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Sodium persulfate

Names
Other names Sodium peroxodisulfate Sodium peroxodisulphate Sodium peroxydisulfate Sodium peroxydisulphate
Identifiers
CAS Number	7775-27-1
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL502764
ChemSpider	56406
ECHA InfoCard	100.028.993
EC Number	231-892-1
PubChem CID	62655
RTECS number	SE0525000
UNII	J49FYF16JE
UN number	1505
CompTox Dashboard (EPA)	DTXSID4029698
InChI InChI=1S/2Na.H2O8S2/c;;1-9(2,3)7-8-10(4,5)6/h;;(H,1,2,3)(H,4,5,6)/q2*+1;/p-2Key: CHQMHPLRPQMAMX-UHFFFAOYSA-L InChI=1/2Na.H2O8S2/c;;1-9(2,3)7-8-10(4,5)6/h;;(H,1,2,3)(H,4,5,6)/q2*+1;/p-2Key: CHQMHPLRPQMAMX-NUQVWONBAA
SMILES ..O=S(=O)()OOS()(=O)=O
Properties
Chemical formula	Na2S2O8
Molar mass	238.10 g/mol
Appearance	White powder
Density	2.601 g/cm
Melting point	180 °C (356 °F; 453 K) decomposes
Solubility in water	55.6 g/100 ml (20 °C)
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H302, H315, H317, H319, H334, H335, H371
Precautionary statements	P220, P261, P280, P305+P351+P338, P342+P311
NFPA 704 (fire diamond)	2 0 1OX
Flash point	Non-flammable
Safety data sheet (SDS)	ICSC 1136
Related compounds
Other anions	Sodium dithionite Sodium sulfite Sodium sulfate
Other cations	Potassium persulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is  ?) Infobox references

Sodium persulfate is the inorganic compound with the formula Na₂S₂O₈. It is the sodium salt of peroxydisulfuric acid, H₂S₂O₈, an oxidizing agent. It is a white solid that dissolves in water. It is almost non-hygroscopic and has good shelf-life.

Production

The salt is prepared by the electrolytic oxidation of sodium bisulfate:

${\displaystyle {\ce {2 NaHSO4 -> Na2S2O8 + H2}}}$

Oxidation is conducted at a platinum anode. In this way about 165,000 tons were produced in 2005.

The standard redox potential of sodium persulfate into hydrogen sulfate is 2.1 V, which is higher than that of hydrogen peroxide (1.8 V) but lower than ozone (2.2 V). The sulfate radical formed in situ has a standard electrode potential of 2.7 V.

However, there are a few drawbacks in utilizing platinum anodes to produce the salts; the manufacturing process is inefficient due to oxygen evolution and the product could contain contaminants coming from platinum corrosion (mainly due to extremely oxidizing nature of the sulfate radical). Thus, boron-doped diamond electrodes have been proposed as alternatives to the conventional platinum electrodes.

Structure

The sodium and potassium salts adopt very similar structures in the solid state, according to X-ray crystallography. In the sodium salt, the O-O distance is 1.476 Å. The sulfate groups are tetrahedral, with three short S-O distances near 1.44 and one long S-O bond at 1.64 Å.

Applications

It is mainly used as a radical initiator for emulsion polymerization reactions for styrene based polymers such as Acrylonitrile butadiene styrene. Also applicable for accelerated curing of low formaldehyde adhesives.

Other uses

It is a bleach, both standalone (particularly in hair cosmetics) and as a detergent component. It is a replacement for ammonium persulfate in etching mixtures for zinc and printed circuit boards, and is used for pickling of copper and some other metals.

It is also used as a soil conditioner and for soil and groundwater remediation and in manufacture of dyestuffs, modification of starch, bleach activator, desizing agent for oxidative desizing, etc.

Organic chemistry

Sodium persulfate is a specialized oxidizing agent in chemistry, classically in the Elbs persulfate oxidation and the Boyland–Sims oxidation reactions. It is also used in radical reactions; for example in a synthesis of diapocynin from apocynin where iron(II) sulfate is the radical initiator.

Safety

The salt is an oxidizer and forms combustible mixtures with organic materials such as paper.

References

1. ^ Allan, David R. (2006). "Sodium peroxodisulfate". Acta Crystallographica Section E. 62 (3): i44–i46. doi:10.1107/S1600536806004302.
2. Pietzsch, A.; Adolph, G. J. Chem. Technol. Biotechnol. 1911, 30, 85.
3. ^ 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.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
4. Block, Philip A., Richard A. Brown, and David Robinson. "Novel activation technologies for sodium persulfate in-situ chemical oxidation." Proceedings of the Fourth International Conference on the remediation of chlorinated and recalcitrant compounds. 2004.
5. ^ Shafiee, Saiful Arifin; Aarons, Jolyon; Hairul Hisham, Hamzah (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.
6. Wacławek, Stanisław; Lutze, Holger V.; Grübel, Klaudiusz; Padil, Vinod V.T.; Černík, Miroslav; Dionysiou, Dionysios.D. (2017). "Chemistry of persulfates in water and wastewater treatment: A review". Chemical Engineering Journal. 330: 44–62. doi:10.1016/j.cej.2017.07.132.
7. Luchtefeld, Ron; Dasari, Mina S.; Richards, Kristy M.; Alt, Mikaela L.; Crawford, Clark F. P.; Schleiden, Amanda; Ingram, Jai; Hamidou, Abdel Aziz Amadou; et al. (2008). "Synthesis of Diapocynin". J. Chem. Educ. 85 (3): 411. Bibcode:2008JChEd..85..411D. doi:10.1021/ed085p411.

• Persulfates
• Sodium compounds
• Oxidizing agents