Sodium persulfate

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-2 Key: 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-2 Key: CHQMHPLRPQMAMX-NUQVWONBAA;
	SMILES [Na+].[Na+].O=S(=O)([O-])OOS([O-])(=O)=O;
Properties
Chemical formula	Na2S2O8
Molar mass	238.10 g/mol
Appearance	white powder
Density	2.59 g/cm3; (Loose bulk density: 1.12 g/cm3)[1]
Melting point	180 °C (356 °F; 453 K) decomposes
Solubility in water	55.6 g/100 ml (20 °C)
Hazards
Safety data sheet	ICSC 1136
GHS pictograms
GHS Signal word	Danger
GHS hazard statements	H272, H302, H315, H317, H319, H334, H335, H371
GHS precautionary statements	P220, P261, P280, P305+351+338, P342+311
NFPA 704 (fire diamond)	0 2 1 OX
Flash point	Non-flammable
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 [77 °F], 100 kPa).
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	Infobox references

Sodium persulfate is the inorganic compound with the formula Na₂S₂ O₈. 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 hydrogen sulfate:

2 NaHSO₄ → Na₂S₂O₈ + H₂

Oxidation is conducted at a platinum anode.[2] In this way about 165,000 tons were produced in 2005.[3]

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).[4] 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.[5]

Applications

It is mainly used as a radical initiator for emulsion polymerization reactions for styrene based polymers such as Acrylonitrile butadiene styrene.[3] 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[5][6] 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.[7]

Safety

The salt is an oxidizer and forms combustible mixtures with organic materials such as paper. Strong reducing agents such as magnesium can form explosive compositions when mixed.

References

FMC Corporation. Sodium Persulfate. "Archived copy" (PDF). Archived from the original (PDF) on 2011-11-21. Retrieved 2013-11-17.CS1 maint: archived copy as title (link) (accessed Nov 17, 2013).
Pietzsch, A.; Adolph, G. J. Chem. Technol. Biotechnol. 1911, 30, 85.
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.CS1 maint: multiple names: authors list (link)
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.
Shafiee, Saiful Arifin; Aarons, Jolyon; Hairul Hisham, Hamzah (2018). "Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction". Journal of the Electrochemical Society. ECS. 165 (13): H785–H798. doi:10.1149/2.1161811jes.
Wacławek, S., Lutze, H. V., Grübel, K., Padil, V.V.T., Černík, M., Dionysiou, D.D. (2017) (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.CS1 maint: multiple names: authors list (link)
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.

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[1] FMC Corporation. Sodium Persulfate. "Archived copy" (PDF). Archived from the original (PDF) on 2011-11-21. Retrieved 2013-11-17.CS1 maint: archived copy as title (link) (accessed Nov 17, 2013).

[2] Pietzsch, A.; Adolph, G. J. Chem. Technol. Biotechnol. 1911, 30, 85.

[Ullmann-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.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.

[:0-5] Shafiee, Saiful Arifin; Aarons, Jolyon; Hairul Hisham, Hamzah (2018). "Electroreduction of Peroxodisulfate: A Review of a Complicated Reaction". Journal of the Electrochemical Society. ECS. 165 (13): H785–H798. doi:10.1149/2.1161811jes.

[6] Wacławek, S., Lutze, H. V., Grübel, K., Padil, V.V.T., Černík, M., Dionysiou, D.D. (2017) (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.CS1 maint: multiple names: authors list (link)

[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.