Sodium perchlorate
Sodium perchlorate is the inorganic compound with the chemical formula NaClO4. It is a white crystalline, hygroscopic solid that is highly soluble in water and in alcohol. It is usually encountered as the monohydrate. The compound is noteworthy as the most water-soluble of the common perchlorate salts.
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Other names
Sodium chlorate(VII) Sodium hyperchlorate Perchloric acid, sodium salt | |
Identifiers | |
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ChEBI | |
ChEMBL | |
ChemSpider | |
ECHA InfoCard | 100.028.647 |
EC Number |
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PubChem CID |
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RTECS number |
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UNII | |
UN number | 1502 |
CompTox Dashboard (EPA) |
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Properties | |
NaClO4 NaClO4.H2O (monohydrate) | |
Molar mass | 122.44 g/mol |
Appearance | White crystalline solid |
Density | 2.4994 g/cm3 2.02 g/cm3 (monohydrate) |
Melting point | 468 °C (874 °F; 741 K) (decomposes, anhydrous) 130 °C (monohydrate) |
Boiling point | 482 °C (900 °F; 755 K) (decomposes, monohydrate) |
209.6 g/100 mL (25 °C, anhydrous) 209 g/100 mL (15 °C, monohydrate) | |
Refractive index (nD) |
1.4617 |
Structure | |
orthorhombic | |
Hazards | |
GHS labelling: | |
Danger | |
H271, H302, H319, H373 | |
P102, P220, P305+P351+P338, P338 | |
NFPA 704 (fire diamond) | |
Flash point | 400 °C (752 °F; 673 K) |
Safety data sheet (SDS) | ICSC 0715 |
Related compounds | |
Other anions |
Sodium chloride Sodium hypochlorite Sodium chlorite Sodium chlorate |
Other cations |
Lithium perchlorate Potassium perchlorate Ammonium perchlorate Caesium perchlorate |
Related compounds |
Perchloric acid |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references |
Sodium perchlorate and other perchlorates has been found on the planet Mars, first detected by the NASA probe Phoenix in 2009. This was later confirmed by spectral analysis by the Mars Reconnaissance Orbiter in 2015 of what is thought to be brine seeps which may be the first evidence of flowing liquid water containing hydrated salts on Mars.[1][2]
Selected properties
Its heat of formation is −382.75 kJ/mol, i.e. it is thermally stable up to high temperatures. At 490 °C it undergoes thermal decomposition, producing sodium chloride and dioxygen.[3]
It crystallizes in the rhombic crystal system.[4]
Uses
Sodium perchlorate is the precursor to many other perchlorate salts, often taking advantage of their low solubility relative to NaClO4 (209 g/100 mL at 25 °C). Perchloric acid is made by treating NaClO4 with HCl.
Ammonium perchlorate and potassium perchlorate, of interest in rocketry and pyrotechnics, are prepared by double decomposition from a solution of sodium perchlorate and ammonium chloride or potassium chloride, respectively.
Laboratory applications
Solutions of NaClO4 are often used as an unreactive electrolyte. It is used in standard DNA extraction and hybridization reactions in molecular biology.
Production
Sodium perchlorate is produced by anodic oxidation of sodium chlorate (NaClO3) at an inert electrode, such as platinum.[6]
- Na+ClO3− + H2O → Na+ClO4− + 2H+ + 2 e− (acidic medium)
- Na+ClO3− + 2 OH− → Na+ClO4− + H2O + 2 e− (alkaline medium)
See also
References
- Wadsworth, Jennifer; Cockell, Charles S. (July 6, 2017). "Perchlorates on Mars enhance the bacteriocidal effects of UV light". Scientific Reports. 7 (2017, #4662): 4662. Bibcode:2017NatSR...7.4662W. doi:10.1038/s41598-017-04910-3. PMC 5500590. PMID 28684729.
- Delbecq, Denis (September 28, 2015). "De l'eau liquide répérée sur les pentes martiennes" [Liquid water spotted on Martian slopes]. Le Temps (in French). Archived from the original on January 18, 2017. Retrieved August 23, 2021.
- Devlin, D. J.; Herley, P. J. (1987). "Thermal decomposition and dehydration of sodium perchlorate monohydrate". Reactivity of Solids. 3 (1–2): 75–84. doi:10.1016/0168-7336(87)80019- (inactive 2023-08-26). Retrieved 3 May 2023.
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: CS1 maint: DOI inactive as of August 2023 (link) - Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 978-3-11-011451-5. Retrieved March 7, 2013.
- Becker C. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Radiologe. 2007 Sep;47(9):768-73.
- Helmut Vogt; Jan Balej; John E. Bennett; Peter Wintzer; Saeed Akbar Sheikh; Patrizio Gallone (2002). "Chlorine Oxides and Chlorine Oxygen Acids". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a06_483. ISBN 3-527-30673-0.