Sodium stannate

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Sodium stannate
White powder of sodium stannate
IUPAC name
Sodium hexahydoxostannate(IV)
Other names
disodium hexahydroxyltin
Sodium stannate(IV)
sodium stannate–3–water
sodium tin(IV) oxide hydrate
ECHA InfoCard 100.031.554
Molar mass 266.73 g/mol
Appearance Colorless or white solid
Density 4.68 g/cm3
Boiling point N/A
Safety data sheet [1][1]
H300 + H310 + H330 + H410
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point 57 °C (135 °F; 330 K)
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

Sodium stannate, formally sodium hexahydoxostannate(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 materials 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]


  1. ^ a b "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.