Sodium perchlorate

Sodium perchlorate is the inorganic compound with the chemical formula NaClO4. It is a white crystalline, hygroscopic solid that is highly soluble in water and in alcohol. It is usually encountered as the monohydrate. The compound is noteworthy as the most water-soluble of the common perchlorate salts.

Sodium perchlorate
Names
Other names
Sodium chlorate(VII)
Sodium hyperchlorate
Perchloric acid, sodium salt
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.647
EC Number
  • 231-511-9
RTECS number
  • SC9800000
UNII
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
GHS pictograms
GHS Signal word Danger
GHS hazard statements
 H271, H302, H319, H373
P102, P220, P305+351+338, P338
NFPA 704 (fire diamond)
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 present on the planet Mars.[1]

Selected properties

Its heat of formation is −382.75 kJ/mol, i.e. it is favorable for it to decompose into sodium chloride and dioxygen.[2] It crystallizes in the rhombic crystal system.[3]

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.

Ammonium and potassium perchlorate, of interest in pyrotechnics, are prepared by double decomposition from a solution of sodium perchlorate and potassium or ammonium chlorides.

Laboratory applications

Solutions of NaClO4 are often used as an unreactive electrolyte. 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).[4]

In animal training

Sodium perchlorate may also be used as a material to train canines to detect bomb materials.[5]

Production

Sodium perchlorate is produced by anodic oxidation of sodium chlorate at an inert electrode, such as platinum.[6]

ClO3− + H2O → ClO4− + 2H+ + 2 e− (acidic medium)

ClO3− + 2 OH− → ClO4− + H2O + 2 e− (alkaline medium)

Safety

LD50 is 2 – 4 g/kg (rabbits, oral).[6]

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See also

References
  1. https://www.letemps.ch/sciences/2015/09/28/eau-liquide-reperee-pentes-martiennes
  2. WebBook page for NaClO4
  3. Eagleson, Mary (1994). Concise Encyclopedia Chemistry. revised, illustrated. Walter de Gruyter. p. 1000. ISBN 9783110114515. Retrieved March 7, 2013.
  4. Becker C. [Prophylaxis and treatment of side effects due to iodinated contrast media relevant to radiological practice]. Radiologe. 2007 Sep;47(9):768-73.
  5. "Explosives Detection Dogs". www.special-dogs.de (in German). Retrieved 2017-07-24.
  6. Helmut Vogt, Jan Balej, John E. Bennett, Peter Wintzer, Saeed Akbar Sheikh, Patrizio Gallone (2002). "Chlorine Oxides and Chlorine Oxygen Acids". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a06_483.CS1 maint: uses authors parameter (link)
Compounds containing perchlorate group
HClO4 He
LiClO4 Be(ClO4)2 B(ClO
4)−
4
B(ClO4)3		 ROClO3 N(ClO4)3
NH4ClO4
NOClO4		 O FClO4 Ne
NaClO4 Mg(ClO4)2 Al(ClO4)3 Si P S ClO−
4
ClOClO3
Cl2O7		 Ar
KClO4 Ca(ClO4)2 Sc(ClO4)3 Ti(ClO4)4 VO(ClO4)3
VO2(ClO4)		 Cr(ClO4)3 Mn(ClO4)2 Fe(ClO4)3 Co(ClO4)2,
Co(ClO4)3		 Ni(ClO4)2 Cu(ClO4)2 Zn(ClO4)2 Ga(ClO4)3 Ge As Se Br Kr
RbClO4 Sr(ClO4)2 Y(ClO4)3 Zr(ClO4)4 Nb(ClO4)5 Mo Tc Ru Rh(ClO4)3 Pd(ClO4)2 AgClO4 Cd(ClO4)2 In(ClO4)3 Sn(ClO4)4 Sb TeO(ClO4)2 I Xe
CsClO4 Ba(ClO4)2   Hf(ClO4)4 Ta(ClO4)5 W Re Os Ir Pt Au Hg2(ClO4)2,
Hg(ClO4)2		 Tl(ClO4),
Tl(ClO4)3		 Pb(ClO4)2 Bi(ClO4)3 Po At Rn
FrClO4 Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La Ce(ClO4)x Pr Nd Pm Sm(ClO4)3 Eu(ClO4)3 Gd(ClO4)3 Tb(ClO4)3 Dy(ClO4)3 Ho(ClO4)3 Er(ClO4)3 Tm(ClO4)3 Yb(ClO4)3 Lu(ClO4)3
Ac Th(ClO4)4 Pa UO2(ClO4)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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