Sodium persulfate

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Sodium persulfate
Two sodium cations and one peroxodisulphate anion
Ball-and-stick model of the crystal structure
Sodium persulfate as a white powder
Identifiers
CAS number 7775-27-1 YesY
PubChem 62655
ChemSpider 56406 YesY
EC number 231-892-1
UN number 1505
ChEMBL CHEMBL502764 YesY
RTECS number SE0525000
Jmol-3D images Image 1
Properties
Molecular formula Na2S2O8
Molar mass 238.10 g/mol (19.31& Na, 53.76% O, 26.93% S) [1]
Appearance white powder
Density 2.40 g/cm3
   Loose bulk density = 1.12 g/cm3[2]
   Crystal density = 2.59 g/cm3[3]
Melting point 180 °C decomp.
Solubility in water 55.6 g/100 ml (20 °C)
Hazards
MSDS ICSC 1136
EU Index Not listed
R-phrases R8 R20 R22 R36 R37 R38
S-phrases S17 S26 S36
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point Non-flammable
Related compounds
Other anions Sodium dithionite
Sodium sulfite
Sodium sulfate
Other cations Potassium persulfate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY (verify) (what is: YesY/N?)
Infobox references

Sodium persulfate (Na2S2O8) is a chemical compound. It is a strong oxidizer. It is a severe irritant of the skin, eyes, and respiratory system. It is almost non-hygroscopic and has particularly good ability to be stored for long time. It is easy and safe to handle. It is not combustible, but releases oxygen easily and assists combustion of other materials.

It is used as 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 a source of free radicals, making it useful as a radical initiator for emulsion polymerization reactions and for accelerated curing of low formaldehyde adhesives. It is also used as a soil conditioner and in manufacture of dyestuffs, modification of starch, bleach activator, desizing agent for oxidative desizing, etc.

Conditions/substances to avoid mixing persulfates with are: moisture, heat, flame, ignition sources, shock, friction, reducing agents, organic material, sodium peroxide, water, aluminium, and powdered metals.

Sodium persulfate is an oxidizing agent in chemistry, for example in a synthesis of diapocynin from apocynin where iron(II) sulfate is the radical initiator:[4]

Diapocynin Synthesis

Sodium persulfate is synthesized using water and sodium sulfate (Na2SO4 * 10H2O) in electrolysis with a pure platinum anode. [5] ( Link to IR Spectra [6] )

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).[7] The sulfate radical formed in situ has a standard electrode potential of 2.7 V.

References[edit]

  1. ^ Anonymous Sodium Persulfate. In Merck Index; O'Neil, M. J., Ed.; Merck & Co., Inc.: Whitehouse Station, NJ, 2006; pp 1488.
  2. ^ FMC Corporation. Sodium Persulfate. http://www.fmcchemicals.com/Portals/chem/Content/docs/Tech%20Data%20Sheets/sodpersulfate.pdf (accessed Nov 17, 2013).
  3. ^ FMC Corporation. Sodium Persulfate. http://www.fmcchemicals.com/Portals/chem/Content/docs/Tech%20Data%20Sheets/sodpersulfate.pdf (accessed Nov 17, 2013).
  4. ^ 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. Ed. 85 (3): 411. doi:10.1021/ed085p411. 
  5. ^ Pietzsch, A.; Adolph, G. J. Chem. Technol. Biotechnol. 1911, 30, 85.
  6. ^ Anonymous. Spectral Database for Organic Compounds. http://sdbs.db.aist.go.jp/sdbs/cgi-bin/direct_frame_disp.cgi?sdbsno=40242 (accessed Oct 7, 2013).
  7. ^ 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.