Disulfuric acid
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| verifiedrevid = 410648395
| ImageFile1 = Dischwefelsäure - Disulfuric acid.svg
| ImageFile1_Ref = {{Chemboximage|correct|??}}
| ImageSize1 = 150
| ImageAltL1 = Structural formula of disulfuric acid
| ImageFile2 = Pyrosulfuric acid molecule ball.png
| ImageFile2_Ref = {{Chemboximage|correct|??}}
| ImageSize2 = 150
| ImageAlt2 = Ball and stick model of the disulfuric acid molecule
| IUPACName = Disulfuric acid {{RedBookRef|page=130}}
| OtherNames = Pyrosulfuric acid, Oleum
| Section1 = {{Chembox Identifiers
| CASNo = 7783-05-3
| CASNo_Ref = {{cascite|correct|??}}
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII = NTC1O8E83E
| PubChem = 62682
| ChemSpiderID = 56433
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| EINECS = 231-976-8
| MeSHName = Pyrosulfuric+acid
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 29211
| SMILES = OS(=O)(=O)OS(O)(=O)=O
| SMILES1 = OS(=O)(=O)OS(=O)(=O)O
| SMILES2 = O=S(=O)(O)OS(=O)(=O)O
| StdInChI = 1S/H2O7S2/c1-8(2,3)7-9(4,5)6/h(H,1,2,3)(H,4,5,6)
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| InChI = 1/H2O7S2/c1-8(2,3)7-9(4,5)6/h(H,1,2,3)(H,4,5,6)
| StdInChIKey = VFNGKCDDZUSWLR-UHFFFAOYSA-N
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| InChIKey = VFNGKCDDZUSWLR-UHFFFAOYAZ
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|Section2={{Chembox Properties
| H=2 | O=7 | S=2
| MeltingPtC = 36
| ConjugateBase = Disulfate
| Appearance = colorless
| pKa = 2.5 ({{degC|20}}; in conc. H2SO4){{cite book|title=Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution|editor-first=D. D.|editor-last=Perrin|edition=2nd|series=IUPAC Chemical Data|issue=29|publisher=Pergamon|location=Oxford|year=1982|publication-date=1984|orig-date=1969|lccn=82-16524|isbn=0-08-029214-3|at=Entry 62}}
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Disulfuric acid (alternative spelling disulphuric acid) or pyrosulfuric acid (alternative spelling pyrosulphuric acid), also named oleum, is a sulfur oxoacid.{{Greenwood&Earnshaw}} It is a major constituent of fuming sulfuric acid, oleum, and this is how most chemists encounter it. As confirmed by X-ray crystallography, the molecule consists of a pair of SO2(OH) groups joined by an oxide.{{cite journal |doi=10.1524/zkri.1991.196.14.279|title=Crystal structure of H2S2O7 at 298 K |year=1991 |last1=Hönle |first1=Wolfgang |journal=Zeitschrift für Kristallographie - Crystalline Materials |volume=196 |issue=1–4 |s2cid=101311329 }}
Reactions
It is also a minor constituent of liquid anhydrous sulfuric acid due to the equilibria:
:{{chem2 | H2SO4(l) <-> H2O(l) + SO3(g)}}
:{{chem2 | SO3(g) + H2SO4(l) <-> H2S2O7(l)}}
:{{chem2 | 2H2SO4(l) <-> H2O(l) + H2S2O7(l)}}
The acid is prepared by reacting excess sulfur trioxide (SO3) with sulfuric acid:
:{{chem2 |H2SO4(l) + SO3(g) -> H2S2O7(l)}}
Disulfuric acid can be seen as the sulfuric acid analog of an acid anhydride. The mutual electron-withdrawing effects of each sulfuric acid unit on its neighbour causes a marked increase in acidity. Disulfuric acid is strong enough to protonate "normal" sulfuric acid in the (anhydrous) sulfuric acid solvent system. There are salts of disulfuric acid, commonly called pyrosulfates, e.g. potassium pyrosulfate.
There are other related acids with the general formula H2O·(SO3)x though none can be isolated.
See also
References
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{{Hydrogen compounds}}