Sodium perchlorate

Sodium perchlorate is an inorganic compound with the chemical formula NaClO4. It consists of sodium cations Na+ and perchlorate anions ClO−4. It is a white crystalline, hygroscopic solid that is highly soluble in water and ethanol. It is usually encountered as sodium perchlorate monohydrate NaClO4·H2O. The compound is noteworthy as the most water-soluble of the common perchlorate salts.

Sodium perchlorate
Sodium perchlorte
Names
Other names
  • Perchloric acid, sodium salt
  • Sodium chlorate(VII)
  • Sodium hyperchlorate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.647
EC Number
  • 231-511-9
RTECS number
  • SC9800000
UNII
UN number 1502
  • InChI=1S/ClHO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 checkY
    Key: BAZAXWOYCMUHIX-UHFFFAOYSA-M checkY
  • InChI=1/ClHO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1
    Key: BAZAXWOYCMUHIX-REWHXWOFAU
  • [Na+].[O-]Cl(=O)(=O)=O
Properties
NaClO4 (anhydrous)
NaClO4·H2O (monohydrate)
Molar mass 122.44 g/mol (anhydrous)
140.45 g/mol (monohydrate)
Appearance White crystalline solid
Density 2.4994 g/cm3 (anhydrous)
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)
1.4617
Structure
orthorhombic
Hazards
GHS labelling:
GHS03: Oxidizing GHS07: Exclamation mark GHS08: Health hazard
Danger
H271, H302, H319, H373
P102, P220, P305+P351+P338, P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
2
0
1
OX
Flash point 400 °C (752 °F; 673 K)
Safety data sheet (SDS) ICSC 0715
Related compounds
Other anions
Other cations
Related compounds
 Perchloric acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
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

Perchloric acid is made by treating NaClO4 with HCl.[5] 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. 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).[6]

It is used in standard DNA extraction and hybridization reactions in molecular biology.

In medicine

Sodium perchlorate can be used to block iodine uptake before administration of iodinated contrast agents in patients with subclinical hyperthyroidism (suppressed TSH).[7]

Production

Sodium perchlorate is produced by anodic oxidation of sodium chlorate (NaClO3) at an inert electrode, such as platinum.[5]

Na+ClO−3 + H2O → Na+ClO−4 + 2 H+ + 2 e− (acidic medium)
Na+ClO−3 + 2 OH− → Na+ClO−4 + H2O + 2 e− (alkaline medium)

Safety

LD50 is 2 – 4 g/kg (rabbits, oral).[5]

See also

References
  1. 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.
  2. 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.
  3. 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 31 January 2024). Retrieved 3 May 2023.{{cite journal}}: CS1 maint: DOI inactive as of January 2024 (link)
  4. Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 978-3-11-011451-5. Retrieved March 7, 2013.
  5. Helmut Vogt; Jan Balej; John E. Bennett; Peter Wintzer; Saeed Akbar Sheikh; Patrizio Gallone (2000). "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.
  6. Angus, Patricia M.; Jackson, W. Gregory (1994). "Linkage Isomerism in Cobalt(III) Pentaammine Complexes of 2-Pyridone". Inorganic Chemistry. 33 (3): 477–483. doi:10.1021/ic00081a014.
  7. Becker C. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Radiologe. 2007 Sep;47(9):768-73.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.