Ammonium persulfate
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Other names
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.028.897 |
EC Number |
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E number | E923 (glazing agents, ...) |
PubChem CID
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RTECS number
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UNII | |
UN number | 1444 |
CompTox Dashboard (EPA)
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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: | |
Danger | |
H272, H302, H315, H317, H319, H334, H335 | |
P210, P221, P284, P305+P351+P338, P405, P501 | |
NFPA 704 (fire diamond) | |
Threshold limit value (TLV)
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Airborne: 0.1 mg/m³ (TWA) |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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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
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Ammonium thiosulfate Ammonium sulfite Ammonium sulfate |
Other cations
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Sodium persulfate Potassium persulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ammonium persulfate (APS) is the
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
- [O3SO–OSO3]2− ⇌ 2 [SO4]•−
Regarding its mechanism of action, the sulfate radical adds to the alkene to give a
Illustrative of its powerful oxidizing properties, ammonium persulfate is used to etch
2O2−
8 (aq) + 2 e− → 2 SO2−
4 (aq).
Ammonium persulfate is a standard ingredient in
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
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
- ^ ISBN 978-3527306732.
- S2CID 106396614.
- ^ F. Feher, "Potassium Peroxydisulfate" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 390.
- .
- S2CID 95804764.
- ^ "Ammonium Persulphate: Copper Etchant". MG Chemicals.
- .
- ^ Encyclopedia of Reagents for Organic Synthesis, vol. 1, pp. 193–197 (1995).
- ^ "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 - PMID 20335296.
- S2CID 1540905.