Magnesium perchlorate

Magnesium perchlorate
Identifiers
CAS Number	10034-81-8 ; 64010-42-0 (hydrate) ; 13446-19-0 (hexahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	23223 ;
ECHA InfoCard	100.030.086
PubChem CID	24840;
RTECS number	SC8925000;
UNII	7N77Z541YF ;
CompTox Dashboard (EPA)	DTXSID70890617 ;
	InChI InChI=1S/2ClHO4.Mg/c22-1(3,4)5;/h2(H,2,3,4,5);/q;;+2/p-2 Key: MPCRDALPQLDDFX-UHFFFAOYSA-L ; InChI=1/2ClHO4.Mg/c22-1(3,4)5;/h2(H,2,3,4,5);/q;;+2/p-2 Key: MPCRDALPQLDDFX-NUQVWONBAH;
	SMILES [Mg+2].O=Cl(=O)(=O)[O-].[O-]Cl(=O)(=O)=O;
Properties
Chemical formula	Mg(ClO4)2
Molar mass	223.206 g/mol
Appearance	white powder, ; deliquescent
Odor	odorless
Density	2.21 g/cm3 (anhydrous) ; 1.98 g/cm3 (hexahydrate)
Melting point	251 °C (484 °F; 524 K) (anhydrous) ; 95-100 °C (hexahydrate)
Boiling point	decomposition
Solubility in water	99.3 g/100 mL
Solubility in ethanol	23.96 g/100 mL
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Oxidizer
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H315, H319, H335
Precautionary statements	P220, P261, P305+P351+P338
NFPA 704 (fire diamond)	1 0 0 OX
Safety data sheet (SDS)	External MSDS
Related compounds
Other cations	Calcium perchlorate; Barium perchlorate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Magnesium perchlorate is a powerful oxidizing agent, with the formula Mg(ClO₄)₂. The salt is also a superior drying agent for gas analysis.

Magnesium perchlorate decomposes at 250 °C.^[2] The heat of formation is -568.90 kJ/mol.^[3]

The enthalpy of solution is quite high, so reactions are done in large amounts of water to dilute it.

It is sold under the trade name anhydrone. Manufacture of this product on a semi-industrial scale was first performed by G. Frederick Smith in his garage in Urbana Illinois, but later at a permanent facility in Columbus, OH called G. Frederick Smith Chemical Co. He sold the magnesium perchlorate to A. H. Thomas Co., now Thomas Scientific, under the trade name Dehydrite.

Uses

It is used as desiccant to dry gas or air samples,^[4]^[5] but is no longer advised, for use as a general desiccant, due to hazards inherent in perchlorates.^[6] It is dried by heating at 220 °C under vacuum.

Magnesium perchlorate and other perchlorates have been found on Mars.^[7] Being a drying agent, magnesium perchlorate retains water from the atmosphere and may release it when conditions are favorable and temperature is above 273 K. Briny solutions that contain salts such as magnesium perchlorate have a lower melting point than that of pure water. Therefore the abundance of magnesium and other perchlorate salts on Mars could support the theory that liquid aqueous solutions might exist on or below the surface, where temperature and pressure conditions would ordinarily cause the water to freeze.

Production

Magnesium perchlorate is produced by the reaction of magnesium hydroxide and perchloric acid.

References

^ "Magnesium Perchlorate, Anhydrous". American Elements. Retrieved August 28, 2019.
^ "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (97th ed.). Taylor and Francis Group. 2016. pp. 4–72. Retrieved June 4, 2023.
^ Lange, Norbert Adolph; Dean, John Aurie (1992). "Thermodynamic properties". Lange's Handbook of Chemistry (14th ed.). McGraw-Hill. p. 6.85.
^ H. H. Willard, G. F. Smith (1922). "The Preparation and Properties of Magnesium Perchlorate and its Use as a Drying Agent". Journal of the American Chemical Society. 44 (10): 2255–2259. doi:10.1021/ja01431a022.
^ L. Wu, H. He (1994). "Preparation of perlite-based magnesium perchlorate desiccant with colour indicator". The Chemical Educator. 41 (5): 633–637. doi:10.1016/0039-9140(94)80041-3. PMID 18965975.
^ W. L. F. Armarego and C. Chai (2003). Purification of laboratory chemicals. Oxford: Butterworth-Heinemann. ISBN 0-7506-7571-3.
^ Hand, Eric (2008-08-06). "Perchlorate found on Mars". Nature: news.2008.1016. doi:10.1038/news.2008.1016. ISSN 0028-0836.

[1] "Magnesium Perchlorate, Anhydrous". American Elements. Retrieved August 28, 2019.

[RubberBible-2] "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (97th ed.). Taylor and Francis Group. 2016. pp. 4–72. Retrieved June 4, 2023.

[Lange's-3] Lange, Norbert Adolph; Dean, John Aurie (1992). "Thermodynamic properties". Lange's Handbook of Chemistry (14th ed.). McGraw-Hill. p. 6.85.

[4] H. H. Willard, G. F. Smith (1922). "The Preparation and Properties of Magnesium Perchlorate and its Use as a Drying Agent". Journal of the American Chemical Society. 44 (10): 2255–2259. doi:10.1021/ja01431a022.

[5] L. Wu, H. He (1994). "Preparation of perlite-based magnesium perchlorate desiccant with colour indicator". The Chemical Educator. 41 (5): 633–637. doi:10.1016/0039-9140(94)80041-3. PMID 18965975.

[6] W. L. F. Armarego and C. Chai (2003). Purification of laboratory chemicals. Oxford: Butterworth-Heinemann. ISBN 0-7506-7571-3.

[7] Hand, Eric (2008-08-06). "Perchlorate found on Mars". Nature: news.2008.1016. doi:10.1038/news.2008.1016. ISSN 0028-0836.

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Magnesium perchlorate

Uses

Production

References

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