Sodium perchlorate

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Sodium perchlorate
Sodium perchlorte
Sodium perchlorte
Names
Other names
  • Perchloric acid, sodium salt
  • Sodium chlorate(VII)
  • Sodium hyperchlorate
Identifiers
3D model (
JSmol
)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard
 100.028.647 Edit this at Wikidata
EC Number
  • 231-511-9
RTECS number
  • SC9800000
UNII
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
SMILES
  • [Na+].[O-]Cl(=O)(=O)=O
Properties
NaClO4 (anhydrous)
NaClO4·H2O (monohydrate)
Molar mass 122.44 g/mol (anhydrous)
140.45 g/mol (monohydrate)
Appearance White crystalline solid
Density 2.4994 g/cm3 (anhydrous)
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
Thermochemistry
Std enthalpy of
formation
(ΔfH⦵298)
 −382.75 kJ/mol
Hazards
GHS labelling:
GHS03: Oxidizing GHS07: Exclamation mark GHS08: Health hazard
Danger
H271, H302, H319, H373
P102, P220, P305+P351+P338, P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2
0
1
OX
Flash point 400 °C (752 °F; 673 K)
Safety data sheet (SDS) ICSC 0715
Related compounds
Other anions
Other cations
Related compounds
 Perchloric acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Sodium perchlorate is an

monohydrate NaClO4·H2O. The compound is noteworthy as the most water-soluble of the common perchlorate
salts.

Sodium perchlorate and other perchlorates has been found on the planet Mars, first detected by the NASA probe Phoenix in 2009. This was later confirmed by spectral analysis by the Mars Reconnaissance Orbiter in 2015 of what is thought to be brine seeps which may be the first evidence of flowing liquid water containing hydrated salts on Mars.[1][2]

Selected properties

Its heat of formation is −382.75 kJ/mol, i.e. it is thermally stable up to high temperatures. At 490 °C it undergoes thermal decomposition, producing

dioxygen.[3]
It crystallizes in the rhombic crystal system.[4]

Uses

Perchloric acid is made by treating NaClO4 with HCl.[5] Ammonium perchlorate and potassium perchlorate, of interest in rocketry and pyrotechnics, are prepared by double decomposition from a solution of sodium perchlorate and ammonium chloride or potassium chloride, respectively.

Laboratory applications

Because of its high

anion. It is also a non-complexing anion with a fairly low ligand
binding capacity.

In the past perchlorates were quite widely used in the synthesis of coordination compounds because their larger size (compared to halides) and excellent

hydrogen bonding
abilities made them highly effective counter-ions for complexes with ammine, aquo and halido ligands, often yielding highly crystalline products. However because of the hazards (see Safety Section below) associated with their use they have been largely superseded in most labs by much less risky counterions like fluoroborate (BF4–, PF6– and related anions.

Sodium perchlorate is the precursor to ammonium, potassium and lithium perchlorate salts, often taking advantage of their low solubility in water relative to NaClO4 (209 g/(100 mL) at 25 °C).[6]

It is used for denaturating proteins in biochemistry and 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).[7]

Production

Sodium perchlorate is produced by

anodic oxidation of sodium chlorate (NaClO3) at an inert electrode, such as platinum.[5]

Na+ClO−3 + H2O → Na+ClO−4 + 2 H+ + 2 e− (
acidic
medium)
Na+ClO−3 + 2 OH− → Na+ClO−4 + H2O + 2 e− (
alkaline
medium)

Safety

All perchlorates are potent oxidisers. When mixed with organic compounds extreme combustion reactions can result, hence the use of such materials in fireworks, low tech rocket propellants and improvised explosives. Because of their kinetic inertness mixtures of perchlorate with organic compounds can ignite/detonate spontaneously and be shock sensitive.

Acute toxicity: The median lethal dose (LD50) is 2 – 4 g/kg (rabbits, oral).[5]

Chronic toxicity: The frequent consumption of

ppb) of perchlorate is harmful for the thyroid gland as the perchlorate anion competes with the uptake of iodide
severely disrupting thyroid function.

Environmental effects: Perchlorate anions are regarded as persistent pollutants that can cause long term contamination of drinking water and NaClO4's high solubility makes it highly mobile in the environment. Significant concerns have been raised about the environmental impacts of perchlorates because of its ability to disrupt iodide uptake and metabolism.[8]

See also

References

  1. PMID 28684729
    .
  2. ^ Delbecq, Denis (September 28, 2015). "De l'eau liquide répérée sur les pentes martiennes" [Liquid water spotted on Martian slopes]. Le Temps (in French). Archived from the original on January 18, 2017. Retrieved August 23, 2021.
  3. doi:10.1016/0168-7336(87)80019- (inactive 1 November 2024). Retrieved 3 May 2023.{{cite journal}}: CS1 maint: DOI inactive as of November 2024 (link
    )
  4. ISBN 978-3-11-011451-5
    . Retrieved March 7, 2013.
  5. ^
    ISBN 3-527-30673-0
    .
  6. doi:10.1021/ic00081a014
    .
  7. doi:10.1007/s00117-007-1550-4
  8. PMID 25004859
    .
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