Sodium silicate

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Sodium silicate
Names
IUPAC name
Sodium metasilicate
Other names
Liquid glass
Waterglass
Identifiers
6834-92-0 YesY
Abbreviations E550
ChEBI CHEBI:60720 YesY
ChemSpider 21758 YesY
EC Number 229-912-9
Jmol interactive 3D Image
MeSH Sodium+metasilicate
PubChem 23266
RTECS number VV9275000
UN number 3253
Properties
Na2SiO3
Appearance White to greenish opaque crystals
Density 2.61 g cm−3
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/mol K
113.71 J K−1 mol−1
−1561.43 kJ mol−1
-1427 kJ/mol
Hazards
Safety data sheet Avantor Performance Materials
C
R-phrases R34, R37
S-phrases (S1/2), S13, S24/25, S36/37/39, S45
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
0
2
0
Lethal dose or concentration (LD, LC):
1153 (rat, oral)
Related compounds
Other anions
 Sodium carbonate
Other cations
 Potassium silicate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
YesY verify (what is YesYN ?)
Infobox references

Sodium silicate is the common name for compounds with the formula Na2(SiO2)nO. A well-known member of this series is sodium metasilicate, Na2SiO3. Also known as waterglass or liquid glass, these materials are available in aqueous solution and in solid form. The pure compositions are colourless or white, but commercial samples are often greenish or blue owing to the presence of iron-containing impurities.

They are used in cements, passive fire protection, textile and lumber processing, refractories, and automobiles. Sodium carbonate and silicon dioxide react when molten to form sodium silicate and carbon dioxide:[1]

Na2CO3 + SiO2 → Na2SiO3 + CO2

Anhydrous sodium silicate contains a chain polymeric anion composed of corner-shared {SiO4} tetrahedral, and not a discrete SiO32− ion.[1] 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.[2]

In industry, the various grades of sodium silicate are characterized by their SiO2:Na2O weight ratio (weight ratios can be converted to molar ratios by multiplication with 1.032), which can vary between 2:1 and 3.75:1.[3] Grades with this ratio below 2.85:1 are termed alkaline. Those with a higher SiO2:Na2O ratio are described as neutral.

History

Water glass[4] was defined in Von Wagner's Manual of Chemical Technology (1892 translation) as any of the soluble alkaline silicates, first observed by Jean Baptist van Helmont circa 1640 as a fluid substance made by melting sand with excess alkali.[5][6] Glauber made what he termed "liquor silicum" in 1646 from potash and silica.[7] Johann Nepomuk von Fuchs, in 1818, obtained what is now known as water glass by treating silicic acid with an alkali, the result being soluble in water, "but not affected by atmospheric changes".[8][9] Von Wagner distinguished soda, potash, double (soda and potash), and fixing (i.e., stabilizing) as types of water glass. The fixing type was "a mixture of silica well saturated with potash water glass and a sodium silicate" used to stabilize inorganic water color pigments on cement work for outdoor signs and murals.

Properties

Sodium silicate is a white powder that is readily soluble in water, producing an alkaline solution. It is one of a number of related compounds which include sodium orthosilicate, Na4SiO4, sodium pyrosilicate, Na6Si2O7, and others. All are glassy, colourless, and soluble in water.

Sodium silicate is stable in neutral and alkaline solutions. In acidic solutions, the silicate ion reacts with hydrogen ions to form silicic acid, which when heated and roasted forms silica gel, a hard, glassy substance.

Production

Sodium silicate is commonly manufactured using a reaction in liquid phase or in solid phase. Both processes use alkaline and quartz sand as raw materials.

Liquid phase

A mixture of caustic soda, quartz sand, and water is prepared in a mixing tank, then fed into a reactor, where steam is introduced. The reaction is
n SiO2 + 2 NaOH → Na2O•nSiO2 + H2O

Solid phase (thermal process)

Sodium carbonate and sodium sulfate melt at temperatures far below that of silica. (<900°C vs >1600°C) Either is melted, and silica dissolved into the molten material, where it reacts to form sodium silicate.

Na2CO3 + x SiO2 → (Na2O)•(SiO2)x + CO2
2 Na2SO4 + C + 2 SiO2 → 2 Na2SiO3 + 2 SO2 + CO2

Uses

In 1990, 4M tons of alkali metal silicates were produced. The main applications were in detergents, paper, water treatment, and construction materials.[3]

Adhesive

The largest application of sodium silicate solutions is a cement for producing cardboard.[3] When used as a paper cement, the tendency is for the sodium silicate joint eventually to crack within a few years, at which point it no longer holds the paper surfaces cemented together.

Drilling fluids

Sodium silicate is frequently used in drilling fluids to stabilize borehole wells and to avoid the collapse of bore walls. It is particularly useful when drill holes pass through argillaceous formations containing swelling clay minerals such as smectite or montmorillonite.

Concrete and general masonry treatment

Concrete treated with a sodium silicate solution helps to significantly reduce porosity in most masonry products such as concrete, stucco, and plasters. A chemical reaction occurs with the excess Ca(OH)2 (portlandite) present in the concrete that permanently binds the silicates with the surface, making them far more durable and water repellent. This treatment generally is applied only after the initial cure has taken place (7 days or so depending on conditions). These coatings are known as silicate mineral paint.

Detergent auxiliaries

It is used in detergent auxiliaries such as complex sodium disilicate and modified sodium disilicate. The detergent granules gain their ruggedness from a coating of silicates.[3]

Water treatment

Water glass is used as coagulant/deflocculant agent in wastewater treatment plants. Waterglass binds to colloidal molecules, creating larger aggregates that sink to the bottom of the water column. The microscopic negatively charged particles suspended in water interact with sodium silicate. Their electrical double layer collapses due to the increase of ionic strength caused by the addition of sodium silicate (doubly negatively charged anion accompanied by two sodium cations) and they subsequently aggregate. This process is called coagulation/deflocculation.[3]

Refractory use

Water glass is a useful binder of solids, such as vermiculite and perlite. When blended with the aforementioned lightweight aggregates, water glass can be used to make hard, high-temperature insulation boards used for refractories, passive fire protection and high temperature insulations, such as moulded pipe insulation applications. When mixed with finely divided mineral powders, such as vermiculite dust (which is common scrap from the exfoliation process), one can produce high temperature adhesives. The intumescence disappears in the presence of finely divided mineral dust, whereby the waterglass becomes a mere matrix. Waterglass is inexpensive and abundantly available, which makes its use popular in many refractory applications.

Dye auxiliary

Sodium silicate solution is used as a fixative for hand dyeing with reactive dyes that require a high pH to react with the textile fiber. After the dye is applied to a cellulose-based fabric, such as cotton or rayon, or onto silk, it is allowed to dry, after which the sodium silicate is painted on to the dyed fabric, covered with plastic to retain moisture, and left to react for an hour at room temperature.[10]

Niche and hobby uses

Passive fire protection

Expantrol proprietary sodium silicate suspended in about a 6.5-mm-thick layer of red rubber, type 3M FS195, inserted into a metal pipe, then heated, to demonstrate hard char intumescence, strong enough to shut a melting plastic pipe
Palusol-based intumescent plastic pipe device used for commercial firestopping

Sodium silicates are inherently intumescent. They come in prill (solid beads) form, as well as the liquid, water glass. The solid sheet form (Palusol) must be waterproofed to ensure long-term passive fire protection (PFP).

Standard, solid, bead-form sodium silicates have been used as aggregate within silicone rubber to manufacture plastic pipe firestop devices. The silicone rubber was insufficient waterproofing to preserve the intumescing function and the products had to be recalled, which is problematic for firestops concealed behind drywall in buildings.

Pastes for caulking purposes are similarly unstable. This, too, has resulted in recalls and even litigation. Only 3M's "Expantrol" version, which has an external heat treatment that helps to seal the outer surface, as part of its process standard, has achieved sufficient longevity to qualify for DIBt approvals in the US for use in firestopping.

Not unlike other intumescents, sodium silicate, both in bead form and in liquid form, are inherently endothermic, due to liquid water in the water glass and hydrates in the prill form. The absence in the US of mandatory aging tests, whereby PFP systems are made to undergo system performance tests after the aging and humidity exposures, are at the root of the continued availability, in North America, of PFP products that can become inoperable within weeks of installation. Indiscriminate use of sodium silicates without proper waterproofing measures are contributors to the problems and risk. When sodium silicates are adequately protected, they function extremely well and reliably for long periods. Evidence of this can be seen in the many DIBt approvals for plastic pipe firestop devices using Palusol, which use waterproofed sodium silicate sheets.

Food preservation

World War I poster suggesting the use of waterglass to preserve eggs (lower right).

Sodium silicate was also used as an egg preservation agent through the early 20th century with large success. When fresh eggs are immersed in it, bacteria which cause the eggs to spoil are kept out and water is kept in. Eggs can be kept fresh using this method for up to five months. When boiling eggs preserved this way, it is well advised to pin-prick the egg to allow steam to escape because the shell is no longer porous.[11]

Metal repair

Sodium silicate is used, along with magnesium silicate, in muffler repair and fitting paste. When dissolved in water, both sodium silicate and magnesium silicate form a thick paste that is easy to apply. When the exhaust system of an internal combustion engine heats up to its operating temperature, the heat drives out all of the excess water from the paste. The silicate compounds that are left over have glass-like properties, making a temporary, brittle repair.

Automotive repair

Sodium silicate is also used currently as an exhaust system joint and crack sealer for repairing mufflers, resonators, tailpipes, and other exhaust components, with and without fiberglass reinforcing tapes. In this application, the sodium silicate (60-70%) is typically mixed with kaolin (40-30%), an aluminium silicate mineral, to make the sodium silicate "glued" joint opaque. The sodium silicate, however, is the high-temperature adhesive; the kaolin serves simply as a compatible high-temperature coloring agent. Some of these repair compounds also contain glass fibres to enhance their gap-filling abilities and reduce brittleness.

Sodium silicate can be used to fill gaps within the head gasket. Commonly used on aluminum alloy cylinder heads, which are sensitive to thermally induced surface deflection. This can be caused by many things including head-bolt stretching, deficient coolant delivery, high cylinder head pressure, overheating, etc.

"Liquid glass" (sodium silicate) is added to the system through the radiator, and allowed to circulate. Sodium silicate is suspended in the coolant until it reaches the cylinder head. At 100–105°C, sodium silicate loses water molecules to form a glass seal with a remelt temperature above 810°C.

A sodium silicate repair can last two years or longer. The repair occurs rapidly, and symptoms disappear instantly. This repair only works when the sodium silicate reaches its "conversion" temperature at 100–105°C. Contamination of engine oil is a serious possibility in situations in which a coolant-to-oil leak is present. Sodium silicate (glass particulate) contamination of lubricants is detrimental to their function.

Sodium silicate solution is used to inexpensively, quickly, and permanently disable automobile engines. Running an engine with about 2 liters of a sodium silicate solution instead of motor oil causes the solution to precipitate, catastrophically damaging the engine's bearings and pistons within a few minutes.[12] In the United States, this procedure was used to comply with requirements of the Car Allowance Rebate System (CARS) program.[12][13]

Homebrewing

Sodium silicate flocculant properties are also used to clarify wine and beer by precipitating colloidal particles. As a clearing agent, though, sodium silicate (water glass) is sometimes confused with isinglass which is prepared from collagen extracted from the dried swim bladders of sturgeon and other fishes. Eggs preserved in a bucket of waterglass gel, and their shells, are sometimes also used (baked and crushed) to clear wine.[14]

Aquaculture

Sodium silicate gel is also used as a substrate for algal growth in aquaculture hatcheries.

Safe construction

A mixture of sodium silicate and sawdust has been used in between the double skin of certain safes. This not only makes them more fire resistant, but also makes cutting them open with an oxyacetylene torch extremely difficult due to the smoke emitted.

Crystal gardens

When crystals of a number of metallic salts are dropped into a solution of water glass, simple or branching stalagmites of coloured metal silicates are formed. This phenomenon has been used by manufacturers of toys and chemistry sets to provide instructive enjoyment to many generations of children from the early 20th century until the present. An early mention of crystals of metallic salts forming a "chemical garden" in sodium silicate is found in the 1946 Modern Mechanix magazine.[15] Metal salts used included the sulfates and/or chlorides of copper, cobalt, iron, nickel, and manganese.

Pottery

Sodium silicate is used as a deflocculant in casting slips helping reduce viscosity and the need for large amounts of water to liquidize the clay body. It is also used to create a crackle effect in pottery, usually wheel-thrown. A vase or bottle is thrown on the wheel, fairly narrow and with thick walls. Sodium silicate is brushed on a section of the piece. After 5 minutes, the wall of the piece is stretched outward with a rib or hand. The result is a wrinkled or cracked look.

It is also the main agent in "magic water", which is used when joining clay pieces, especially if the moisture level of the two differs.[16]

Sealing of leaking water-containing structures

Sodium silicate with additives was injected into the ground to harden it and thereby to prevent further leakage of highly radioactive water from the Fukushima Daiichi nuclear power plant in Japan in April, 2011.[17] The residual heat carried by the water used for cooling the damaged reactors accelerated the setting of the injected mixture.

On June 3, 1958, the USS Nautilus, the world's first nuclear submarine, visited Everett and Seattle. In Seattle, crewmen dressed in civilian clothing were sent in to secretly buy 140 quarts of an automotive product containing sodium silicate (originally identified as Stop Leak) to repair a leaking condenser system. The Nautilus was en route to the North Pole on a top secret mission to cross the North Pole submerged.[18]

Cartridges

A historical use of the adhesive properties of sodium silicates is the production of paper cartridges for black powder revolvers produced by Colt's Manufacturing Company during the period from 1851 until 1873, especially during the American Civil War. Sodium silicate was used to seal combustible nitrated paper together to form a conical paper cartridge to hold the black powder, as well as to cement the lead ball or conical bullet into the open end of the paper cartridge. Such sodium silicate cemented paper cartridges were inserted into the cylinders of revolvers, thereby speeding the reloading of cap-and-ball black powder revolvers. This use largely ended with the introduction of Colt revolvers employing brass-cased cartridges starting in 1873.[19][20] Similarly, sodium silicate was also used to cement the top wad into brass shotgun shells, thereby eliminating any need for a crimp at the top of the brass shotgun shell to hold a shotgun shell together. Reloading brass shotgun shells was widely practiced by self-reliant American farmers during the 1870s, using the same waterglass material that was also used to preserve eggs. The cementing of the top wad on a shotgun shell consisted of applying from three to five drops of waterglass on the top wad to secure it to the brass hull. Brass hulls for shotgun shells were superseded by paper hulls starting around 1877. The newer paper-hulled shotgun shells used a roll crimp in place of a waterglass-cemented joint to hold the top wad in the shell. However, whereas brass shotshells with top wads cemented with waterglass could be reloaded nearly indefinitely (given powder, wad, and shot, of course), the paper hulls that replaced the brass hulls could be reloaded only a few times.

References

  1. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  2. ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  3. 1 2 3 4 5 Gerard Lagaly, Werner Tufar, A. Minihan, A. Lovell "Silicates" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, 2005. doi:10.1002/14356007.a23_661
  4. ↑ See also:
    • Leopold Wolff, Das Wasserglas: Seine Darstellung, Eigenschaften und seine mannichfache Anwendung in den technischen Gewerben [Water-glass: its preparation, properties, and its manifold uses in technical commerce] (Leipzig, (Germany): Quedlinburg, 1846).
    • Emile Kopp (1857) "Sur la préparation et les propriétés du verre soluble ou des silicates de potasse et de soude; analyse de tous les travaux publiés jusqu'a ce jour sur ce sujet" (On the preparation and properties of water-glass or the silicates of potash and soda; analysis of all works published until today on this subject) Le Moniteur scientifique, 1 : 337-349, 366-391.
    • Hermann Krätzer, Wasserglas und Infusorienerde, deren Natur und Bedeutung für Industrie, Technik und die Gewerbe [Water-glass and soluble earths, their nature and significance for industry, technology, and commerce] (Vienna (Wien), Austria: Hartleben, 1887).
    • Hermann Mayer, Das Wasserglas; Sein Eigenschaften, Fabrikation und Verwendung auf Grund von Erfahrungen und Mitteilungen der Firma Henkel & Cie. [Water-glass: Its properties, production, and application on the basis of experiences and communications of the firm of Henkel & Co.] (Braunschweig, Germany: Vieweg, 1925).
    • Morris Schrero, Water-glass: A Bibliography (Pittsburgh, Pennsylvania: Carnegie Library, 1922).
  5. ↑ Johannes van Helmont, Opuscula medica inaudita, (Cologne (Coloniæ Agrippinæ), (Germany): Jost Kalckhoven (Jodocum Kalcoven), 1644), part I: De Lithiasi. On page 53, van Helmont mentions that alkalis dissolve silicates: "Porro lapides, gemmae, arenae, marmora, silices, &c. adjuncto alcali, vitrificantur: sin autem plure alcali coquantur, resolvuntur in humido quidem: ac resoluta, facili negotio acidorum spirituum, separantur ab alcali, pondere pristini pulveris lapidum." (Furthermore, stone, gems, sand, marble, silica, etc., become glassy by the addition of alkali: but if roasted with more alkali, they are dissolved in moisture: and the former weight of the stone powder is separated from the alkali and released by simply adding acid.)
  6. ↑ A number of other alchemists supposedly discovered potassium silicate before van Helmont. See:
    • Giambattista della Porta in his book Magia naturalis sive de miraculis rerum naturalium (1567), mentions that cream of tartar (tartari salis) causes powdered quartz (crystallum) to melt at a lower temperature. See: Baptista Porta, Magia naturalis sive de miraculis rerum naturalium, libri iiii [Natural magic or on the miracles of nature, in four books] (Lyon (Lugdunum), France: Guillaume Rouillé (Gulielmum Rovillium), 1569), pages 290-291, "Crystallus, ut fusilis fiat" (quartz, so made molten).
    • Some evidence indicates the alchemist Basil Valentine prepared potassium silicate in 1520. See: Kohn, C. (1862) "Die Erfindung des Wasserglas im Jahre 1520" (The invention of waterglass in the year 1520), Zeitschrift des Oesterreichischen Ingenieur-Vereins (Journal of the Austrian Engineer Association), 14 : 229-230.
    However, subsequently an article pointed out that the substance prepared by Basil Valentine in 1520, by Agricola in 1550, by van Helmont around 1640, and by Glauber in 1648 was not the waterglass that Fuchs produced in 1818. See:
  7. ↑ Johann Rudolf Glauber, Furni Novi Philosophici [New philosophical furnace] (Amsterdam: Johan Jansson, 1646). In the 1661 German-language edition, see Chapter "LXXIX. Wie durch Hülff eines reinen Sandes oder Kißlings / auß Sale Tartari ein kräfftiger Spiritus kan erlanget werden." (How with the help of a pure sand or silica / a powerful solution can be gotten from cream of tartar). Glauber's recipe for liquor silicum (potassium silicate) appears on pages 164-166. The recipe is simple: Potassium hydrogen tartrate (cream of tartar, Sale tartari, Weinstein ) is heated in a furnace until it is converted to potassium carbonate. The potassium carbonate is mixed with sand in a crucible and heated until the mixture melts. The mixture is maintained in a liquid state until it ceases to bubble (due to the release of carbon dioxide from the potassium carbonate). The mixture is allowed to cool and then pulverized to a fine powder. When the powder is exposed to moist air, it gradually forms a viscous liquid, which Glauber called "Oleum oder Liquor Silicum, Arenæ, vel Crystallorum" (i.e., oil or solution of silica, sand or [quartz] crystal).
  8. ↑ See:
  9. ↑ VonWagner, Rudolf (1892 translation of 13th edition by Willian Crookes) Manual of Chemical Technology
  10. ↑ Burch, Paula (March 22, 2010). "Sodium silicate as a fixative for dyeing". Retrieved March 22, 2010.
  11. ↑ How To Store Fresh Eggs
  12. 1 2 Helliker, Kevin. "The Killer App for Clunkers Breathes Fresh Life Into 'Liquid Glass'" The Wall Street Journal, 4 August 2009.
  13. ↑ Engine Disablement Procedures for the CARS program, cars.gov
  14. ↑ SM Tritton (1956) Amateur wine making.
  15. ↑ "Magic garden". Mechanix Illustrated: 88. April 1946.
  16. ↑ http://lakesidepottery.com/HTML%20Text/Tips/pottery-magic-mud-magic-water-paper-clay.htm
  17. ↑ Daily Mail Reporter. "Liquid glass successfully plugs radioactive leak at crippled Fukushima nuclear plant", "Mail Online News", April 6, 2011, accessed April 7, 2010.
  18. ↑ Commander William R. Anderson with Clay Blair Jr., Nautilus 90 North (Cleveland and New York: The World Publishing Co., 1959), pp. 133-137; Commander William R. Anderson with Clay Blair Jr., Nautilus 90 North (New York: The New American Library, 1959), 89-90
  19. ↑ Tom Kelley (August 1995). "Making and using combustible paper pistol cartridges".
  20. ↑ Kirst, W.J. (1983). Self consuming paper cartridges for the percussion revolver. Minneapolis, Minnesota: Northwest Development Co.

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