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
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
  • 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) checkY
    Key: ROOXNKNUYICQNP-UHFFFAOYSA-N checkY
  • 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
  • O=S(=O)([O-])OOS([O-])(=O)=O.[NH4+].[NH4+]
  • [NH4+].[NH4+].[O-]S(=O)(=O)OOS(=O)(=O)[O-]
Properties
(NH4)2S2O8
Molar mass 228.18 g/mol
Appearance white to yellowish crystals
Density 1.98 g/cm3
Melting point 120 °C (248 °F; 393 K) decomposes
80 g/100 mL (25 °C)
Solubility Moderately soluble in MeOH
Hazards
GHS labelling:
GHS03: OxidizingGHS07: Exclamation markGHS08: Health hazard
Danger
H272, H302, H315, H317, H319, H334, H335
P210, P221, P284, P305+P351+P338, P405, P501
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 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 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
1
2
OX
Airborne: 0.1 mg/m³ (TWA)
Lethal dose or concentration (LD, LC):
689 mg/kg (rat, oral);
2,000 mg/kg (rat, dermal);
2.95 mg/L for 4 hours (rat, inhalation)
Safety data sheet (SDS) 7727-54-0
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 [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Ammonium persulfate (APS) is the inorganic compound with the formula (NH4)2S2O8. It is a colourless (white) salt that is highly soluble in water, much more so than the related potassium salt. It is a strong oxidizing agent that is used as a catalyst in polymer chemistry, as an etchant, and as a cleaning and bleaching agent.[1]

Preparation and structure

Ammonium persulfate is prepared by electrolysis of a cold concentrated solution of either ammonium sulfate or ammonium bisulfate in sulfuric acid at a high current density.[2][3] The method was first described by Hugh Marshall.[4]

The ammonium, sodium, and potassium salts adopt very similar structures in the solid state, according to X-ray crystallography. In the ammonium salt, the O-O distance is 1.497 Å. The sulfate groups are tetrahedral, with three short S-O distances near 1.44 Å and one long S-O bond at 1.64 Å.[5]

Uses

As a source of radicals, APS is mainly used as a radical initiator in the polymerization of certain alkenes. Commercially important polymers prepared using persulfates include styrene-butadiene rubber and polytetrafluoroethylene. In solution, the dianion dissociates into radicals:[1]

[O3SO–OSO3]2− ⇌ 2 [SO4]•−

Regarding its mechanism of action, the sulfate radical adds to the alkene to give a sulfate ester radical. It is also used along with tetramethylethylenediamine to catalyze the polymerization of acrylamide in making a polyacrylamide gel, hence being important for SDS-PAGE and western blot.

Illustrative of its powerful oxidizing properties, ammonium persulfate is used to etch copper on printed circuit boards as an alternative to ferric chloride solution.[1][6] 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 nickel, cadmium, and iron, all of which yielded similar results.[7] The oxidation equation is thus: S
2O2−
8 (aq) + 2  e− → 2 SO2−
4 (aq).

Ammonium persulfate is a standard ingredient in hair bleach.

Persulfates are used as oxidants in organic chemistry.[8] For example, in the Minisci reaction and Elbs persulfate oxidation

Safety

Airborne dust containing ammonium persulfate may be irritating to eye, nose, throat, lung and skin upon contact. Exposure to high levels of dust may cause difficulty in breathing.[9]

It has been noted that persulfate salts are a major cause of asthmatic effects.[10] Furthermore, it has been suggested that exposure to ammonium persulfate can cause asthmatic effects in hair dressers and receptionists working in the hairdressing industry. These asthmatic effects are proposed to be caused by the oxidation of cysteine residues, as well as methionine residues.[11]

References

  1. ^ a b c Harald Jakob; Stefan Leininger; Thomas Lehmann; Sylvia Jacobi; Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3527306732.
  2. ^ Shafiee, Saiful Arifin; Aarons, Jolyon; Hamzah, Hairul Hisham (2018). "Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction". Journal of the Electrochemical Society. 165 (13): H785–H798. doi:10.1149/2.1161811jes. S2CID 106396614.
  3. ^ F. Feher, "Potassium Peroxydisulfate" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 390.
  4. ^ Hugh Marshall (1891). "LXXIV. Contributions from the Chemical Laboratory of the University of Edinburgh. No. V. The trisulphates". J. Chem. Soc., Trans. 59: 771–786. doi:10.1039/CT8915900771.
  5. ^ Sivertsen, Β. K.; Sorum, H. (1969). "A reinvestigation of the crystal structure of ammonium persulfate, (NH4)2S2O8". Zeitschrift für Kristallographie - Crystalline Materials. 130 (1–6): 449–460. doi:10.1524/zkri.1969.130.16.449. S2CID 95804764.
  6. ^ "Ammonium Persulphate: Copper Etchant". MG Chemicals.
  7. ^ Turrentine, J. W. (1908). "Action of Ammonium Persulphate on Metals". Journal of Physical Chemistry. 11 (8): 623–631. doi:10.1021/j150089a004.
  8. ^ Encyclopedia of Reagents for Organic Synthesis, vol. 1, pp. 193–197 (1995).
  9. ^ "Archived copy" (PDF). Archived from the original (PDF) on 2011-07-11. Retrieved 2010-03-08.((cite web)): CS1 maint: archived copy as title (link) FMC Corporation, MSDS sheet dated: 2009-06-26
  10. ^ 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 (3): 252–257. doi:10.1136/thx.2009.121293. PMID 20335296.
  11. ^ 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 (4): 409–419. doi:10.1159/000343020. PMID 23183487. S2CID 1540905.

External links

Ammonium salts
Salts and covalent derivatives of the persulfate ion
E numbers
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