Sodium fluorosilicate
Unit cell of sodium hexafluoridosilicate
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| Names | |
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| Preferred IUPAC name
Sodium fluorosilicate | |
| Systematic IUPAC name
Sodium hexafluoridosilicate(2–)
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| Other names
Disodium hexafluorosilicate/sodium fluosilicate/sodium silicofluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
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| EC Number |
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| E number | Lua error in Module:Wikidata at line 880: attempt to index field 'wikibase' (a nil value). |
PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 2674 |
CompTox Dashboard (EPA)
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| Properties | |
| Na2[SiF6] | |
| Molar mass | 188 g/mol |
| Appearance | white granular powder |
| Odor | odorless |
| Density | 2.7 g/cm3 |
| 0.64 g/100 mL (20 °C) 1.27 g/100 mL (50 °C) 2.45 g/100 mL (100 °C) | |
| Solubility | insoluble in alcohol |
Refractive index (nD)
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1.312 |
| Structure[2] | |
| trigonal | |
| P321 | |
a = 8.859, c = 5.038
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Formula units (Z)
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4 |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LDLo (lowest published)
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70 mg/kg (mouse, oral) 125 mg/kg (rabbit, oral)[3] |
| Related compounds | |
Other cations
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Ammonium hexafluorosilicate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium fluorosilicate is a compound with the chemical formula Na2[SiF6]. Unlike other sodium salts, it has a low solubility in water.
Natural occurrence
[edit | edit source]Sodium hexafluorosilicate occurs naturally as the rare mineral malladrite found within some volcanic fumaroles.[4]
Manufacturing
[edit | edit source]Sodium fluorosilicate is made by neutralizing fluorosilicic acid with sodium chloride or sodium sulfate.
- H2[SiF6] + 2 NaCl → Na2[SiF6] + 2 HCl
Possible application
[edit | edit source]Sodium fluorosilicate is used in some countries as additives for water fluoridation, opal glass raw material, ore refining, or other fluoride chemical (like sodium fluoride, magnesium silicofluoride, cryolite, aluminum fluoride) production.[5]
It is used for extraction of beryllium from beryl, by roasting the mineral with it at 700-750 °C, leaching the soluble fluoride with water, and then precipitating it as Be(OH)2 at about pH 13.[6]
It also is an ingredient in some ceramic cements.
See also
[edit | edit source]References
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