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'''Ammonium persulfate (APS)''' (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. In addition, a high ammonium persulfate solution can be used to leach copper from chalcopyrite under high pressure conditions. <ref>{{cite journal | title = Leaching of copper from chalcopyrite concentrate by using ammonium persulphate in an autoclave: Determination of most suitable impeller type by using response surface methodology. | author = Turan, M; Altundoğan, H. S.| journal = Journal of Central South University | year = 2013 | volume = 20 | pages = 622-628}}</ref> '''Ammonium persulfate (APS)''' (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. When APS dissolves in water, it is broken down into ] and ]. 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. In addition, a high ammonium persulfate solution can be used to leach copper from chalcopyrite under high pressure conditions. <ref>{{cite journal | title = Leaching of copper from chalcopyrite concentrate by using ammonium persulphate in an autoclave: Determination of most suitable impeller type by using response surface methodology. | author = Turan, M; Altundoğan, H. S.| journal = Journal of Central South University | year = 2013 | volume = 20 | pages = 622-628}}</ref>


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 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>

Revision as of 00:19, 20 November 2013

Ammonium persulfate
Structural formulas of two ammonium cations and one peroxydisulfate anion
Ball-and-stick models of two ammonium cations and one peroxydisulfate anion
Solid sample of ammonium persulfate, as a white powder
Names
Other names Ammonium peroxydisulfate
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.897 Edit this at Wikidata
EC Number
  • 231-786-5
E number E923 (glazing agents, ...)
RTECS number
  • SE0350000
UNII
UN number 1444
CompTox Dashboard (EPA)
InChI
  • InChI=1S/2H3N.H2O8S2/c;;1-9(2,3)7-8-10(4,5)6/h2*1H3;(H,1,2,3)(H,4,5,6)Key: ROOXNKNUYICQNP-UHFFFAOYSA-N
  • 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)Key: ROOXNKNUYICQNP-UHFFFAOYAL
SMILES
  • O=S(=O)()OOS()(=O)=O..
  • ..S(=O)(=O)OOS(=O)(=O)
Properties
Chemical formula (NH4)2S2O8
Molar mass 228.18 g/mol
Appearance white to yellowish crystals
Density 1.98 g/cm
Melting point 120 °C (393 K) decomp.
Solubility in water 80 g/100 ml (25 °C)
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2 0 2OX
Lethal dose or concentration (LD, LC):
LD50 (median dose) 689 mg/kg, oral (rat)
Related compounds
Other anions Ammonium thiosulfate
Ammonium sulfite
Ammonium sulfate
Other cations Sodium persulfate
Potassium persulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Ammonium persulfate (APS) (NH4)2S2O8 is a strong oxidizing agent. It is very soluble in water; the dissolution of the salt in water is endothermic. When APS dissolves in water, it is broken down into ammonia and peroxydisulfuric acid. It is a radical initiator. It is used to etch copper on printed circuit boards as an alternative to ferric chloride solution. It is also used along with tetramethylethylenediamine to catalyze the polymerization of acrylamide in making a polyacrylamide gel. In addition, a high ammonium persulfate solution can be used to leach copper from chalcopyrite under high pressure conditions.

Ammonium persulfate was prepared by H. Marshall by the method used for the preparation of potassium persulfate — by the electrolysis of a solution of ammonium sulfate and sulfuric acid.

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 nickel, cadium, and iron, all of which yielded similar results.

Ammonium persulfate is the main component of Nochromix. On dissolving in sulfuric acid, it is used to clean laboratory glassware as a metal-free alternative to chromic acid baths. It is also a standard ingredient in western blot gels and hair bleach.

Safety

Airborne dust may be irritating to eye, nose, throat, lung and skin upon contact. Exposure to high levels of dust may cause difficulty in breathing.

It has been noted that persulfate salts are a major cause of asthmatic effects in women. Furthermore, it has been suggested that exposure to ammonium persulfate can cause asthmatic effects in hair dressers and receptionists working in the hair dressing industry. These asthmatic affects are proposed to be caused by the oxidation of cysteine residues, as well as methionine residues.

References

  1. "Ammonium Persulphate: Copper Etchant". MG Chemicals.
  2. Turan, M; Altundoğan, H. S. (2013). "Leaching of copper from chalcopyrite concentrate by using ammonium persulphate in an autoclave: Determination of most suitable impeller type by using response surface methodology". Journal of Central South University. 20: 622–628.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  3. Hugh Marshall (1891). "LXXIV. Contributions from the Chemical Laboratory of the University of Edinburgh. No. V. The persulphates". J. Chem. Soc., Trans. 59: 771. doi:10.1039/CT8915900771.
  4. Turrentine, J. W. (1908). "Action of Ammonium Persulphate on Metals". Journal of Physical Chemistry. 11: 623–631.
  5. "Nochromix". Sigma-Aldrich. Retrieved 2008-03-01.
  6. FMC Corporation, MSDS sheet dated: 06/26/2009
  7. De Vooght, V.; Jesus Cruz, M.; Haenen, S.; Wijnhoven, K.; Munoz, X.; Cruz, M.; Munoz, X.; Morell, F.; Nemery, B (2010). "Ammonium persulfate can initiate an asthmatic response in mice". Thorax. 65: 252–257.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  8. Pignatti, P.; Frossi, B.; Pala, G.; Negri, S.; Oman, H.; Perfetti, L.; Pucillo, C.; Imbriani, M.; Moscato, G. (2013). "Oxidative activity of ammonium persulfate salt on mast cells and basophils: implication in hairdressers' asthma". Int. Arch. Allergy Immunol. 160: 409–419.{{cite journal}}: CS1 maint: multiple names: authors list (link)

For a review of its uses in organic chemistry see Encyclopedia of Reagents for Organic Synthesis, vol. 1, pp. 193–197(1995).

External links

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