Chemistry:Magnesium perchlorate
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| Properties | |
| 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 |
| 99.3 g/100 mL | |
| Solubility in ethanol | 23.96 g/100 mL |
| Hazards[1] | |
| Main hazards | Oxidizer |
| Safety data sheet | External MSDS |
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| GHS Signal word | Danger |
| H272, H315, H319, H335 | |
| P220, P261, P305+351+338 | |
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Other cations
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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   ?)
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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. https://www.americanelements.com/magnesium-perchlorate-anhydrous-10034-81-8. Retrieved August 28, 2019.
- ↑ "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (97th ed.). Taylor and Francis Group. 2016. p. 4-72. https://archive.org/details/CRCHandbookOfChemistryAndPhysics97thEdition2016/page/n790. 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. https://archive.org/details/langeshandbookof00lang_0/page/n834.
- ↑ 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. https://zenodo.org/record/1428802.
- ↑ 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" (in en). Nature: news.2008.1016. doi:10.1038/news.2008.1016. ISSN 0028-0836. http://www.nature.com/articles/news.2008.1016.
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