Sodium perchlorate
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| Other names
Sodium chlorate(VII)
Sodium hyperchlorate Perchloric acid, sodium salt | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| ECHA InfoCard | 100.028.647 |
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PubChem CID
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| RTECS number |
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| 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)
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1.4617 |
| Structure | |
| orthorhombic | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | 400 °C (752 °F; 673 K) |
| Safety data sheet (SDS) | ICSC 0715 |
| Related compounds | |
Other anions
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Sodium chloride Sodium hypochlorite Sodium chlorite Sodium chlorate |
Other cations
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Lithium perchlorate Potassium perchlorate Ammonium perchlorate Caesium perchlorate |
Related compounds
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Perchloric acid |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium perchlorate is the inorganic compound with the chemical formula NaClO4. It is the most soluble of the common perchlorate salts. It is a white crystalline, hygroscopic solid that is highly soluble in water and in alcohol. It usually comes as the monohydrate, which has a rhombic crystal system.[1]
Its heat of formation is −382.75 kJ/mol, meaning that it would be thermodynamically favorable for it to decompose into sodium chloride and dioxygen.[2]
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.
NaClO4 finds only minimal use in pyrotechnics because it is hygroscopic; ammonium and potassium perchlorates are preferred. These salts are prepared by double decomposition from a solution of sodium perchlorate and potassium or ammonium chlorides.
Laboratory applications
NaClO4 has a variety of uses in the laboratory, often as an unreactive electrolyte. For example, 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).[3]
In animal training
Sodium perchlorate may also be used as a material to train canines to detect bomb materials.[4]
Production
Sodium perchlorate is produced by anodic oxidation of sodium chlorate at an inert electrode, such as platinum.[5]
ClO3−(aq) + H2O(l) → ClO4−(aq) + 2H+(aq) + 2e- (acidic medium)
ClO3−(aq) + 2OH-(aq) → ClO4−(aq)+ H2O(l) + 2e- (alkaline medium)
See also
References
- ^ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 9783110114515. Retrieved March 7, 2013.
- ^ WebBook page for NaClO4
- ^ Becker C. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Radiologe. 2007 Sep;47(9):768-73.
- ^ "Explosives Detection Dogs". www.special-dogs.de (in German). Retrieved 2017-07-24.
- ^ Helmut Vogt, Jan Balej, John E. Bennett, Peter Wintzer, Saeed Akbar Sheikh, Patrizio Gallone "Chlorine Oxides and Chlorine Oxygen Acids" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH. doi:10.1002/14356007.a06_483