Sodium stannate

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]

Sodium stannate
Names
IUPAC name
Sodium hexahydroxostannate(IV)
Other names
disodium hexahydroxyltin
Sodium stannate(IV)
sodium stannate–3–water
sodium tin(IV) oxide hydrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.554
EC Number
  • 234-724-5
UNII
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]
GHS pictograms
GHS Signal word Danger
H314, H315, H318, 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)
Flammability code 0: Will not burn. E.g. waterHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
2
0
Flash point 57 °C (135 °F; 330 K)
N/A
Lethal dose or concentration (LD, LC):
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

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]

References
  1. "Material Safety Data Sheet – sodium stannate trihydrate MSDS". Science Lab. 21 May 2013. Retrieved 1 June 2017.
  2. Clark, John D. (1972). Ignition! An Informal History of Liquid Rocket Propellants. Rutgers University Press. ISBN 0813507251.
  3. Similarly, stannites are sometimes represented with the anion SnO22−
  4. National Center for Biotechnology Information (2017). "Sodium Stannate". PubChem. Retrieved 1 June 2017.
  5. "Sodium Stannate MSDS" (PDF). Santa Cruz Biotechnology. 14 June 2011. Retrieved 1 June 2017.
  6. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0750633654.
  7. 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.
  8. Jacobs, Herbert; Stahl, Rainer (2000). "Neubestimmung der Kristallstrukturen der Hexahydroxometallate Na2Sn(OH)6, K2Sn(OH)6 und K2Pb(OH)6". Z. Anorg. Allg. Chem. (in German). 626 (9): 1863–1866. doi:10.1002/1521-3749(200009)626:9<1863::AID-ZAAC1863>3.0.CO;2-M.
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