Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Sodium bisulfite: Difference between pages

{{Distinguish|Sodium bisulfate}}

| Watchedfields = changed

| verifiedrevid = 477858271

| ImageFile2 = Hydrogensiřičitan sodný.jpg

| OtherNames = {{Unbulleted list|E222|sodium bisulphite}}

|Section1={{Chembox Identifiers

| CASNo = 7631-90-5

| CASNo_Ref = {{cascite|correct|CAS}}

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = TZX5469Z6I

| ChEBI_Ref = {{ebicite|correct|EBI}}

| ChEBI = 26709

| PubChem = 23665763

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChEMBL = 1689285

| SMILES = [Na+].[O-]S(=O)O

| InChI = 1/Na.H2O3S/c;1-4(2)3/h;(H2,1,2,3)/q+1;/p-1

| InChIKey = DWAQJAXMDSEUJJ-REWHXWOFAL

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| RTECS = VZ2000000

|Section2={{Chembox Properties

| Formula = NaHSO₃

| MolarMass = 104.061{{nbsp}}g/mol

| Appearance = White solid

| Odor = Slight sulfurous odor

| Density = 1.48{{nbsp}}g/cm³

| MeltingPtC = 150

| BoilingPtC = 315

| Solubility = 42{{nbsp}}g/100{{thinsp}}mL

| RefractIndex = 1.526

|Section7={{Chembox Hazards

| ExternalSDS =

| GHSPictograms = {{GHS07}}

| HPhrases = {{H-phrases|302}}

| PPhrases = {{P-phrases|301+312+330}}

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 1

| FlashPt = Non-flammable

| LD50 =

| IDLH = N.D.<ref name=PGCH>{{PGCH|0561}}</ref>

| PEL = none<ref name=PGCH/>

| REL = TWA 5{{nbsp}}mg/m³<ref name=PGCH/>

|Section8={{Chembox Related

| OtherAnions = [[Sodium sulfite]]<br/>[[Sodium metabisulfite]]<br/>[[Sodium biselenite]]

| OtherCations = [[Potassium bisulfite]]

'''Sodium bisulfite''' (or '''sodium bisulphite''', '''sodium hydrogen sulfite''') is a [[chemical]] mixture with the approximate [[chemical formula]] NaHSO₃. Sodium bisulfite is not a real compound,<ref>{{cite journal|doi=10.1021/ed080p1482|bibcode=2003JChEd..80.1482T|title=New Methods to Estimate Lattice Energies: Application to the Relative Stabilities of Bisulfite (HSO₃⁻) and Metabisulfite (S₂O₅^2-) Salts|year=2003|last1=Tudela|first1=David|last2=Jenkins|first2=H. Donald B.|journal=[[Journal of Chemical Education]]|volume=80|issue=12|pages=1482|url=https://pubs.acs.org/doi/pdf/10.1021/ed080p1482|url-access=subscription}}</ref> but a mixture of salts that dissolve in water to give solutions composed of sodium and [[bisulfite]] ions. It appears in form of white or yellowish-white crystals with an odor of [[sulfur dioxide]]. Regardless of its ill-defined nature, sodium bisulfite is used in many different industries such as a [[food additive]] with [[E number]] E222 in the food industry, a [[reducing agent]] in the cosmetic industry, and a [[Chemical decomposition|decomposer]] of residual hypochlorite used in the bleaching industry.<ref name=":0" /><ref name=":1" /><ref name=":2">{{cite journal |last=EFSA Panel on Food additives and Nutrient Sources added to Food (ANS) |date=2016 |title=Scientific Opinion on the re-evaluation of sulfur dioxide (E 220), sodium sulfite (E 221), sodium bisulfite (E 222), sodium metabisulfite (E 223), potassium metabisulfite (E 224), calcium sulfite (E 226), calcium bisulfite (E 227) and potassium bisulfite (E 228) as food additives |journal=[[EFSA Journal]] |volume=14 |issue=4 |doi=10.2903/j.efsa.2016.4438|doi-access=free }}</ref>

==Synthesis==

Sodium bisulfite solutions can be prepared by treating a solution of suitable base, such as [[sodium hydroxide]] or [[sodium bicarbonate]] with [[sulfur dioxide]].

:SO₂ + NaOH → NaHSO₃

:SO₂ + NaHCO₃ → NaHSO₃ + CO₂

Attempts to crystallize the product yield [[sodium metabisulfite]] (also called [[sodium disulfite]]), Na₂S₂O₅.<ref>{{cite book|doi=10.1002/9780470132333.ch49|isbn=9780470132333|chapter=Sulfites and Pyrosulfites of the Alkali Metals|series=[[Inorganic Syntheses]]|year=1946|last1=Johnstone|first1=H. F.|title=Inorganic Syntheses|pages=162–167|volume=2|url=https://onlinelibrary.wiley.com/doi/pdf/10.1002/9780470132333.ch49|url-access=subscription}}</ref>

Upon dissolution of the metabisulfite in water, bisulfite is regenerated:

:Na₂S₂O₅ + H₂O → 2 Na⁺ + 2 HSO₃⁻

Sodium bisulfite is formed during the [[Wellman-Lord process]].<ref>{{cite book | chapter-url = https://books.google.com/books?id=rfSItUDqX9sC&pg=PA554 |chapter-url-access=subscription| title = Gas Purification | chapter = Sulfur Dioxide Removal | first = Arthur L. | last = Kohl |author2=Nielsen, Richard B. | publisher = [[Gulf Professional Publishing]] | year = 1997 | isbn = 978-0-88415-220-0 | pages =554&ndash;555}}</ref>

==Uses==

===Cosmetics===

The safety of cosmetic products is constantly in question as the components are always changing or being discovered as a possibly harmful substance. The sulfite components of cosmetic ingredients, such as sodium bisulfite, underwent clinical trials to find out their safety in cosmetic formulations. Sodium bisulfite functions as a [[reducing agent]] and furthermore as a hair-waiving/straightening agent.<ref>{{cite journal |last1=Leite |first1=Marcella Gabarra Almeida |last2=Garbossa |first2=Wanessa Almeida Ciancaglio |last3=Campos |first3=Patricia Maria Berardo Gonçalves Maia |date=2018-11-29 |title=Hair straighteners: an approach based on science and consumer profile |journal=Brazilian Journal of Pharmaceutical Sciences |volume=54 |issue=3 |doi=10.1590/s2175-97902018000317339 |issn=2175-9790|doi-access=free }}</ref> As of 1998, sodium bisulfite was used in 58 different cosmetic products including hair conditioners, moisturizers, and hair dyes.<ref>{{cite journal |last1=Cherian |first1=Priya |last2=Zhu |first2=Jinqiu |last3=Bergfeld |first3=Wilma F. |last4=Belsito |first4=Donald V. |last5=Hill |first5=Ronald A. |last6=Klaassen |first6=Curtis D. |last7=Liebler |first7=Daniel C. |last8=Marks |first8=James G. |last9=Shank |first9=Ronald C. |last10=Slaga |first10=Thomas J. |last11=Snyder |first11=Paul W. |date=2020 |title=Amended Safety Assessment of Parabens as Used in Cosmetics |url=http://dx.doi.org/10.1177/1091581820925001 |journal=[[International Journal of Toxicology]] |volume=39 |issue=1_suppl |pages=5S–97S |doi=10.1177/1091581820925001 |pmid=32723119 |s2cid=220850521 |issn=1091-5818}}</ref>

In a cosmetic context, the reducing ability of sodium bisulfite is used to prevent discoloration, bleach food starches, and delay spoilage of the product. Since the sulfite molecule was used in so many compounds in the 1990s, the EPA, FDA, and American Conference of Governmental Industrial Hygienists established a working place threshold limit value for sulfur dioxide of 2ppm averaged over 8 hours, and a 3-hour level of 5ppm. Even with this threshold established, the FDA recognized sodium bisulfite as a "generally recognized as safe" compound.<ref name=":0" />

A final examination on the carcinogenicity, genotoxicity, oral toxicity, and cellular toxicity on consumed sodium bisulfite was conducted using living subjects such as mice and rats. The International Agency for Research on Cancer concluded that there was inadequate evidence that sodium bisulfite was [[Carcinogen|carcinogenic]].<ref name=":0" /> Under specific conditions such as acidity and concentration level, sodium bisulfite was able to cause negative alterations to the genome such as catalyzing [[transamination]], and induce [[Sister chromatids|sister-chromatid]] exchanges suggesting possible [[genotoxicity]].<ref>{{cite journal |last1=Abe |first1=Syuiti |last2=Sasaki |first2=Motomichi |date=1977 |title=Chromosome Aberrations and Sister Chromatid Exchanges in Chinese Hamster Cells Exposed to Various Chemicals 2 |url=https://academic.oup.com/jnci/article-lookup/doi/10.1093/jnci/58.6.1635|url-access=subscription |journal=[[Journal of the National Cancer Institute]] |language=en |volume=58 |issue=6 |pages=1635–1641 |doi=10.1093/jnci/58.6.1635 |pmid=864744 |issn=1460-2105}}</ref> In a study using Osbourne-Mendel strain rats, it was concluded that oral toxicity was not significant if the consumed concentration was less than 0.1% (615ppm as SO2).<ref>{{cite journal |last1=Jonker |first1=D. |last2=Woutersen |first2=R.A. |last3=van Bladeren |first3=P.J. |last4=Til |first4=H.P. |last5=Feron |first5=V.J. |date=1990 |title=4-Week oral toxicity study of a combination of eight chemicals in rats: Comparison with the toxicity of the individual compounds |url=https://linkinghub.elsevier.com/retrieve/pii/027869159090170R |url-access=subscription|journal=[[Food and Chemical Toxicology]] |language=en |volume=28 |issue=9 |pages=623–631 |doi=10.1016/0278-6915(90)90170-R|pmid=2272560 }}</ref> A study done by Servalli, Lear, and Cottree in 1984 found that sodium bisulfite did not produce membrane fusion in [[Liver|hepatic]] and [[Murinae|murine]] [[Glia|glial cells]] and human [[Fibroblast|fibroblasts]] so there is no oral toxicity. These clinical studies concluded that sodium bisulfite was safe to use in cosmetic formulations.<ref name=":0" />

===Food industry===

Similar to the cosmetic industry, the European Commission requested the [[European Food Safety Authority]] (EFSA) to review and determine if the use of sulfites as food additives was still safe in light of new scientific technology and information. Since sodium bisulfite is a known sulfonating compound, it underwent the experimentation. Based on clinical experiments using rats and mice, the World Health Organization Expert Committee on Food Additives came to the conclusion that 0-0.7mg of sulfur dioxide equivalent/kg of body weight per day will cause no harm to an individual consuming this compound as a food additive. The genotoxicity and carcinogenicity were examined just as in the cosmetic trials and in both cases, no potential for concern with respect to the sulfites were found.<ref name=":2" />

The production of sodium bisulfite used as a food additive can be described by the combination of [[sulfur dioxide]] gas with aqueous [[sodium hydroxide]] solution in usual absorber apparatuses. In order to analyze the amount of free sulfites in food as a result of the sulfonation of sodium bisulfite, multiple methods can be used including the Monier-Williams type procedure,<ref>{{cite journal |title=Reevaluation of Monier-Williams method for determining sulfite in food |url=https://academic.oup.com/jaoac/article-abstract/69/1/3/5697566 |access-date=2022-09-20 |publisher=[[Oxford University Press]]|journal=[[Journal of AOAC International]]}}</ref> [[High-performance liquid chromatography|HPLC]] after extraction, and [[Flow injection analysis|Flow Injection]] analysis. Overall, the use of sodium bisulfite in the food industry as an additive and antioxidant is safe and beneficial to the lifespan of processed foods.<ref name=":2" />

===Textile industry===

An [[antichlor]] is a substance used to decompose residual [[hypochlorite]] or chlorine after [[Chlorine-based bleach|chlorine-based bleaching]], in order to prevent ongoing reactions with, and therefore damage to, the material that has been bleached. Sodium bisulfite is an example of an antichlor. Historically, sodium bisulfite has been used in the textile industry, cosmetic industry, food industry, and more.<ref name=":0">{{cite journal |date=2003-06-01 |title=Final Report on the Safety Assessment of Sodium Sulfite, Potassium Sulfite, Ammonium Sulfite, Sodium Bisulfite, Ammonium Bisulfite, Sodium Metabisulfite and Potassium Metabisulfite |url=http://ijt.sagepub.com/cgi/doi/10.1080/10915810390239478 |journal=[[International Journal of Toxicology]] |language=en |volume=22 |issue=2 Suppl |pages=63–88 |doi=10.1080/10915810305077X |pmid=14555420 |issn=1091-5818|last1=Nair |first1=B. |last2=Elmore |first2=A. R. |author3=Cosmetic Ingredients Review Expert Panel }}</ref><ref name=":1">{{Citation |last1=Periyasamy |first1=A.P. |title=Denim processing and health hazards |date=2017 |url=https://linkinghub.elsevier.com/retrieve/pii/B9780081020432000071 |work=Sustainability in Denim |pages=161–196 |publisher=Elsevier |language=en |doi=10.1016/b978-0-08-102043-2.00007-1 |isbn=978-0-08-102043-2 |access-date=2022-05-11 |last2=Militky |first2=J.|url-access=subscription}}</ref>

Antichlors are very useful in the textile industry because bleaching of compounds using chlorine is a standard practice. However, the use of sodium bisulfite in the decomposition of excess hypochlorite can lead to harmful byproducts when it comes into contact with water at the concentrations present for industrial use.<ref name=":1" /> Contact with these dangerous byproducts or even strong concentrations of sodium bisulfite can be harmful to the environment and contact with the skin. Strong concentrations of these compounds can contaminate ecosystems, harm animals, and cause contact dermatitis with industrial workers.<ref name=":1" /><ref>{{cite journal |last1=Nagayama |first1=Hirotoshi |last2=Hatamochi |first2=Atsushi |last3=Shinkai |first3=Hiroshi |date=1997 |title=A Case of Contact Dermatitis Due to Sodium Bisulfite in an Ophthalmic Solution |url=https://onlinelibrary.wiley.com/doi/10.1111/j.1346-8138.1997.tb02315.x|url-access=subscription |journal=The Journal of Dermatology|language=en |volume=24 |issue=10 |pages=675–677 |doi=10.1111/j.1346-8138.1997.tb02315.x|pmid=9375469 |s2cid=21945156 }}</ref> The concentrations that could result in these outcomes are much stronger than the concentrations discussed in the cosmetic and food industry.

==See also==

* [[Sodium metabisulfite]]

* [[Calcium bisulfite]]

* [[Potassium bisulfite]]

* [[Croscarmellose sodium]]

* [[Sulfurous acid]]

==References==

{{reflist}}

{{Sodium compounds}}

[[Category:Sodium compounds]]

[[Category:Bisulfites]]

[[Category:Reagents for organic chemistry]]

[[Category:Food additives]]

[[Category:Reducing agents]]

[[Category:E-number additives]]