Sodium metasilicate

Sodium metasilicate is the chemical substance with formula Na
2SiO
3, which is the main component of commercial sodium silicate solutions. It is an ionic compound consisting of sodium cations Na+
 and the polymeric metasilicate anions [–SiO2−
3–]n. It is a colorless crystalline hygroscopic and deliquescent solid, soluble in water (giving an alkaline solution), but not in alcohols.[1]

Sodium metasilicate
Names
IUPAC name
Sodium metasilicate
Identifiers
3D model (JSmol)
Abbreviations E550
ChEBI
ChemSpider
ECHA InfoCard 100.027.193
EC Number
  • 600-279-4229-912-9
MeSH Sodium+metasilicate
RTECS number
  • VV9275000
UNII
UN number 1759 3253
Properties
Na2SiO3
Molar mass 122.062 g·mol−1
Appearance White crystals
Density 2.61 g/cm3
Melting point 1,088 °C (1,990 °F; 1,361 K)
22.2 g/100 ml (25 °C)
160.6 g/100 ml (80 °C)
Solubility insoluble in alcohol
1.52
Thermochemistry
111.8 J/(K·mol)
113.71 J/(K·mol)
Std enthalpy of
formation (ΔfH⦵298)
 −1561.43 kJ/mol
−1427 kJ/mol
Hazards
Safety data sheet Avantor Performance Materials
GHS pictograms
GHS Signal word Danger
GHS hazard statements
 H302, H314, H315, H318, H319, H335
P260, P261, P264, P270, P271, P280, P301+312, P301+330+331, P302+352, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P330, 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
Lethal dose or concentration (LD, LC):
1153 (rat, oral)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is YN ?)
Infobox references

Preparation and properties

The anhydrous compound can be prepared by fusing silicon dioxide SiO
2 (silica, quartz) with sodium oxide Na
2O in 1:1 molar ratio.[2]

The compound crystallizes from solution as various hydrates, such as

  • pentahydrate Na
    2    SiO
    3    ·5H
    2    O     (CAS 10213-79-3, EC 229-912-9, PubChem, 57652358)
  • nonahydrate Na
    2    SiO
    3    ·9H
    2    O     (CAS 13517-24-3, EC 229-912-9, PubChem 57654617)[3]

Structure

In the anhydrous solid, the metasilicate anion is actually polymeric, consisting of corner-shared {SiO4} tetrahedra, and not a discrete SiO32− ion.[4]

In addition to the anhydrous form, there are hydrates with the formula Na2SiO3·nH2O (where n = 5, 6, 8, 9), which contain the discrete, approximately tetrahedral anion SiO2(OH)22− with water of hydration. For example, the commercially available sodium silicate pentahydrate Na2SiO3·5H2O is formulated as Na2SiO2(OH)2·4H2O, and the nonahydrate Na2SiO3·9H2O is formulated as Na2SiO2(OH)2·8H2O.[5] The pentahydrate and nonahydrate forms have their own CAS Numbers, 10213-79-3 and 13517-24-3 respectively.

Uses

Sodium Metasilicate reacts with acids to produce silica gel.[6]

  • Cements and Binders - dehydrated sodium metasilicate forms cement or binding agent.
  • Pulp and Paper - sizing agent and buffer/stabilizing agent when mixed with hydrogen peroxide.
  • Soaps and Detergents - as an emulsifying and suspension agent.
  • Automotive applications - decommissioning of old engines (CARS program), cooling system sealant, exhaust repair.
  • Egg Preservative - seals eggs increasing shelf life.
  • Crafts - forms "stalagmites" by reacting with and precipitating metal ions.

See also

References
  1. Chemical Book: "Sodium metasilicate". Accessed on 2018-05-13.
  2. J. F. Schairer and N. L. Bowen (1956): "The system Na
    2    O    —Al
    2    O
    3    —SiO
    2    ". American Journal of Science, volume 254, issue 3, pages 129-195 doi:10.2475/ajs.254.3.129
  3. M. F. Bechtold (1955): "Polymerization and Properties of Dilute Aqueous Silicic Acid from Cation Exchange" Journal of Physical Chemistry, volume 59, issue 6, pages 532–541. doi:10.1021/j150528a013
  4. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  5. Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  6. https://sciencing.com/uses-sodium-metasilicate-5447484.html
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