Sodium persulfate

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Sodium persulfate
Two sodium cations and one peroxodisulphate anion
Ball-and-stick model of the crystal structure
Sodium persulfate as a white powder
Names
Other names
Sodium peroxodisulfate
Sodium peroxodisulphate
Sodium peroxydisulfate
Sodium peroxydisulphate
Identifiers
  • 7775-27-1 checkY
3D model (JSmol)
ChEMBL
ChemSpider
ECHA InfoCard 100.028.993 Edit this at Wikidata
EC Number
  • 231-892-1
RTECS number
  • SE0525000
UNII
UN number 1505
Properties
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
55.6 g/100 ml (20 °C)
Hazards
Safety data sheet ICSC 1136
GHS pictograms GHS03: Oxidizing GHS07: Harmful GHS08: Health hazard
GHS Signal word Danger
GHS hazard statements
 H272, H302, H315, H317, H319, H334, H335, H371
P220, P261, P280, P305+351+338, P342+311
NFPA 704 (fire diamond)
2
0
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 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 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]

Diapocynin Synthesis

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[]

  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.
  3. ^ Jump up to: a b 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.
  5. ^ Jump up to: a b 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.
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