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{{chembox {{chembox
| Verifiedfields = changed
⚫ | verifiedrevid = 399519350
| Watchedfields = changed
⚫ | ImageFile = Ammonium-persulfate.svg
⚫ | verifiedrevid = 442343854
| ImageName = Structural formulas of two ammonium cations and one peroxydisulfate anion
⚫ | Name =
⚫ | ImageFile1 = Ammonium-persulfate-3D-balls-ionic.png
⚫ | ImageFile = Ammonium-persulfate.svg
⚫ | ImageSize1 = 240px
| ImageName1 = Ball-and-stick models of two ammonium cations and one peroxydisulfate anion | ImageName = Structural formulas of two ammonium cations and one peroxydisulfate anion
⚫ | ImageFile1 = Ammonium-persulfate-3D-balls-ionic.png
⚫ | ImageFile2 = Peroxodisíran amonný.JPG
⚫ | ImageSize1 = 240px
⚫ | ImageName2 = Solid sample of ammonium persulfate, as a white powder
| OtherNames = Ammonium peroxydisulfate | ImageName1 = Ball-and-stick models of two ammonium cations and one peroxydisulfate anion
⚫ | ImageFile2 = Peroxodisíran amonný.JPG
⚫ | ImageName2 = Solid sample of ammonium persulfate, as a white powder
| OtherNames = {{Unbulleted list|Ammonium peroxydisulfate}}
| IUPACName =
| SystematicName =
| Section1 = {{Chembox Identifiers | Section1 = {{Chembox Identifiers
| UNII_Ref = {{fdacite|correct|FDA}} | UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 22QF6L357F | UNII = 22QF6L357F
| InChI = 1/2H3N.H2O8S2/c;;1-9(2,3)7-8-10(4,5)6/h2*1H3;(H,1,2,3)(H,4,5,6) | InChI = 1/2H3N.H2O8S2/c;;1-9(2,3)7-8-10(4,5)6/h2*1H3;(H,1,2,3)(H,4,5,6)
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| StdInChIKey = ROOXNKNUYICQNP-UHFFFAOYSA-N | StdInChIKey = ROOXNKNUYICQNP-UHFFFAOYSA-N
| CASNo = 7727-54-0 | CASNo = 7727-54-0
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| EINECS = 231-786-5 | PubChem = 62648
| UNNumber = 1444 | EINECS = 231-786-5
| RTECS = SE0350000 | UNNumber = 1444
| RTECS = SE0350000
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID=56400 | ChemSpiderID =56400
}} }}
| Section2 = {{Chembox Properties | Section2 = {{Chembox Properties
| Formula = (NH<sub>4</sub>)<sub>2</sub>S<sub>2</sub>O<sub>8</sub> | Formula = (NH<sub>4</sub>)<sub>2</sub>S<sub>2</sub>O<sub>8</sub>
| MolarMass = 228.18 g/mol | MolarMass = 228.18 g/mol
| Appearance = white to yellowish crystals | Appearance = white to yellowish crystals
| Density = 1.98 g/cm<sup>3</sup> | Density = 1.98 g/cm<sup>3</sup>
| Solubility = 80 g/100 ml (25 °C) | Solubility = 80 g/100 mL (25 °C)
| SolubleOther = Moderately soluble in MeOH
| MeltingPt = 120 °C (393 K) decomp.
| pKa = | MeltingPtC = 120
| MeltingPt_notes = decomposes
⚫ | pKb =
| pKa =
| pKb =
}} }}
| Section3 = {{Chembox Structure | Section3 = {{Chembox Structure
| MolShape = | MolShape =
| Coordination = | Coordination =
| CrystalStruct = | CrystalStruct =
| Dipole = | Dipole =
}} }}
| Section4 =
| Section5 =
| Section6 =
| Section7 = {{Chembox Hazards | Section7 = {{Chembox Hazards
| ExternalSDS =
| ExternalMSDS =
| GHSPictograms = {{GHS03}}{{GHS07}}{{GHS08}}
| EUIndex = 016-060-00-6
| GHSSignalWord = Danger
| EUClass = Oxidant ('''O''')<br/>Harmful ('''Xn''')<br/>Irritant ('''Xi''')
| HPhrases = {{H-phrases|272|302|315|319|334|317|335}}
| RPhrases = {{R8}}, {{R22}}, {{R36/37/38}}, {{R42/43}}
| PPhrases = {{P-phrases|210|221|284|305+351+338|405|501}}
| SPhrases = {{S2}}, {{S22}}, {{S24}}, {{S26}}, {{S37}}
| NFPA-H = 2 | NFPA-H = 2
| NFPA-F = 0 | NFPA-F = 1
| NFPA-R = 2 | NFPA-R = 2
| NFPA-O = OX | NFPA-S = OX
| FlashPt = | FlashPt =
| LD50 = 689 mg/kg, oral (rat) | LD50 = 689 mg/kg (rat, oral);<br/>2,000 mg/kg (rat, dermal);<br/>2.95 mg/L for 4 hours (rat, inhalation)
| TLV = Airborne: 0.1 mg/m³ (TWA)
}} }}
| Section8 = {{Chembox Related | Section8 = {{Chembox Related
| OtherAnions = ]<br/>]<br/>] | OtherAnions = ]<br/>]<br/>]
| OtherCations = ]<br/>] | OtherCations = ]<br/>]
| OtherCpds = | OtherCompounds =
}} }}
}} }}
'''Ammonium persulfate''' (NH<sub>4</sub>)<sub>2</sub>S<sub>2</sub>O<sub>8</sub> is a strong ]. It is very soluble in water; the dissolution of the salt in water is endothermic. It is a ]. It is used to etch copper on ] as an alternative to ] solution.<ref>{{cite web | url = http://www.mgchemicals.com/products/410.html | publisher = MG Chemicals | title = Ammonium Persulphate: Copper Etchant}}</ref> It is also used along with ] to catalyze the polymerization of ] in making a ] gel. '''Ammonium persulfate (APS)''' is the ] with the formula (NH<sub>4</sub>)<sub>2</sub>S<sub>2</sub>O<sub>8</sub>. It is a colourless (white) ] that is highly soluble in water, much more so than the related ]. It is a strong ] that is used as a catalyst in ], as an ], and as a cleaning and ].<ref name = Ullmann/>


==Preparation and structure==
Ammonium persulfate was prepared by H. Marshall by the method used for the preparation of ] &mdash; by the electrolysis of a solution of ] and ].<ref>{{cite journal | title = LXXIV. Contributions from the Chemical Laboratory of the University of Edinburgh. No. V. The persulphates | author = Hugh Marshall | journal = ] | year = 1891 | volume = 59 | pages = 771 | doi = 10.1039/CT8915900771}}</ref>
Ammonium persulfate is prepared by ] of a cold concentrated solution of either ] or ] in ] at a high ].<ref>{{Cite journal|last1=Shafiee|first1=Saiful Arifin|last2=Aarons|first2=Jolyon|last3=Hamzah|first3=Hairul Hisham|year=2018|title=Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction|url=http://m.jes.ecsdl.org/content/165/13/H785.abstract?sid=3ddef67b-7f3b-49fa-93a7-c6eee812bfe4|journal=Journal of the Electrochemical Society|volume=165|issue=13|pages=H785–H798|doi=10.1149/2.1161811jes|s2cid=106396614 |doi-access=free}}</ref><ref name=Brauer>F. Feher, "Potassium Peroxydisulfate" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 390.</ref> The method was first described by ].<ref>{{cite journal | title = LXXIV. Contributions from the Chemical Laboratory of the University of Edinburgh. No. V. The trisulphates | author = Hugh Marshall | journal = ] | year = 1891 | volume = 59 | pages = 771–786 | doi = 10.1039/CT8915900771| url = https://zenodo.org/record/1723783 }}</ref>


The ammonium, sodium, and potassium salts adopt very similar structures in the solid state, according to ]. In the ammonium salt, the ] distance is 1.497{{nbsp}}Å. The sulfate groups are ], with three short S-O distances near 1.44{{nbsp}}Å and one long S-O bond at 1.64{{nbsp}}Å.<ref>{{cite journal |doi=10.1524/zkri.1969.130.16.449|title=A reinvestigation of the crystal structure of ammonium persulfate, (NH4)2S2O8 |year=1969 |last1=Sivertsen |first1=Β. K. |last2=Sorum |first2=H. |journal=Zeitschrift für Kristallographie - Crystalline Materials |volume=130 |issue=1–6 |pages=449–460 |s2cid=95804764 }}</ref>
Ammonium persulfate is the main component of ]. On dissolving in ], it is used to clean ] as a metal-free alternative to ] baths.<ref>{{cite web | publisher = ] | url = http://www.sigmaaldrich.com/catalog/search/SpecificationSheetPage/ALDRICH/328693 | title = Nochromix | accessdate = 2008-03-01}} {{Dead link|date=October 2010|bot=H3llBot}}</ref> It is also a standard ingredient in ] gels and ].

==Uses==
As a source of ], APS is mainly used as a ] in the ] of certain ]s. Commercially important polymers prepared using persulfates include ] and ]. In solution, the ] dissociates into radicals:<ref name = Ullmann>{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob |author2=Stefan Leininger |author3=Thomas Lehmann |author4=Sylvia Jacobi |author5=Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}}</ref>
:<sup>2−</sup> {{eqm}} 2 <sup>•−</sup>
Regarding its mechanism of action, the sulfate radical adds to the alkene to give a ] radical. It is also used along with ] to catalyze the polymerization of ] in making a ] gel, hence being important for ] and ].

Illustrative of its powerful oxidizing properties, ammonium persulfate is used to etch ] on ] as an alternative to ] solution.<ref name = Ullmann/><ref>{{cite web | url = http://www.mgchemicals.com/products/prototyping-and-circuit-repair/prototyping/ammonium-persulphate-410 | publisher = MG Chemicals | title = Ammonium Persulphate: Copper Etchant}}</ref> This property was discovered many years ago. In 1908, John William Turrentine used a dilute ammonium persulfate solution to etch copper. Turrentine weighed copper spirals before placing the copper spirals into the ammonium persulfate solution for an hour. After an hour, the spirals were weighed again and the amount of copper dissolved by ammonium persulfate was recorded. This experiment was extended to other metals such as ], ], and ], all of which yielded similar results.<ref>{{cite journal | title = Action of Ammonium Persulphate on Metals. | author = Turrentine, J. W. | journal = Journal of Physical Chemistry | year = 1908 | volume = 11 | issue = 8 | pages = 623–631 | doi=10.1021/j150089a004| url = https://zenodo.org/record/1428764 }}</ref>
The oxidation equation is thus: {{chem|S|2|O|8|2−}} (aq) + 2 {{E-}} → 2 {{chem|SO|4|2−}} (aq).

Ammonium persulfate is a standard ingredient in ].

Persulfates are used as ] in ].<ref>''Encyclopedia of Reagents for Organic Synthesis'', vol. 1, pp.&nbsp;193–197 (1995).</ref> For example, in the ] and ]


==Safety== ==Safety==
Airborne dust may be irritating to ], ], ], ] and ] upon contact. Exposure to high levels of dust may cause difficulty in breathing.<ref> FMC Corporation, MSDS sheet dated: 06/26/2009 </ref> Airborne dust containing ammonium persulfate may be irritating to ], ], ], ] and ] upon contact. Exposure to high levels of dust may cause difficulty in breathing.<ref>{{cite web|url=http://msds.fmc.com/msds/100000010587-MSDS_US-E.pdf |title=Archived copy |access-date=2010-03-08 |url-status=dead |archive-url=https://web.archive.org/web/20110711014614/http://msds.fmc.com/msds/100000010587-MSDS_US-E.pdf |archive-date=2011-07-11 }} FMC Corporation, MSDS sheet dated: 2009-06-26</ref>

It has been noted that persulfate salts are a major cause of ]tic effects.<ref>{{cite journal | title = Ammonium persulfate can initiate an asthmatic response in mice. |author1=De Vooght, V. |author2=Jesus Cruz, M. |author3=Haenen, S. |author4=Wijnhoven, K. |author5=Munoz, X. |author6=Cruz, M. |author7=Munoz, X. |author8=Morell, F. |author9=Nemery, B. | journal = Thorax | year = 2010 | volume = 65 |issue=3 | pages = 252–257 | doi=10.1136/thx.2009.121293 | pmid=20335296|doi-access=free }}</ref> Furthermore, it has been suggested that exposure to ammonium persulfate can cause asthmatic effects in ] and receptionists working in the hairdressing industry. These asthmatic effects are proposed to be caused by the oxidation of ] residues, as well as ] residues.<ref>{{cite journal | title = Oxidative activity of ammonium persulfate salt on mast cells and basophils: implication in hairdressers' asthma. |author1=Pignatti, P. |author2=Frossi, B. |author3=Pala, G. |author4=Negri, S. |author5=Oman, H. |author6=Perfetti, L. |author7=Pucillo, C. |author8=Imbriani, M. |author9=Moscato, G. | journal = Int. Arch. Allergy Immunol. | year = 2013 | volume = 160 |issue=4 | pages = 409–419 | doi=10.1159/000343020|pmid=23183487 |s2cid=1540905 }}</ref>


==References== ==References==
{{Reflist}}
<references/>


==External links== ==External links==
* *
*


{{Ammonium salts}}
{{Persulfates}}
{{E number infobox 920-929}} {{E number infobox 920-929}}


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