Sodium perchlorate

Sodium perchlorate
Names
Other names
Sodium chlorate(VII)
Sodium hyperchlorate
Perchloric acid, sodium salt
Identifiers
7601-89-0 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:132103 N
ChEMBL ChEMBL1644700 N
ChemSpider 22668 YesY
ECHA InfoCard 100.028.647
EC Number 231-511-9
PubChem 522606
RTECS number SC9800000
UN number 1502
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)
1.4617
Structure
orthorhombic
Hazards
Safety data sheet ICSC 0715
Oxidant (O)
Harmful (Xn)
R-phrases R9, R22
S-phrases (S2), S13, S22, S27
NFPA 704
Flash point 400 °C (752 °F; 673 K)
Related compounds
Other anions
 Sodium chloride
Sodium hypochlorite
Sodium chlorite
Sodium chlorate
Other cations
 Lithium perchlorate
Potassium perchlorate
Ammonium perchlorate
Caesium 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).
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Infobox references

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−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 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]

Production

Sodium perchlorate is produced by anodic oxidation of sodium chlorate at an inert electrode, such as platinum.[4]

ClO3−(aq) + H2O(l) → ClO4−(aq) + H2(g)

See also

References

  1. ↑ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 9783110114515. Retrieved March 7, 2013.
  2. ↑ WebBook page for NaClO4
  3. ↑ Becker C. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Radiologe. 2007 Sep;47(9):768-73.
  4. ↑ 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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