Sodium perchlorate

Sodium perchlorate
Names
	Other names Perchloric acid, sodium salt; Sodium chlorate(VII); Sodium hyperchlorate;
Identifiers
CAS Number	7601-89-0 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:132103 ;
ChEMBL	ChEMBL1644700 ;
ChemSpider	22668 ;
ECHA InfoCard	100.028.647
EC Number	231-511-9;
PubChem CID	522606;
RTECS number	SC9800000;
UNII	97F4MTY3VA ;
UN number	1502
CompTox Dashboard (EPA)	DTXSID1034185 ;
	InChI InChI=1S/ClHO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Key: BAZAXWOYCMUHIX-UHFFFAOYSA-M ; InChI=1/ClHO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Key: BAZAXWOYCMUHIX-REWHXWOFAU;
	SMILES [Na+].[O-]Cl(=O)(=O)=O;
Properties
Chemical formula	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)
Solubility in water	209.6 g/(100 mL) (25 °C, anhydrous) ; 209 g/(100 mL) (15 °C, monohydrate)
Refractive index (nD)	1.4617
Structure
Crystal structure	orthorhombic
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H271, H302, H319, H373
Precautionary statements	P102, P220, P305+P351+P338, P338
NFPA 704 (fire diamond)	2 0 1 OX
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; Rubidium perchlorate; Caesium perchlorate; Ammonium 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). verify (what is ?) Infobox references

Sodium perchlorate is an inorganic compound with the chemical formula Na Cl O₄. 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 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

Because of its high solubility (2096 g/L at 25 °C) and the inert behaviour of dissolved perchlorate, solutions of NaClO₄ are often used as unreactive background electrolyte (supporting electrolyte). Indeed, because the reduction reaction of perchlorate is kinetically limited even if it is a thermodynamically unstable compound, perchlorate is a redox non-sensitive anion. It is also a non-complexing anion with no ligand binding capacity.

Sodium perchlorate is the precursor to ammonium, potassium and lithium perchlorate salts, often taking advantage of their low solubility relative to NaClO₄ (209 g/(100 mL) at 25 °C).^[6]

It is used for denaturating proteins in biochemistry and 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

Acute toxicity: The median lethal dose (LD₅₀) is 2 – 4 g/kg (rabbits, oral).^[5]

Chronic toxicity: The frequent consumption of drinking water with low concentrations (in the range of μg/L, ppb) of perchlorate is harmful for the thyroid gland as the perchlorate anion competes with the uptake of iodide.

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 2024-09-12). Retrieved 3 May 2023.{{cite journal}}: CS1 maint: DOI inactive as of September 2024 (link)
^ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 978-3-11-011451-5. Retrieved March 7, 2013.
^ ^a ^b ^c 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.
^ 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.
^ Becker, C. (2007, September). Radiologisch praxisrelevante prophylaxe und therapie von nebenwirkungen jodhaltiger kontrastmittel. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Der Radiologe. 47(9), 768–773. doi:10.1007/s00117-007-1550-4

External links

WebBook page for NaClO₄

[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 2024-09-12). Retrieved 3 May 2023.{{cite journal}}: CS1 maint: DOI inactive as of September 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.

[Ullmann-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. (2007, September). Radiologisch praxisrelevante prophylaxe und therapie von nebenwirkungen jodhaltiger kontrastmittel. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Der Radiologe. 47(9), 768–773. doi:10.1007/s00117-007-1550-4

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