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Sodium perchlorate

Sodium perchlorate
Other names Sodium Chlorate(VII),
Sodium Hyperchlorate,
Perchloric Acid Sodium Salt
Molecular formula NaClO4
Molar mass 122.44 g/mol
Appearance White Crystalline Solid
CAS number [7601-89-0]
Specific Gravity 2.02
Solubility in water Soluble, Hygroscopic in Air
Melting point 400 °C (Decomposes)
General Oxidizer.
Reacts with concentrated
sulfuric acid to produce
perchloric acid.
Related Compounds
Other anions Sodium chloride
Sodium chlorite
Sodium chlorate
Sodium hypochlorite
sodium sulfate
Other cations Lithium perchlorate
Calcium perchlorate
Potassium perchlorate
ammonium perchlorate
Related Compounds Perchloric acid
Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references

Sodium perchlorate is a perchlorate of sodium and has the formula NaClO4. Sodium perchlorate melts with decomposition at 480 °C.[1] Its heat of formation is -382.75 kJ mol-1.[2] It is a white crystalline solid. It is hygroscopic. It is soluble in water and in alcohol. It usually comes as the monohydrate, which has a rhombic crystal structure.



The present major use of perchlorate salts is as oxidizers in solid propellants such as NASA's solid rocket boosters. The potassium salt was first used and quickly followed by what is now the more important salt, ammonium perchlorate. Lithium perchlorate, which has the highest weight percentage of oxygen of all compounds, has been tested as an oxidizer in solid propellants, but has not found favor with propellant manufacturers due to its hygroscopicity.

Sodium perchlorate itself finds only minimal use in pyrotechnics because it is hygroscopic; ammonium and potassium perchlorates are preferred. They are made by double decomposition from a solution of sodium perchlorate and potassium or ammonium chlorides.


Sodium perchlorate is manufactured by anodic oxidation of sodium chloride or sodium chlorate at high current density, with platinum (or in some cases, lead dioxide, manganese dioxide, and possibly magnetite and cobalt oxide) anodes and graphite, steel, nickel, or titanium cathodes.[3]

See also


  1. ^ Lange's
  2. ^ WebBook page for NaClO4
  3. ^ Sodium Perchlorate
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Sodium_perchlorate". A list of authors is available in Wikipedia.
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