Chemistry:Sodium sulfite

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Sodium sulphite
Sodium sulfite
Sodium-sulfite-xtal-3x3x3-c-3D-bs-17.png
Sodium sulfite.jpg
anhydrous
Sodium sulfite hydrate.jpg
hydrate
Names
IUPAC name
Sodium sulfite
Other names
Hypo clear (photography)
E221
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
EC Number
  • 231-821-4
RTECS number
  • WE2150000
UNII
Properties
Na2SO3
Molar mass 126.043 g/mol
Appearance White solid
Odor Odorless
Density 2.633 g/cm3 (anhydrous)
1.561 g/cm3 (heptahydrate)
Melting point 33.4 °C (92.1 °F; 306.5 K) (dehydration of heptahydrate)
500 °C (anhydrous)
Boiling point Decomposes
27.0 g/100mL water (20 °C)
Solubility Soluble in glycerol
Insoluble in ammonia, chlorine
log P −4
Acidity (pKa) ~9 (heptahydrate)
1.565
Structure
Hexagonal (anhydrous)
Monoclinic (heptahydrate)
Hazards
Safety data sheet ICSC 1200
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 codeNFPA 704 four-colored diamond
0
2
0
Flash point Non-flammable
Related compounds
Other anions
Sodium selenite
Other cations
Potassium sulfite
Related compounds
Sodium bisulfite
Sodium metabisulfite
Sodium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Sodium sulfite (sodium sulphite) is the inorganic compound with the chemical formula Na2SO3. A white, water-soluble solid, it is used commercially as an antioxidant and preservative. A heptahydrate is also known but it is less useful because of its greater susceptibility toward oxidation by air.[1]

Preparation

Sodium sulfite can be prepared by treating a solution of sodium hydroxide with sulfur dioxide. When conducted in warm water, Na2SO3 initially precipitates as a white solid. With more SO2, the solid dissolves to give the disulfite, which crystallizes upon cooling.[1]

[math]\ce{ SO2 + 2 NaOH -> Na2SO3 + H2O }[/math]

Sodium sulfite is made industrially by treating sulfur dioxide with a solution of sodium carbonate.[2] The overall reaction is:

[math]\ce{ SO2 + Na2CO3 -> Na2SO3 + CO2 }[/math]

Applications

Sodium sulfite is primarily used in the pulp and paper industry.[3] It has been also applied in the thermomechanical conversion of wood to fibres (defibration) for producing medium density fibreboards (MDF).[4]

As an oxygen scavenger agent, it is used to treat water being fed to steam boilers to avoid corrosion problems,[5] in the photographic industry, it protects developer solutions from oxidation and (as hypo clear solution) to wash fixer (sodium thiosulfate) from film and photo-paper emulsions.

As a reducing agent it is used in the textile industry as a bleaching, desulfurizing, and dechlorinating agent (e.g. in swimming pools). Its reducing properties are exploited in its use as a preservative to prevent dried fruit from discoloring, and for preserving meats.

It is used as a reagent in sulfonation and sulfomethylation agent. It is used in the production of sodium thiosulfate.

The Wellman–Lord process utilizes sodium sulfite for flue gas desulfurization

Reactions

Main page: Chemistry:Sulfite

Sodium sulfite is primarily used as a mild reducing agent. The heptahydrate crystals effloresce in warm dry air. Heptahydrate crystals also oxidize in air to form sodium sulfate. The anhydrous form is more resistant to oxidation by air.[6]

Sodium bisulfite, NaHSO3, is mixture of salts that dissolve in water to give solutions composed of sodium and bisulfite ions.

Structure

According to X-ray crystallography sodium sulfite heptahydrate features pyramidal SO32- centers. The S-O distances are 1.50 and the O-S-O angles are near 106º.[7]

References

  1. 1.0 1.1 Johnstone, H. F. (1946). "Sulfites and Pyrosulfites of the Alkali Metals". Inorganic Syntheses. Inorganic Syntheses. 2. pp. 162–167. doi:10.1002/9780470132333.ch49. ISBN 9780470132333. 
  2. Weil, Edward D.; Sandler, Stanley R. (1999). "Sulfur Compounds". in Kroschwitz, Jacqueline I.. Kirk-Othmer Concise Encyclopedia of Chemical Technology (4th ed.). New York: John Wiley & Sons, Inc.. p. 1937. ISBN 978-0471419617. 
  3. Barberá, José Jiménez; Metzger, Adolf; Wolf, Manfred (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_477. 
  4. "DE19958756A1 - Production of light-colored medium-density fibreboard (MDF) from old fibreboard comprises treatment with sodium sulfite, conversion into pulp and feeding into the blow-line of an MDF plant". 1999-12-07. https://patents.google.com/patent/DE19958756A1/en. 
  5. "Pre-boiler and Boiler Corrosion Control | GE Water". http://www.gewater.com/handbook/boiler_water_systems/ch_11_preboiler.jsp. 
  6. Merck Index of Chemicals and Drugs, 9th ed. monograph 8451
  7. Larsson, Lars Olof; Kierkegaard, Peder; Lindberg, Bengt; Holme, Tord; Lindberg, Alf A.; Craig, J. Cymerman (1969). "The Crystal Structure of Sodium Sulphite. A Refinement Allowing for the Effect of Crystal Twinning". Acta Chemica Scandinavica 23: 2253–2260. doi:10.3891/acta.chem.scand.23-2253.