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Sodium perchlorate

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Sodium perchlorate
Sodium perchlorte
Names
Other names
Sodium chlorate(VII)
Sodium hyperchlorate
Perchloric acid, sodium salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.647 Edit this at Wikidata
EC Number
  • 231-511-9
RTECS number
  • SC9800000
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
NaClO4.H2O (monohydrate)
Molar mass 122.44 g/mol
Appearance White crystalline solid
Density 2.4994 g/cm3
Melting point 130 °C (monohydrate)
>400 °C (decomp.)
209.6 g/100 ml at 25 °C
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Sodium perchlorate is the inorganic compound with the 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.[1]

Its heat of formation is −382.75 kJ mol−1.[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 a nonreactive electrolyte. For example, it is used in standard DNA extraction and hybridization reactions in molecular biology.


Production

Sodium perchlorate is produced by anodic oxidation of sodium chlorate, not sodium chloride, at a platinum electrode.[3]

ClO3− + H2O → ClO4− + H2

See also

References

  1. ^ Lange's
  2. ^ WebBook page for NaClO4
  3. ^ 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
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