Sodium bisulfite
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| Names | |
|---|---|
| IUPAC name
Sodium hydrogen sulfite
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| Other names
E222
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| Identifiers | |
| ECHA InfoCard | 100.028.680 |
| E number | E222 (preservatives) |
PubChem CID
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| RTECS number |
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CompTox Dashboard (EPA)
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| Properties | |
| NaHSO3 | |
| Molar mass | 104.061 g/mol |
| Appearance | White solid |
| Density | 1.48 g/cm3 |
| Melting point | 150 °C (302 °F; 423 K) |
| 42 g/100 mL | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Sodium sulfite Sodium metabisulfite |
Other cations
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Potassium bisulfite |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium bisulfite (sodium hydrogen sulfite) is a chemical compound with the chemical formula NaHSO3. Sodium bisulfite is a food additive with E number E222. This salt of bisulfite can be prepared by bubbling sulfur dioxide in a solution of sodium carbonate in water. Sodium bisulfite in contact with chlorine bleach (aqueous solution of sodium hypochlorite) will release harmful fumes.
Uses in chemistry
In organic chemistry sodium bisulfite has several uses. It forms a bisulfite adduct with aldehyde groups and with certain cyclic ketones to a sulfonic acid.[1]
This reaction has limited synthetic value(s) but it is used in purification procedures. Contaminated aldehydes in a solution precipitate as the bisulfite adduct which can be isolated by filtration. The reverse reaction takes place in presence of a base such as sodium bicarbonate or sodium hydroxide and the bisulfite is liberated as sulfur dioxide.[2]
Examples of such procedures are described for benzaldehyde,[3] tetralone,[4] citral,[5] the ethyl ester of pyruvic acid[6] and glyoxal.[7] In the ring-expansion reaction of cyclohexanone with diazald, the bisulfite reaction is reported to be able to differentiate between the primary reaction product cycloheptanone and the main contaminant cyclooctanone.[8]
The other main use of sodium bisulfite is as a mild reducing agent in organic synthesis in particular in purification procedures. It can efficiently remove traces or excess amounts of chlorine, bromine, iodine, hypochlorite salts, osmate esters, chromium trioxide and potassium permanganate.
A third use of sodium bisulfite is as a decoloration agent in purification procedures because it can reduce strongly coloured oxidizing agents, conjugated alkenes and carbonyl compounds.
Sodium bisulfite is also the key ingredient in the Bucherer reaction. In this reaction an aromatic hydroxyl group is replaced by an aromatic amine group and vice versa because it is a reversible reaction. The first step in this reaction is an addition reaction of sodium bisulfite to an aromatic double bond. The Bucherer carbazole synthesis is a related organic reaction.
Uses in food
While the related compound, sodium metabisulfite, is used in almost all commercial wines to prevent oxidation and preserve flavor, sodium bisulfite is sold by some home winemaking suppliers for the same purpose.[9] In fruit canning, sodium bisulfite is used to prevent browning (caused by oxidation) and to kill microbes.
In the case of wine making, sodium bisulfite releases sulfur dioxide gas when added to water or products containing water. The sulfur dioxide kills yeasts, fungi, and bacteria in the grape juice before fermentation. When the sulfur dioxide levels have subsided (about 24 hours), fresh yeast is added for fermentation.
It is later added to bottled wine to prevent the formation of vinegar if bacteria are present, and to protect the color, aroma and flavor of the wine from oxidation, which causes browning and other chemical changes. The sulfur dioxide quickly reacts with oxidation by-products and prevents them from causing further deterioration.
Sodium bisulfite is also added to leafy green vegetables in salad bars and elsewhere, to preserve apparent freshness, under names like LeafGreen. The concentration is sometimes high enough to cause severe allergic reactions.[10]
In the 1980s, sodium bisulfite was banned from use on raw fruits and vegetables in the United States following the deaths of 13 people who unknowingly consumed produce treated with excessive amounts of the substance.[11]
Industrial uses
Sodium bisulfite is a common reducing agent in the chemical industries. As it readily reacts with dissolved oxygen:
- 2 NaHSO3 + O2 → 2 NaHSO4
It is usually added to large piping systems to prevent oxidative corrosion. In biochemical engineering applications, it is helpful to maintain anaerobic conditions within a reactor. Sodium bisulfite should not be confused with sodium bisulfate which is used as a pH lowering chemical for swimming pools.
In wastewater treatment, sodium bisufite is often added following disinfection with a chlorine solution to neutralize the residual chlorine before discharging the treated effluent.
Bisulfite DNA sequencing
Sodium bisulfite is used in the analysis of methylation status of cytosines in DNA.
In this technique, sodium bisulfite deaminates cytosine into uracil, but does not affect 5-methylcytosine, a methylated form of cytosine with a methyl group attached to carbon 5.
When the bisulfite-treated DNA is amplified via polymerase chain reaction, the uracil is amplified as thymine and the methylated cytosines are amplified as cytosine. DNA sequencing techniques are then used to read the sequence of the bisulfite-treated DNA. Those cytosines that are read as cytosines after sequencing represent methylated cytosines, while those that are read as thymines represent unmethylated cytosines in the genomic DNA.[12]
See also
References
- ^ Steven D. Young, Charles T. Buse, and Clayton H. Heathcock (1990). "2-Methyl-2-(Trimethylsiloxy)pentan-3-one". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 7, p. 381. - ^ S. A. Buntin and Richard F. Heck (1990). "2-Methyl-3-phenylpropanal". Organic Syntheses; Collected Volumes, vol. 7, p. 361.
- ^ Harold M. Taylor and Charles R. Hauser (1973). "α-(N,N-Dimethylamino)phenylacetonitrile". Organic Syntheses; Collected Volumes, vol. 5, p. 437.
- ^ M. D. Soffer, M. P. Bellis, Hilda E. Gellerson, and Roberta A. Stewart (1963). "β-Tetralone". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 4, p. 903. - ^ Alfred Russell and R. L. Kenyon (1955). "Pseudoionone". Organic Syntheses; Collected Volumes, vol. 3, p. 747.
- ^ J. W. Cornforth (1963). "Ethyl Pyruvate". Organic Syntheses; Collected Volumes, vol. 4, p. 467.
- ^ Anthony R. Ronzio and T. D. Waugh (1955). "Glyoxal Bisulfite". Organic Syntheses; Collected Volumes, vol. 3, p. 438.
- ^ Hyp J. Dauben, Jr., Howard J. Ringold, Robert H. Wade, David L. Pearson, and Arthur G. Anderson, Jr. "Cycloheptanone". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 4, p. 221. - ^ The Many Uses Of Sodium Bisulfite
- ^ Albertson, Timothy Eugene (2006). Bronchial Asthma: A Guide for Practical Understanding and Treatment (Current Clinical Practice) (fifth ed.). Totowa, NJ: Humana Press. pp. 260–266. ISBN 1-58829-872-8. Retrieved 2011-11-11.
- ^ van der Leun, Justine (July 2009). "What's In Your Food?". AOL Health. Retrieved August 2009.
{{cite web}}: Check date values in:|accessdate=(help) - ^ Frommer, M.; McDonald, L. E.; Millar, D. S.; Collis, C.M.; Watt, F.; Grigg, G.W.; Molloy P.L.; Paul, C.L. (1992). "A genomic sequencing protocol that yields a positive display of 5-methylcytosine residues in individual DNA strands" (free full text). PNAS. 89 (5): 1827–31. doi:10.1073/pnas.89.5.1827. PMC 48546. PMID 1542678.
{{cite journal}}: CS1 maint: multiple names: authors list (link)