|Jmol-3D images||Image 1|
|Molar mass||122.44 g/mol|
|Appearance||White crystalline solid|
2.02 g/cm3 (monohydrate)
|Melting point||468 °C (decomp., anhydrous)
130 °C (monohydrate)
|Boiling point||482 °C (decomp, monohydrate)|
|Solubility in water||209.6 g/100 mL (25 °C, anhydrous)
209 g/100 mL (15 °C, monohydrate)
|Refractive index (nD)||1.4617|
|EU classification||Oxidant (O)
|S-phrases||(S2), S13, S22, S27|
|Flash point||400 °C; 752 °F; 673 K|
|Other anions||Sodium chloride
|Other cations||Lithium perchlorate
|Related compounds||Perchloric acid|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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 structure.
Its heat of formation is −382.75 kJ mol−1.
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.
NaClO4 has a variety of uses in the laboratory, often as a nonreactive electrolyte. For example, it is used in standard DNA extraction and hybridization reactions in molecular biology.
- ClO3−(aq) + H2O(l) → ClO4−(aq) + H2(g)
- 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.
- 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