Magnesium sulfite
Crystal structure | ||||||||||||||||
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
![]() ![]() |
||||||||||||||||
General | ||||||||||||||||
Surname | Magnesium sulfite | |||||||||||||||
Ratio formula | MgSO 3 | |||||||||||||||
Brief description |
white solid (hexahydrate) |
|||||||||||||||
External identifiers / databases | ||||||||||||||||
|
||||||||||||||||
properties | ||||||||||||||||
Molar mass | 104.37 g mol −1 | |||||||||||||||
Physical state |
firmly |
|||||||||||||||
density |
1.72 g cm −3 (hexahydrate) |
|||||||||||||||
safety instructions | ||||||||||||||||
|
||||||||||||||||
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Magnesium sulfite is an inorganic chemical compound of magnesium from the group of sulfites .
Extraction and presentation
Magnesium sulfite can be obtained by reacting magnesium hydroxide with sulfur dioxide , with the hexahydrate being formed at temperatures below 40 ° C and the trihydrate above.
It is also possible to display it by reacting sodium sulfite with magnesium chloride .
properties
Magnesium sulfite hexahydrate has a rhombohedral crystal structure with space group R 3 (space group no. 146) . The hexahydrate loses crystal water above 78 ° C and converts to the trihydrate. At 120 ° C for further reaction takes place dihydrate and at 395 ° C for anhydrate . The trihydrate has a tetragonal crystal structure with the space group P 4 1 2 1 2 (No. 92) , the dihydrate the monoclinic space group P 2 1 / c (No. 14) .
Formation during flue gas desulphurization
Magnesium sulphite is produced in systems for flue gas desulphurisation in which magnesium hydroxide is used as a washing alkali ( magnesium process ).
Individual evidence
- ^ A b c William M. Haynes: CRC Handbook of Chemistry and Physics, 93rd Edition . CRC Press, 2012, ISBN 1-4398-8049-2 , pp. 4–74 ( limited preview in Google Book Search).
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ↑ a b c Richard C. Ropp: Encyclopedia of the Alkaline Earth Compounds . Newnes, 2012, ISBN 0-444-59553-8 , pp. 143 ( limited preview in Google Book search).
- ^ Ulrich Förstner: Environmental protection technology . Springer DE, 2003, ISBN 3-540-44369-X , p. 150 ( limited preview in Google Book search).
- ^ Dale L. Perry: Handbook of Inorganic Compounds, Second Edition . Taylor & Francis US, 2011, ISBN 1-4398-1461-9 , pp. 258 ( limited preview in Google Book search).