Chemistry:Sodium stannate
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| Names | |
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| IUPAC name
Sodium hexahydroxostannate(IV)
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| Other names
disodium hexahydroxyltin
Sodium stannate(IV) sodium stannate–3–water sodium tin(IV) oxide hydrate | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
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PubChem CID
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| Properties | |
| H6Na2O6Sn | |
| Molar mass | 266.73 g/mol |
| Appearance | Colorless or white solid |
| Density | 4.68 g/cm3 |
| Boiling point | N/A |
| Hazards | |
| Safety data sheet | [1][1] |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H314, H315, H319, H335, H412 | |
| P260, P261, P264, P271, P273, P280, P301+330+331, P302+352, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P332+313, P337+313, P362, P363, P403+233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | 57 °C (135 °F; 330 K) |
| N/A | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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2132 mg/kg [Mouse] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium stannate, formally sodium hexahydroxostannate(IV), is the inorganic compound with the formula Na2[Sn(OH)6]. This colourless salt forms upon dissolving metallic tin or tin(IV) oxide in sodium hydroxide, and is used as a stabiliser for hydrogen peroxide.[2] In older literature, stannates are sometimes represented as having the simple oxyanion SnO32−,[3] in which case this compound is sometimes named as sodium stannate–3–water and represented as Na2SnO3·3H2O, a hydrate with three waters of crystallisation.[1] The anhydrous form of sodium stannate, Na2SnO3, is recognised as a distinct compound with its own CAS Registry Number,[4] 12058-66-1 , and a distinct material safety data sheet.[5]
Alkali metal stannate compounds are prepared by dissolving elemental tin in a suitable metal hydroxide, in the case of sodium stannate by the reaction:[6]
- Sn + 2 NaOH + 4 H2O → Na2[Sn(OH)6] + 2 H2
A similar reaction occurs when tin dioxide is dissolved in base:
- SnO2 + 2 NaOH + 2 H2O → Na2[Sn(OH)6]
The anhydrous form can also be prepared from tin dioxide by roasting with sodium carbonate in a mixed carbon monoxide / carbon dioxide environment:[7]
- SnO2 + Na2CO3 → Na2SnO3 + CO2
The anion is a coordination complex that is octahedral in shape, similar to most stannates, such as the hexachlorostannate anion [SnCl6]2−. The Sn—O bond distances average 2.071 Å.[8]
See also
References
- ↑ 1.0 1.1 "Material Safety Data Sheet – sodium stannate trihydrate MSDS". Science Lab. 21 May 2013. http://www.sciencelab.com/msds.php?msdsId=9925038.
- ↑ Clark, John D. (1972). Ignition! An Informal History of Liquid Rocket Propellants. Rutgers University Press. ISBN 0813507251.
- ↑ Similarly, stannites are sometimes represented with the anion SnO22−
- ↑ National Center for Biotechnology Information (2017). "Sodium Stannate". PubChem. https://pubchem.ncbi.nlm.nih.gov/compound/Sodium_stannate#section=Molecular-Formula.
- ↑ "Sodium Stannate MSDS". Santa Cruz Biotechnology. 14 June 2011. http://datasheets.scbt.com/sc-229318.pdf.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0750633654.
- ↑ Zhang, Yuanbo; Su, Zijian; Liu, Bingbing; You, Zhixiong; Yang, Guang; Li, Guanghui; Jiang, Tao (2014). "Sodium stannate preparation from stannic oxide by a novel soda roasting–leaching process". Hydrometallurgy 146: 82–88. doi:10.1016/j.hydromet.2014.03.008. Bibcode: 2014HydMe.146...82Z.
- ↑ Jacobs, Herbert; Stahl, Rainer (2000). "Neubestimmung der Kristallstrukturen der Hexahydroxometallate Na2Sn(OH)6, K2Sn(OH)6 und K2Pb(OH)6" (in German). Z. Anorg. Allg. Chem. 626 (9): 1863–1866. doi:10.1002/1521-3749(200009)626:9<1863::AID-ZAAC1863>3.0.CO;2-M.
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