| Revision as of 10:57, 20 January 2012 editThe chemistds (talk | contribs)Extended confirmed users5,761 edits added CSID, (std)InChI and (Std)InChIKey← Previous edit |
Latest revision as of 11:32, 26 December 2024 edit undoJohn of Reading (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers766,770 editsm →Economical: Typo fixing, replaced: effieciency → efficiencyTag: AWB |
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{{chembox |
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| verifiedrevid = 421616428 |
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| verifiedrevid = 472231117 |
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| Name = |
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|ImageFile=Calcium bisulfite.png |
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| ImageFile = Calcium bisulfite.png |
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|ImageSize=120px |
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| ImageSize = 120px |
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|IUPACName=Calcium hydrogen sulfite |
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| ImageFile1 = Calcium bisulfite ball-and-stick.png |
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|OtherNames=Calcium bisulphite<br>E227 |
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| IUPACName = Calcium hydrogen sulfite |
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|Section1= {{Chembox Identifiers |
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| OtherNames = {{Unbulleted list|Calcium bisulphite|E227}} |
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| CASNo_Ref = {{cascite|correct|??}} |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo=13780-03-5 |
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| CASNo=13780-03-5 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| PubChem=26268 |
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| RTECS = EV9294500 |
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| UNII = SNM7K02JP2 |
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| PubChem=26268 |
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| SMILES=OS(=O).OS(=O). |
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| RTECS = EV9294500 |
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| ChemSpiderID = 24475 |
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| SMILES=OS(=O).OS(=O). |
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| InChI = 1/Ca.2H2O3S/c;2*1-4(2)3/h;2*(H2,1,2,3)/q+2;;/p-2 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| InChIKey = LVGQIQHJMRUCRM-NUQVWONBAX |
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| ChemSpiderID = 24475 |
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| StdInChI = 1S/Ca.2H2O3S/c;2*1-4(2)3/h;2*(H2,1,2,3)/q+2;;/p-2 |
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| InChI = 1/Ca.2H2O3S/c;2*1-4(2)3/h;2*(H2,1,2,3)/q+2;;/p-2 |
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| StdInChIKey = LVGQIQHJMRUCRM-UHFFFAOYSA-L |
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| InChIKey = LVGQIQHJMRUCRM-NUQVWONBAX |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/Ca.2H2O3S/c;2*1-4(2)3/h;2*(H2,1,2,3)/q+2;;/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = LVGQIQHJMRUCRM-UHFFFAOYSA-L |
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|Section2= {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula=Ca(HSO<sub>3</sub>)<sub>2</sub> |
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| Formula=Ca(HSO<sub>3</sub>)<sub>2</sub> |
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| MolarMass=202.22 g/mol |
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| MolarMass=202.22 g/mol |
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| MeltingPt=203 °C |
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|Section3= {{Chembox Hazards |
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| Section3 = {{Chembox Hazards |
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| Section4 = |
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'''Calcium bisulfite''' (calcium bisulphite) is an ] which is the ] of a ] cation and a ] anion. It may be prepared by reacting lime with an excess of ], essentially a mixture of ] and water. It is a weak reducing agent, as is sulfur dioxide, ]s, and any other compound containing sulfur in the +4 oxidation state. As a ] it is used as a ] under the ] E227.Calcium bisuphite is an acid salt and behaves like an acid in in its aqueous solution. |
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'''Calcium bisulfite''' ('''calcium bisulphite''' or '''calcium hydrogen sulfite''') is an ] which is the ] of a ] cation and a ] anion. It may be prepared by treating lime with an excess of ] and water. As a ] it is used as a ] under the ] E227. Calcium bisulfite is an ] and behaves like an acid in aqueous solution. It is used in the ] for producing paper from wood chips.<ref>{{Ullmann|doi=10.1002/14356007.a18_545|isbn=3527306730|title=Paper and Pulp|year=2000|last1=Patt|first1=Rudolf|last2=Kordsachia|first2=Othar|last3=Süttinger|first3=Richard|last4=Ohtani|first4=Yoshito|last5=Hoesch|first5=Jochen F.|last6=Ehrler|first6=Peter|last7=Eichinger|first7=Rudolf|last8=Holik|first8=Herbert|last9=Hamm|first9=Udo|last10=Rohmann|first10=Michael E.|last11=Mummenhoff|first11=Peter|last12=Petermann|first12=Erich|last13=Miller|first13=Richard F.|last14=Frank|first14=Dieter|last15=Wilken|first15=Renke|last16=Baumgarten|first16=Heinrich L.|last17=Rentrop|first17=Gert-Heinz}}</ref> |
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== Synthesis == |
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Calcium bisulfite can be prepared by treating lime (chemical formula Ca(OH)<sub>2</sub>) with an excess of ] and water.<ref name=":1">{{Cite journal |last1=Karatza |first1=Despina |last2=Prisciandaro |first2=Marina |last3=Lancia |first3=Amedeo |last4=Musmarra |first4=Dino |date=2010-06-01 |title=Sulfite Oxidation Catalyzed by Cobalt Ions in Flue Gas Desulfurization Processes |url=https://doi.org/10.3155/1047-3289.60.6.675 |journal=Journal of the Air & Waste Management Association |volume=60 |issue=6 |pages=675–680 |doi=10.3155/1047-3289.60.6.675 |pmid=20564992 |bibcode=2010JAWMA..60..675K |s2cid=9127556 |issn=1096-2247}}</ref> Upon synthesis of calcium bisulfite solution, it will have a green to yellow opaque appearance as an aqueous solution.<ref name=":0">{{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> |
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== Chemical reactions == |
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When calcium bisulfite reacts with the surrounding air, a crystalline precipitate will form composed of ].{{cn|date=September 2023}} |
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When calcium bisulfite is digested as a food additive, different reactions in metabolic pathways can result. One common pathway results in a reaction that will yield 6%-8% ]. This can go to ] when absorbed by the lungs, and the sulfite will be converted to sulfate in the liver by an enzyme called ]. Sulfite can be harmful for people susceptible to asthma, leading to asthma attacks. Sulfite can also cause urticaria and angioedema in otherwise healthy individuals. <ref name=":0" /> |
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A process known as wet limestone scrubbing is a means by which sulfur dioxide is removed from the waste emitted during the ] of ]s. A step in this process is the oxidation of calcium bisulfite to produce sulfate. When this reaction occurs in an aqueous solution, ] results. The rate of this reaction can be increased in the presence of magnesium(II) sulfate as a catalyst.<ref>{{Cite journal |last1=Lancia |first1=Amedeo |last2=Musmarra |first2=Dino |last3=Prisciandaro |first3=Marina |last4=Tammaro |first4=Marco |date=1999-07-01 |title=Catalytic oxidation of calcium bisulfite in the wet limestone–gypsum flue gas desulfurization process |url=https://www.sciencedirect.com/science/article/pii/S0009250998004837 |journal=Chemical Engineering Science |language=en |volume=54 |issue=15 |pages=3019–3026 |doi=10.1016/S0009-2509(98)00483-7 |bibcode=1999ChEnS..54.3019L |issn=0009-2509}}</ref> |
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Other catalysts for the oxidation of calcium bisulfite include ], ], ], ], ], and ].<ref name=":1" /> |
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== Application == |
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=== Economical === |
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Calcium bisulfite is one of the chemicals used in an overall mild bisulfite treatment meant to increase the sugar yield efficiency in processing timber excess to biofuel and ]. The use of the Mild Bisulfite methodology both increases the yield and also saves cost in shipping wood to ] for processing.<ref>{{Cite web |last=Dwight Anderson and |first=Johnway Gao |date=2015 |title=Mild Bisulfite Pretreatment of Forest Residuals |url=https://s3.amazonaws.com/na-st01.ext.exlibrisgroup.com/01ALLIANCE_WSU/storage/alma/03/75/F5/3A/33/3A/DD/50/93/FC/A6/39/20/B2/44/C0/Mild%20Bisulfite%20Report.pdf?response-content-type=application%2Fpdf&X-Amz-Algorithm=AWS4-HMAC-SHA256&X-Amz-Date=20230329T182812Z&X-Amz-SignedHeaders=host&X-Amz-Expires=119&X-Amz-Credential=AKIAJN6NPMNGJALPPWAQ%2F20230329%2Fus-east-1%2Fs3%2Faws4_request&X-Amz-Signature=082da084ae382e2d77b57cbf5da69b5489f0051e2a7bb4a1f2ee8d13024a34e3}}</ref> |
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Calcium bisulfite is often used as a food preservative. One such case is to brine cherries. However, research is showing that some microorganisms can cause cherries to rot since they produce the enzyme ] that can work even in the presence of calcium bisulfite. Three species of fungi that are especially capable of rotting brined cherries are ''], ],'' and '']''.<ref>{{Cite journal |last=Lewis JC |first=Pierson CF, Powers MJ |date=1963 |title=Fungi Associated with Softening of Bisulfite-Brined Cherries |url=https://doi.org/10.1128/am.11.2.93-99.1963 |journal=Applied and Environmental Microbiology |volume=11 |issue=2 |pages=93–99 |doi=10.1128/am.11.2.93-99.1963 |pmid=16349630 |pmc=1057949 |s2cid=9370969 |via=ASM Journals}}</ref> |
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=== Medicinal === |
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A calcium bisulfite liquor solution is used in the process of converting ] in tree bark pulp and then converting dihydroquercetin to a usable form: ]. Calcium bisulfite is not the optimum bisulfite compound for this reaction since the calcium ions can be removed from the calcium bisulfite solution during the reaction, thereby inhibiting the mechanism. However, calcium bisulfites, like other bisuflites such as ], have a catalytic capacity in this reaction since they are not used up and can be reused.<ref>{{Cite journal |last=Kurth |first=Ervin |date=1953 |title=Quercetin from Fir and Pine Bark |url=https://pubs.acs.org/doi/abs/10.1021/ie50525a047 |access-date=2023-03-29 |journal=Industrial & Engineering Chemistry|volume=45 |issue=9 |pages=2096–2097 |doi=10.1021/ie50525a047 }}</ref> |
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==See also== |
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==References== |
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{{reflist}} |
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{{Calcium compounds}} |
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{{Calcium compounds}} |
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