ref name=":32">{{cite book |last=Martyn |first=Huser, Brian J. Egemose, Sara Harper, Harvey Hupfer, Michael Jensen, Henning Pilgrim, Keith M. Reitzel, Kasper Rydin, Emil Futter |url=http://worldcat.org/oclc/1233676585 |title=Longevity and effectiveness of aluminum addition to reduce sediment phosphorus release and restore lake water quality |date=2016 |publisher=Uppsala universitet, Limnologi |oclc=1233676585}}</ref> |
|
|
|
|
|
When dissolved in a large amount of neutral or slightly alkaline water, aluminium sulfate produces a gelatinous precipitate of ], Al(OH)<sub>3</sub>. 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 ] of garden soil, as it ] to form the aluminium hydroxide precipitate and a dilute ] solution. An example of what changing the pH level of soil can do to plants is visible when looking at '']''. The gardener can add aluminium sulfate to the soil to reduce the pH which in turn will result in the flowers of the ''Hydrangea'' turning a different color (blue). The aluminium is what makes the flowers blue; at a higher pH, the aluminium is not available to the plant.<ref>{{cite web|url=https://web.extension.illinois.edu/state/newsdetail.cfm?NewsID=29303|title=Blue or Pink - Which Color is Your Hydrangea|author1=Kari Houle|publisher=University of Illinois Extension|date=2013-06-18|access-date=2018-09-03}}</ref> |
|
|
|
|
|
In the construction industry, it is used as waterproofing agent and accelerator in ]. Another use is a foaming agent in ]. |
|
|
|
|
|
It can also be very effective as a ],<ref>{{cite book|url=https://books.google.com/books?id=INcnAQAAMAAJ&q=Aluminum+sulfate+can+also+be+very+effective+as+a+molluscicide|title=Field margins: integrating agriculture and conservation : proceedings of a symposium organised by the British Crop Protection Council in association with the British Ecological Society and the Association of Applied Biologists and held at the University of Warwick, Coventry on 18–20 April 1994|last1=Council|first1=British Crop Protection|last2=Society|first2=British Ecological|last3=Biologists|first3=Association of Applied|date=1994|publisher=British Crop Protection Council|isbn=9780948404757|language=en}}</ref> killing ]s. |
|
|
|
|
|
]s ] and ] can be prepared from aluminium sulfate, the product formed being determined by the amount of ] used:<ref>{{cite book|url = https://books.google.com/books?id=GL98CgAAQBAJ&q=aluminium+acetate+mordant&pg=PT118|title = The Chemical Technology of Textile Fibres – Their Origin, Structure, Preparation, Washing, Bleaching, Dyeing, Printing and Dressing|first = Von|last = Georgievics|publisher = ]|year = 2013|isbn = 9781447486121|url-status = live|archive-url = https://web.archive.org/web/20171205203041/https://books.google.com/books?id=GL98CgAAQBAJ&pg=PT118&dq=aluminium+acetate+mordant&hl=en&sa=X&ved=0ahUKEwjv3IbHzb3QAhVFNY8KHYOKAu0Q6AEIJTAA|archive-date = 2017-12-05}}</ref> |
|
|
|
|
|
:{{chem2|Al2(SO4)3 + 3Pb(CH3CO2)2 → 2Al(CH3CO2)3 + 3PbSO4}} |
|
|
|
|
|
:{{chem2|Al2(SO4)3 + 2Pb(CH3CO2)2 → Al2SO4(CH3CO2)4 + 2PbSO4}} |
|
|
|
|
|
==Chemical reactions== |
|
|
The compound decomposes to ] and ] when heated between 580 and 900 °C. It combines with water forming hydrated salts of various compositions. |
|
|
|
|
|
Aluminium sulfate reacts with ] to which foam stabilizer has been added, producing ] for ]s: |
|
|
|
|
|
: {{chem2|Al2(SO4)3 + 6NaHCO3 → 3Na2SO4 + 2Al(OH)3 + 6CO2}} |
|
|
|
|
|
The ] 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 ], smothering the ]. Chemical foam was unsuitable for use on ]s such as ], 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 ] or fixed installation using hoselines. Chemical foam is considered obsolete in the United States and has been replaced by synthetic mechanical foams, such as ] which have a longer shelf life, are more effective, and more versatile, although some countries such as Japan and India continue to use it.{{citation needed|date=August 2010}} |
|
|
|
|
|
==References== |
|
|
|
|
|
===Footnotes=== |
|
|
{{reflist}} |
|
|
|
|
|
===Notations=== |
|
|
* {{cite EB1911|wstitle=Aluminium |volume=1 |page=767}} |
|
|
* {{cite book | author=Pauling, Linus | title=General Chemistry | location=W.H. Freeman | publisher=San Francisco | year=1970 | isbn=978-0-486-65622-9 | url-access=registration | url=https://archive.org/details/generalchemistry00paul_0 }} |
|
|
|
|
|
==External links== |
|
|
* |
|
|
* |
|
|
* |
|
|
* |
|
|
* |
|
|
|
|
|
{{Aluminium compounds}} |
|
|
{{Sulfates}} |
|
|
|
|
|
{{Authority control}} |
|
|
|
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |
|
|
] |