Browse history interactively

Page 1

Page 1Revision 1

Page 2

Page 2Revision 2

← Previous editContent deleted Content addedVisualWikitext

Revision as of 11:14, 9 April 2011 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'UNII_Ref', 'ChemSpiderID_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref', 'ChEMBL_Ref', 'KEGG_Ref') per Chem/Drugbox validation (← Previous edit		Latest revision as of 15:34, 19 April 2024 edit undoReconrabbit (talk | contribs)Autopatrolled, Extended confirmed users, New page reviewers8,257 editsm →Use: typoTag: Visual edit
(52 intermediate revisions by 33 users not shown)
Line 1:		Line 1:
	{{Distinguish|Bisulfite}}		{{Distinguish|Bisulfite}}
	{{chembox		{{chembox
			| Watchedfields = changed
	| verifiedrevid = 410199422		| verifiedrevid = 423158544
	| Name = Disulfite ion		| Name = Disulfite ion
	| ImageFile = Disulfit-Ion2.svg		| ImageFile = Structure of metabisulfite ion.png
	| ImageSize = 140px		| ImageSize = 190px
	| ImageFile1 =		| ImageFile1 = Metabisulfite-ion-from-xtal-3D-bs-17.png
		⚫	| IUPACName = disulfite<ref name=redbookname>{{RedBookRef|page=130}}</ref>
	| ImageSize1 =
			| SystematicName = pentaoxido-1''κ''<sup>3</sup>''O'',2''κ''<sup>2</sup>''O''-disulfate(S—S)(2−)<ref name=redbookname/>
	| ImageName1 =
⚫	| IUPACName = disulfite <ref>{{RedBookRef|page=130}}</ref>
	| OtherNames = metabisulfite ion<br />pyrosulfite		| OtherNames = metabisulfite ion<br />pyrosulfite
	| Section1 = {{Chembox Identifiers		| Section1 = {{Chembox Identifiers
	| CASNo =		| CASNo = 23134-05-6
	| CASNo_Ref =		| CASNo_Ref = {{cascite|correct|CAS}}
			| ChemSpiderID = 140610
	| PubChem = 159940		| PubChem = 159940
	| RTECS =		| RTECS =
			| UNII = 7992SO049K
			| SMILES = ()()()
			| StdInChI=1S/H2O5S2/c1-6(2)7(3,4)5/h(H,1,2)(H,3,4,5)/p-2
			| StdInChIKey = WBZKQQHYRPRKNJ-UHFFFAOYSA-L
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = S<sub>2</sub>O<sub>5		| Formula = {{chem|S|2|O|5|2−}}
	| MolarMass =		| MolarMass =
	| Appearance =		| Appearance =
Line 25:		Line 29:
	| MeltingPt =		| MeltingPt =
	| BoilingPt =		| BoilingPt =
			| ConjugateAcid = ]
	}}		}}
	}}		}}
			A '''disulfite''', commonly known as '''metabisulfite''' or '''pyrosulfite''', is a ] containing the ion {{chem|S|2|O|5|2−}}. It is a colorless dianion that is primarily marketed in the form of ] or ]. When dissolved in water, these salts release the hydrogensulfite {{chem|H|S|O|3|−}} anion. These salts act equivalently to ] or ].<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}}</ref>
	A '''disulfite''', commonly known as '''metabisulfite''', is a ] containing the '''disulfite ion''' ('''metabisulfite ion''') .
	==Chemistry==		==Structure==
			In contrast to ] ({{chem|S|2|O|7|2−}}), disulfite ion ({{chem|S|2|O|5|2−}}) has an unsymmetrical structure with an S-S bond. The oxidation state of the sulfur atom bonded to 3 oxygen atoms is +5 while oxidation number of other sulfur atom is +3.<ref>{{cite journal|first1=I.|last1=Lindqvist|first2=M.|last2=Mörtsell|title=The Structure of Potassium Pyrosulfite and the Nature of the Pyrosulfite Ion". |journal=] |date= 1957|volume=10 |pages=406–409 |doi=10.1107/S0365110X57001322 |doi-access=free}}</ref>
⚫	===Production of the disulfite ion===
			The anion consists of an SO<sub>2</sub> group linked to an SO<sub>3</sub> group, with the negative charge more localized on the SO<sub>3</sub> end. The S–S bond length is 2.22&nbsp;Å, and the "thionate" and "thionite" S–O distances are 1.46 and 1.50&nbsp;Å respectively.<ref>K. L. Carter, T. A. Siddiquee, K. L. Murphy, D. W. Bennett "The surprisingly elusive crystal structure of sodium metabisulfite" ''Acta Crystallogr.'' (2004). '''B60''', 155–162. {{doi|10.1107/S0108768104003325}}</ref>
	The disulfite ion is a ] of the ] ion (HSO<sub>3</sub><sup>−</sup>). It can arise from:
		⚫	===Production===
			Salts of disulfite ion are produced by dehydration of salts of ] ion ({{chem|HSO|3|−}}). When solutions of ] or ] are evaporated, ] and ] result.<ref>{{Ullmann|doi=10.1002/14356007.a25_477|isbn=3527306730|title=Sulfites, Thiosulfates, and Dithionitesl Chemistry|year=2000|last1=Barberá|first1=José Jiménez|last2=Metzger|first2=Adolf|last3=Wolf|first3=Manfred}}</ref>
			:{{chem2|2 HSO3−}} ] {{chem2|S2O5(2−) + H2O}}
		⚫	Although the equilibrium lies far to the left, evaporation of a bisulfite salt will produce a substantial amount of disulfite.<ref name=Bassam>Bassam Z. Shakhashiri: The University of Wisconsin Press, 1992, p.9</ref>
	''']'''
		⚫	Disulfite is the conjugate base of ] (pyrosulfurous acid), which originates from ] in accordance with the dehydration reaction above:<br />
	In aqueous solution, the disulfite ion is formed in minor amounts by dehydration of bisulfite in an equilibrium:
	: 2 HSO<sub>3</sub><sup>−</sup> (aq) ] S<sub>2</sub>O<sub>5</sub><sup>2&minus;</sup> (aq) + H<sub>2</sub>O (l)		:2 H<sub>2</sub>SO<sub>3</sub> → 2 {{chem|HSO|3|−}} + 2 H<sup>+</sup> → H<sub>2</sub>S<sub>2</sub>O<sub>5</sub> + H<sub>2</sub>O
		⚫	The disulfite ion also arises from the addition of ] to the ] ion:
⚫	Although the equilibrium lies far to the left, evaporation of a bisulfite salt will produce a substantial amount of disulfite.<ref name=Bassam>Bassam Z. Shakhashiri: The University of Wisconsin Press @Google Books, 1992, p.9</ref>
⚫	In fact, disulfite is the ion of ] (pyrosulfurous acid), which originates from ] in accordance with the dehydration reaction above:<br />
	:2 H<sub>2</sub>SO<sub>3</sub> → 2 HSO<sub>3</sub><sup>−</sup> + 2 H<sup>+</sup> → H<sub>2</sub>S<sub>2</sub>O<sub>5</sub> + H<sub>2</sub>O
	'''addition'''
⚫	The disulfite ion also arises from the addition of ] to the ] ion:<br />
	{| class="wikitable"		{| class="wikitable"
	|-		|-
	|HSO<sub>3</sub><sup>−</sup> ] SO<sub>3</sub><sup>2−</sup> + H<sup>+</sup><br /><br />SO<sub>3</sub><sup>2−</sup> + SO<sub>2</sub> ] S<sub>2</sub>O<sub>5</sub><sup>2−</sup> || &nbsp; || ]		|{{chem|HSO|3|−}} ] {{chem|SO|3|2−}} + H<sup>+</sup><br /><br />SO<sub>3</sub><sup>2−</sup> + SO<sub>2</sub> ] {{chem|S|2|O|5|2−}} || &nbsp; || ]
	|}		|}
			==Use==
	===Other reactions===
			Disulfite salts are used for ] and as ], with the main species used for this purpose being ] (])<ref>{{Cite journal |last=Noorafshan |first=A. |last2=Asadi-Golshan |first2=R. |last3=Monjezi |first3=S. |last4=Karbalay-Doust |first4=S. |date=2014 |title=Sodium metabisulphite, a preservative agent, decreases the heart capillary volume and length, and curcumin, the main component of Curcuma longa, cannot protect it |url=https://pubmed.ncbi.nlm.nih.gov/25629268 |journal=Folia Biologica |volume=60 |issue=6 |pages=275–280 |issn=0015-5500 |pmid=25629268}}</ref> and ] (E224).<ref>{{Cite web |last=PubChem |title=Potassium metabisulfite |url=https://pubchem.ncbi.nlm.nih.gov/compound/28019 |access-date=2024-04-19 |website=pubchem.ncbi.nlm.nih.gov |language=en}}</ref> Sulfites are implicated in asthmatic reactions and may also cause symptoms in non-asthmatic individuals, namely ], ], ], ], ] and ], and even life-threatening ].<ref name="pmid24834193">{{cite journal |vauthors=Vally H, Misso NL |title=Adverse reactions to the sulphite additives |journal=Gastroenterol Hepatol Bed Bench |volume=5 |issue=1 |pages=16–23 |date=2012 |pmid=24834193 |pmc=4017440 |doi= |url=}}</ref>
	In aqueous solution, disulfite salts decompose with acids:<br />
	S<sub>2</sub>O<sub>5</sub><sup>2−</sup> + H<sup>+</sup> → HSO<sub>3</sub><sup>−</sup> + SO<sub>2</sub>
	==Examples of disulfites==
	*] (]) and ] (E224) are used as a ] and ] in food.
	==References==		==References==
	{{reflist}}		{{reflist}}
	]		]
			]
	]
	]