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Revision as of 12:16, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 476560361 of page Ammonium_sulfate for the Chem/Drugbox validation project (updated: '').		Latest revision as of 21:19, 28 September 2024 edit Smokefoot (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers, Rollbackers74,550 edits →Reactions: Triammonium hydrogen disulphate,
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			{{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
			| Watchedfields = changed
	| verifiedrevid = 444492723
			| verifiedrevid = 476992905
	| ImageFile = Ammonium sulfate.png		| ImageFile = Ammonium sulfate.png
	| ImageSize = 180px		| ImageSize = 180px
			| ImageName = Ammonium sulfate Lewis structure
	| ImageFile1 = Ammonium-sulfate-3D-balls.png		| ImageFile1 = Ammonium-sulfate-3D-balls.png
	| ImageSize1 = 220px		| ImageSize1 = 220px
	| ImageName1 = Ball-and-stick model of two ammonium cations and one sulfate anion		| ImageName1 = Ball-and-stick model of two ammonium cations and one sulfate anion
	| IUPACName = Diazanium sulfate		| IUPACName = Ammonium sulfate
	| OtherNames = ammonium sulfate<br/>ammonium sulfate (2:1)<br/>diammonium sulfate<br/>sulfuric acid diammonium salt<br/>]<br/>Actamaster<br/>Dolamin		| OtherNames = {{Unbulleted list|Ammonium sulphate|Ammonium sulfate (2:1)|Diammonium sulfate|Sulfuric acid diammonium salt|]|Actamaster|Dolamin}}
			| SystematicName =
	| Section1 = {{Chembox Identifiers		| Section1 = {{Chembox Identifiers
	| UNII_Ref = {{fdacite|correct|FDA}}		| UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = SU46BAM238		| UNII = SU46BAM238
			| ChEBI = 62946
	| KEGG_Ref = {{keggcite|correct|kegg}}		| KEGG_Ref = {{keggcite|correct|kegg}}
	| KEGG = D08853		| KEGG = D08853
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	| StdInChIKey = BFNBIHQBYMNNAN-UHFFFAOYSA-N		| StdInChIKey = BFNBIHQBYMNNAN-UHFFFAOYSA-N
	| CASNo = 7783-20-2		| CASNo = 7783-20-2
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=22944		| ChemSpiderID=22944
	| PubChem =		| PubChem = 6097028
			| EC_number = 231-984-1
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = (NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>		| Formula = (NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>
	| MolarMass = 132.14 g/mol		| MolarMass = 132.14 g/mol
	| Appearance = Fine white ] granules or crystals.		| Appearance = Fine white ] granules or crystals
	| Density = 1.769 g/cm<sup>3</sup> (20 °C)		| Density = 1.77 g/cm<sup>3</sup>
	| MeltingPtCL = 235		| MeltingPtC = 235 to 280
			| MeltingPt_notes = (decomposes)
	| MeltingPtCH = 280
			| CriticalRelativeHumidity = 79.2% (30&nbsp;°C)
	| Melting_notes = decomposes
			| Solubility = 70.6&nbsp;g per 100&nbsp;g water (0&nbsp;°C)<br>74.4&nbsp;g per 100&nbsp;g water (20&nbsp;°C) <br>103.8&nbsp;g per 100&nbsp;g water (100&nbsp;°C)<ref>{{RubberBible87th}}</ref>
	| CriticalRelativeHumidity = 79.2% (30 °C)
			| SolubleOther = Insoluble in ], ] and ]
	| Solubility = 70.6 g/100 mL (0 °C)<br/> <br> 74.4 g/100 mL (20 °C) <br> 103.8 g/100 mL (100 °C)<ref>Handbook of Chemistry and Physics</ref>
			| MagSus = {{val|-67.0e-6|u=cm<sup>3</sup>/mol}}
	| SolubleOther = insoluble in ], ] and ]
	}}		}}
			|Section3={{Chembox Structure
			| Coordination =
			| CrystalStruct = orthorhombic
			}}
			| Section4 =
			| Section5 =
			| Section6 =
	| Section7 = {{Chembox Hazards		| Section7 = {{Chembox Hazards
	| ExternalMSDS =		| ExternalSDS =
			| MainHazards =
	| EUIndex = Not listed
			| FlashPt = Non-flammable
	| MainHazards =
			| NFPA-H = 2
	| FlashPt = Non-flammable
	| NFPA-H = 2		| NFPA-F = 1
	| NFPA-F = 1		| NFPA-R = 0
			| LD50 = 2840 mg/kg, rat (oral)
	| NFPA-R = 0
			| GHSPictograms = {{GHS07}}{{GHS09}}
	| LD50 = 2840 mg/kg, rat (oral)
			| GHSSignalWord = Warning
			| HPhrases = {{H-phrases|315|319|335}}
			| PPhrases = {{P-phrases|261|264|270|271|273|280|301+312|302+352|304+340|305+351+338|312|321|330|332+313|337+313|362|391|403+233|405|501}}
	}}		}}
	| Section8 = {{Chembox Related		| Section8 = {{Chembox Related
	| OtherAnions = ]<br/>]<br/>]<br/>]		| OtherAnions = ]<br/>]<br/>]<br/>]
	| OtherCations = ]<br/>]		| OtherCations = ]<br/>]
	| OtherCpds = ]		| OtherCompounds = ]
	}}		}}
	}}		}}
			'''Ammonium sulfate''' (American English and international scientific usage; '''ammonium sulphate''' in ]); (NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>, is an inorganic ] with a number of commercial uses. The most common use is as a soil fertilizer. It contains 21% ] and 24% ].
			== Uses ==
			===Agriculture===
			The primary use of ammonium sulfate is as a ] for ]s. In the soil, the ] ion is released and forms a small amount of acid, lowering the ] balance of the ], while contributing essential ] for plant growth. One disadvantage to the use of ammonium sulfate is its low nitrogen content relative to ], which elevates transportation costs.<ref name=Ullmann>{{cite encyclopedia|first=Karl-Heinz |last=Zapp |title=Ammonium Compounds |encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry |year=2012 |publisher=Wiley-VCH |location=Weinheim |doi=10.1002/14356007.a02_243|isbn=9783527303854 }}</ref>
			It is also used as an agricultural spray ] for water-soluble ]s, ]s, and ]s. There, it functions to bind iron and calcium cations that are present in both well water and plant cells. It is particularly effective as an adjuvant for ] (amine), ], and ] herbicides.
			=== Laboratory use ===
			] is a common method for ] by precipitation. As the ] of a solution increases, the solubility of proteins in that solution decreases. Being extremely soluble in water, ammonium sulfate can "salt out" (precipitate) proteins from aqueous solutions.<ref>{{cite book|title=Methods in Enzymology|last1=Duong-Ly|first1=Krisna C.|last2=Gabelli|first2=Sandra B.|date=2014-01-01|publisher=Academic Press|editor-last=Lorsch|editor-first=Jon|series=Laboratory Methods in Enzymology: Protein Part C|volume=541|pages=85–94|doi=10.1016/B978-0-12-420119-4.00007-0|pmid=24674064|chapter=Salting out of Proteins Using Ammonium Sulfate Precipitation|isbn=9780124201194}}</ref><ref>{{cite book|last1=Duong-Ly|first1=Krisna C.|last2=Gabelli|first2=Sandra B.|chapter=Salting out of Proteins Using Ammonium Sulfate Precipitation |date=2014-01-01|title=Laboratory Methods in Enzymology: Protein Part C|volume=541|pages=85–94|doi=10.1016/B978-0-12-420119-4.00007-0|issn=1557-7988|pmid=24674064|isbn=9780124201194}}</ref> Precipitation by ammonium sulfate is a result of a reduction in solubility rather than ], thus the precipitated protein can be resolubilized through the use of standard ].<ref>{{cite journal|last=Wingfield|first=Paul T.|date=2017-05-05|title=Protein Precipitation Using Ammonium Sulfate|journal=Current Protocols in Protein Science |volume=13 |issue=1 |pages=A.3F.1–8|doi=10.1002/0471140864.psa03fs13|issn=1934-3655|pmc=4817497|pmid=18429073|isbn=978-0471140863}}</ref> Ammonium sulfate precipitation provides a convenient and simple means to fractionate complex protein mixtures.<ref>{{cite web |url=http://www.encorbio.com/protocols/AM-SO4.htm |title=Ammonium Sulfate Calculator |publisher=EnCor Biotechnology Inc. |year=2013 |access-date=March 2, 2013 |archive-date=January 26, 2016 |archive-url=https://web.archive.org/web/20160126164138/http://www.encorbio.com/protocols/AM-SO4.htm |url-status=live }}</ref>
			In the analysis of rubber lattices, volatile fatty acids are analyzed by precipitating rubber with a 35% ammonium sulfate solution, which leaves a clear liquid from which volatile fatty acids are regenerated with sulfuric acid and then distilled with steam. Selective precipitation with ammonium sulfate, opposite to the usual precipitation technique which uses acetic acid, does not interfere with the determination of volatile fatty acids.<ref>ASTM Standard Specification for Rubber Concentrates D 1076-06</ref>
			=== Food additive ===
			As a food additive, ammonium sulfate is considered ] (GRAS) by the U.S. ],<ref>{{cite web |url=https://www.fda.gov/Food/FoodIngredientsPackaging/GenerallyRecognizedasSafeGRAS/GRASSubstancesSCOGSDatabase/ucm260866.htm |title=Select Committee on GRAS Substances (SCOGS) Opinion: Ammonium sulfate |publisher=U.S. ] |date=August 16, 2011 |access-date=March 2, 2013 |archive-date=February 11, 2012 |archive-url=https://web.archive.org/web/20120211002116/http://www.fda.gov/Food/FoodIngredientsPackaging/GenerallyRecognizedasSafeGRAS/GRASSubstancesSCOGSDatabase/ucm260866.htm |url-status=live }}</ref> and in the European Union it is designated by the ] E517. It is used as an ] in flours and breads.<ref>{{cite web |url=http://www.panerabread.com/menu/nutrition/profile.php?id=17 |title=Panera Bread: Menu & Nutrition: Nutrition Information Profile |archive-url=https://web.archive.org/web/20090819050107/http://www.panerabread.com/menu/nutrition/profile.php?id=17 |archive-date=August 19, 2009 |access-date=March 2, 2013}}<!-- Page lists ammonium sulfate as an ingredient but does not say that it is an acidity regulator. Better reference required.--></ref><ref>{{cite web |url=http://www.subway.com/subwayroot/menunutrition/Nutrition/frmUsIngredients.aspx |title=Official Subway Restaurants U.S. Products Ingredients Guide |archive-url=https://web.archive.org/web/20110814145734/http://www.subway.com/subwayroot/menunutrition/Nutrition/frmUsIngredients.aspx |archive-date=August 14, 2011 |access-date=March 2, 2013}}</ref><ref>{{cite news |author=Sarah Klein |url=http://www.huffingtonpost.com/2012/05/11/gross-ingredients-processed-foods_n_1510516.html?ref=mostpopular#s=967544 |title=Gross Ingredients In Processed Foods |work=] |date=May 14, 2012 |access-date=March 2, 2013 |archive-date=May 18, 2012 |archive-url=https://web.archive.org/web/20120518070402/http://www.huffingtonpost.com/2012/05/11/gross-ingredients-processed-foods_n_1510516.html?ref=mostpopular#s=967544 |url-status=live }}</ref>
			=== Other uses ===
			Ammonium sulfate is a precursor to other ammonium salts, especially ].
			Ammonium sulfate is listed as an ingredient for many United States vaccines per the ].<ref>{{cite web |url=https://www.cdc.gov/vaccines/pubs/pinkbook/downloads/appendices/B/excipient-table-2.pdf |title=Vaccine Excipient & Media Summary |publisher=] (CDC) |date=February 2012 |access-date=March 2, 2013 |archive-date=February 5, 2011 |archive-url=https://web.archive.org/web/20110205155918/http://www.cdc.gov/vaccines/pubs/pinkbook/downloads/appendices/b/excipient-table-2.pdf |url-status=live }}</ref>
			Ammonium sulfate has also been used in ] compositions acting much like ]. As a flame retardant, it increases the combustion temperature of the material, decreases maximum weight loss rates, and causes an increase in the production of residue or char.<ref>{{cite journal|last1=George |first1=C. W. |last2=Susott |first2=R. A. |title=Effects of Ammonium Phosphate and Sulfate on the Pyrolysis and Combustion of Cellulose |publisher=USDA Forest Service |journal=Research Paper INT-90 |place=Intermountain Forest and Range Experiment Station |date=April 1971 |ol=16022833M |url=https://openlibrary.org/b/OL16022833M/Effects_of_ammonium_phosphate_and_sulfate_on_the_pyrolysis_and_combustion_of_cellulose}}</ref>
			== Preparation ==
			Ammonium sulfate is made by treating ] with ]:
			:{{chem2 | 2 NH3 + H2SO4 -> (NH4)2SO4 }}
			A mixture of ammonia gas and water vapor is introduced into a reactor that contains a saturated solution of ammonium sulfate and about 2% to 4% of free sulfuric acid at 60&nbsp;°C. Concentrated sulfuric acid is added to keep the solution acidic, and to retain its level of free acid. The heat of reaction keeps reactor temperature at 60&nbsp;°C. Dry, powdered ammonium sulfate may be formed by spraying sulfuric acid into a reaction chamber filled with ammonia gas. The heat of reaction evaporates all ] present in the system, forming a powdery salt. Approximately 6,000 million tons were produced in 1981.<ref name=Ullmann/>
			Ammonium sulfate also is manufactured from ] (CaSO<sub>4</sub>·2H<sub>2</sub>O). Finely divided gypsum is added to an ] solution. ] precipitates as a solid, leaving ammonium sulfate in the solution.
			:{{chem2 | (NH4)2CO3 + CaSO4 -> (NH4)2SO4 + CaCO3 }}
			Ammonium sulfate occurs naturally as the rare mineral ] in volcanic ]s and due to coal fires on some dumps.<ref>{{cite web |url=http://www.mindat.org/min-2584.html/ |title=Mascagnite |publisher=Mindat |access-date=March 2, 2013 |archive-date=January 19, 2013 |archive-url=https://web.archive.org/web/20130119033628/http://www.mindat.org/min-2584.html |url-status=live }}</ref>
			Ammonium sulfate is a byproduct in the production of ].<ref name=Ull>{{Ullmann|first1=William|last1=Bauer, Jr.|title=Methacrylic Acid and Derivatives|year=2002|doi=10.1002/14356007.a16_441}}.</ref>
			== Properties ==
			Ammonium sulfate becomes ] at temperatures below –49.5&nbsp;°C. At room temperature it crystallises in the ] system, with cell sizes of ''a'' = 7.729&nbsp;Å, ''b'' = 10.560&nbsp;Å, ''c'' = 5.951&nbsp;Å. When chilled into the ferrorelectric state, the symmetry of the crystal changes to ] Pna2<sub>1</sub>.<ref name="Okaya1958">{{cite journal|last=Okaya|first=Y.|author2=K. Vedam |author3=R. Pepinsky |year=1958|title=Non-isomorphism of ferroelectric phases of ammonium sulfate and ammonium fluoberyllate|journal=Acta Crystallographica|volume=11|issue=4|pages=307|issn=0365-110X|doi=10.1107/s0365110x58000803|doi-access=free|bibcode=1958AcCry..11..307O }}</ref>
			== Reactions ==
			Ammonium sulfate decomposes upon heating above {{convert|250|°C}}, first forming ]. Heating at higher temperatures results in decomposition into ], ], ], and water.<ref>{{cite journal | author = Liu Ke-wei, Chen Tian-lang | title = Studies on the thermal decomposition of ammonium sulfate |language=zh | journal = Chemical Research and Application | volume = 14 | issue = 6 | year = 2002 | doi=10.3969/j.issn.1004-1656.2002.06.038}}</ref>
			As a salt of a strong acid (H<sub>2</sub>SO<sub>4</sub>) and weak base (NH<sub>3</sub>), its solution is acidic; the pH of 0.1&nbsp;M solution is 5.5. In aqueous solution the reactions are those of {{chem|NH|4|+}} and {{chem|SO|4|2-}} ions. For example, addition of ], precipitates out ]. The filtrate on evaporation yields ].
			Ammonium sulfate forms many ]s (ammonium metal sulfates) when its solution is mixed with equimolar solutions of metal sulfates and the solution is slowly evaporated. With trivalent metal ions, ]s such as ] are formed. Double metal sulfates include ammonium cobaltous sulfate, ], ammonium nickel sulfate which are known as ] and ].<ref name=Ullmann/> Anhydrous double sulfates of ammonium also occur in the ] family. The ammonia produced has a pungent smell and is toxic.
			Airborne particles of evaporated ammonium sulfate comprise approximately 30% of fine ] worldwide.<ref>{{cite web|url=https://www.purakamasks.com/sources-of-particulates|title=Where Does Air Pollution Come From?|date=2019-02-15|website=www.purakamasks.com|language=en|access-date=2019-02-20|archive-date=2019-02-20|archive-url=https://web.archive.org/web/20190220122732/https://www.purakamasks.com/sources-of-particulates|url-status=live}}</ref>
			It reacts with additional sulfuric acid to give triammonium hydrogen disulphate,, {{chem2|(NH4)3H(SO4)2}}.<ref>{{cite journal |doi=10.1107/S0567740878003969 |title=The crystal structure of Triammonium hydrogen Disulphate, (NH<sub>4</sub>)<sub>3</sub>H(SO<sub>4</sub>)<sub>2</sub> |date=1978 |last1=Suzuki |first1=S. |last2=Makita |first2=Y. |journal=Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry |volume=34 |issue=3 |pages=732–735 |bibcode=1978AcCrB..34..732S }}</ref>
			== Legislation and control ==
			In November 2009, a ban on ammonium sulfate, ] and ] fertilizers was imposed in the former ]—comprising the ], ], ], ] and ] districts of the ] (NWFP) of ], by the NWFP government, following reports that they were used by militants to make explosives. In January 2010, these substances were also banned in ] for the same reason.<ref>{{cite web |url=http://www.irinnews.org/Report/87937/PAKISTAN-Anti-terrorist-fertilizer-ban-hinders-farmers |title=PAKISTAN: 'Anti-terrorist' fertilizer ban hinders farmers |publisher=IRIN Humanitarian News and Analysis |year=2010 |access-date=April 24, 2013 |archive-date=May 13, 2013 |archive-url=https://web.archive.org/web/20130513213427/http://www.irinnews.org/Report/87937/PAKISTAN-Anti-terrorist-fertilizer-ban-hinders-farmers |url-status=live }}</ref>
			== See also ==
			*]
			{{Commonscat|Ammonium sulfate}}
			== References ==
			{{reflist}}
			== Further reading ==
			* Properties: UNIDO and ] (1998), ''Fertilizer Manual'', Kluwer Academic Publishers, {{ISBN|0-7923-5032-4}}.
			== External links ==
			* {{PPDB|36}}
			*Calculators: , and of aqueous ammonium sulfate
			{{Ammonium salts}}
			{{Sulfates}}
			{{Authority control}}
			]
			]
			]
			]
			]
			]
			]