Fluoroantimonic acid and Lithium monoxide anion: Difference between pages
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| ImageFileL1 = Fluoroantimonic acid.png |
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| ImageFileL1_Ref = {{chemboximage|correct|??}} |
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| verifiedrevid = 459445215 |
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| ImageSizeL1 = 121 |
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| ImageFile = |
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| ImageNameL1 = Canonical, stereo, skeletal formula of fluoroantimonic acid |
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| ImageFile2 = |
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| ImageFileR1 = Fluoroantimonic-acid-3D-vdW.png |
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| ImageSize = 240 |
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| ImageFileR1_Ref = {{chemboximage|correct|??}} |
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| IUPACName = Lithium monoxide anion |
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| ImageSizeR1 = 121 |
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| OtherNames = Lithate |
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| ImageNameR1 = Canonical, spacefill model of fluoroantimonic acid |
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|Section1={{Chembox Identifiers |
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| IUPACName = Fluoroantimonic acid{{Citation needed|date = July 2011}} |
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| CASNo = 64538-53-0 |
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| Section1 = {{Chembox Identifiers |
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| CASNo_Ref =<ref>{{cite web |title=Lithium oxide anion |url=https://webbook.nist.gov/cgi/formula?ID=C64538530 |website=webbook.nist.gov |language=en}}</ref> |
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| CASNo = <!-- blanked - oldvalue: 16950-06-4 --> |
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| SMILES = [Li]-[O-] |
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| StdInChI=1S/Li.O/q;-1 |
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| PubChem_Ref = {{Pubchemcite|correct|pubchem}} |
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| StdInChIKey = IXZJKKSRIFXCQD-UHFFFAOYSA-N |
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| ChemSpiderID = 20137913 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| EINECS = 241-023-8 |
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| SMILES = F[Sb-](F)(F)(F)(F)[FH+] |
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| StdInChI = 1S/FH.2H2O.O.Sb/h1H;2*1H2;;/q;;;;+3/p-3 |
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| StdInChIKey = DAIOAWAJEVEBIG-UHFFFAOYSA-K |
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}} |
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|Section2={{Chembox Properties |
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| Li=1|O=1|Formula_Charge=- |
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| Formula = {{Chem|SbHF|6}} |
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| ConjugateAcid = [[Lithium hydroxide]] |
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| MolarMass = 236.76 g mol<sup>-1</sup> |
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| ExactMass = 235.902062306 g mol<sup>-1</sup> |
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| Appearance = Colourless liquid |
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| pKa = −25 |
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| pKb = 39 |
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|Section3={{Chembox Hazards |
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| MainHazards = Extremely corrosive |
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| RPhrases = {{R26}}, {{R29}}, {{R35}} |
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| NFPA-H = 4 |
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| NFPA-F = 0 |
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| NFPA-R = 3 |
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| NFPA-O = W |
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|Section4={{Chembox Related |
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| OtherFunction_label = [[base (chemistry)|base]]s |
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| Function = [[acid]]s |
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| OtherFunction = {{unbulleted list| |
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| OtherFunctn = [[Antimony pentafluoride]]<br /> |
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* [[Methyl anion]] |
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[[Hydrogen fluoride]]<br /> |
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* [[Diethynylbenzene dianion]]s |
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[[Magic acid]] |
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}} |
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}} |
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'''Lithium monoxide anion''' ({{chem2|LiO−}}) is a [[superbase]] existing in the gas phase. It was the strongest known [[base (chemistry)|base]] until 2008, when the isomeric [[diethynylbenzene dianion]]s were determined to have a higher proton affinity. The [[methyl anion|methanide ion]] {{chem2|CH3−}} was the strongest known base before lithium monoxide anion was discovered.<ref>{{cite journal |last1=Poad |first1=Berwyck L. J. |last2=Reed |first2=Nicholas D. |last3=Hansen |first3=Christopher S. |last4=Trevitt |first4=Adam J. |last5=Blanksby |first5=Stephen J. |last6=Mackay |first6=Emily G. |last7=Sherburn |first7=Michael S. |last8=Chan |first8=Bun |last9=Radom |first9=Leo |title=Preparation of an ion with the highest calculated proton affinity: ''ortho''-diethynylbenzene dianion |journal=Chemical Science |date=2016 |volume=7 |issue=9 |pages=6245–6250 |doi=10.1039/C6SC01726F |pmid=30034765 |pmc=6024202 |doi-access=free}}</ref> |
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'''Fluoroantimonic acid''' (HSbF<sub>6</sub>) is a mixture of [[hydrogen fluoride]] and [[antimony pentafluoride]] in various ratios.<ref name=Olah>[[George Olah|Olah]], G. A.; Prakash, G. K. S.; Wang, Q.; Li, X. “Hydrogen Fluoride–Antimony(V) Fluoride” in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.</ref> The 1:1 combination forms the strongest known [[superacid]], which has been demonstrated to [[protonate]] even [[hydrocarbon]]s to afford [[carbocation]]s and H<sub>2</sub>.<ref>{{cite book |
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| title = A life of magic chemistry: autobiographical reflections of a nobel prize winner |
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| author = George Andrew Olah |
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| publisher = John Wiley and Sons |
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| year = 2001 |
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| isbn = 0471157430 |
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| pages = 100–101 |
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}}</ref> |
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{{chem2|LiO−}} has a [[proton affinity]] of ~1782 kJ/[[Mole (unit)|mol]].<ref>{{Cite journal|date=6 February 2016|doi=10.1016/j.cplett.2016.02.010|title=OLi<sub>3</sub>O<sup>–</sup> anion: Designing the strongest base to date using OLi<sub>3</sub> superalkali|last1=Srivastava|first1=Ambrish Kumar|last2=Misra|first2=Neeraj|journal=Chemical Physics Letters|volume=648|pages=152–155|bibcode=2016CPL...648..152S}}</ref> |
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The reaction of hydrogen fluoride (HF) and SbF<sub>5</sub> is exothermic. HF, being a [[Lewis base]], attacks the molecules of SbF<sub>5</sub> to give an adduct. In the fluoroantimonic molecule, the anion is coordinated to the hydrogen, although the anion is formally classified as [[noncoordinating anion|noncoordinating]], because it is both a very weak [[nucleophile]] and a very weak [[base (chemistry)|base]]. |
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== Synthesis of the lithium monoxide anion == |
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Despite the [[proton]] being called effectively "naked," it is in fact always attached to a fluorine through a very weak [[dative bond]], similar to the [[hydronium]] cation.<ref> [http://www.psc.edu/science/klein2000.html] The quantum chemistry of proton "hopping" or transfer in his acid. Accessed 2-27-2011.</ref> However, the weakness of this bond accounts for the system's extreme acidity. Fluoroantimonic acid is 2×10<sup>19</sup> (20 quintillion) times stronger than 100% [[sulfuric acid]].<ref name=Olah2>{{cite journal | author = Olah, George A. | year = 2005 | title = Crossing Conventional Boundaries in Half a Century of Research | journal = [[J. Org. Chem.]] | volume = 70 | issue = 7 | pages = 2413–2429 | doi = 10.1021/jo040285o | pmid = 15787527}}</ref> |
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The anion is prepared in a [[mass spectrometer]] by successive [[decarboxylation]] and [[decarbonylation]] of [[lithium oxalate]] anion under [[collision-induced dissociation]] (CID) conditions: |
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:{{chem2|LiO\sC(\dO)\sCO2− → LiO\sC(\dO)− + CO2}} |
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:{{chem2|LiO\sC(\dO)− → LiO− + CO}} |
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The above method to synthesize the lithium monoxide anion is inefficient and difficult to carry out. The required ion rapidly reacts with traces of moisture and molecular [[oxygen]] present in the air. The reaction is further intensified by the high pressure [[argon]] that is introduced into the instrument to carry out the CID step.<ref name="auto">{{Cite journal|last1=Tian|first1=Zhixin|last2=Chan|first2=Bun|last3=Sullivan|first3=Michael B.|last4=Radom|first4=Leo|last5=Kass|first5=Steven R.|date=2008-06-03|title=Lithium monoxide anion: A ground-state triplet with the strongest base to date|journal=Proceedings of the National Academy of Sciences of the United States of America|volume=105|issue=22|pages=7647–7651|doi=10.1073/pnas.0801393105|issn=0027-8424|pmc=2409378|pmid=18511563|bibcode=2008PNAS..105.7647T|doi-access=free}}</ref> |
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:[[Image:Reaction of HF with SbF5.png|400px]] |
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==Structure== |
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Two related products have been crystallised from HF-SbF<sub>5</sub> mixtures, and both have been analyzed by single crystal X-ray [[crystallography]]. These salts have the formulas [H<sub>2</sub>F<sup>+</sup>][Sb<sub>2</sub>F<sub>11</sub><sup>−</sup>] and [H<sub>3</sub>F<sub>2</sub><sup>+</sup>][Sb<sub>2</sub>F<sub>11</sub><sup>−</sup>]. In both salts the anion is Sb<sub>2</sub>F<sub>11</sub><sup>−</sup>.<ref>{{cite journal | author = Mootz, D.; Bartmann, K. | title = The Fluoronium Ions H<sub>2</sub>F<sup>+</sup> and H<sub>3</sub>F<sub>2</sub><sup>+</sup>: Characterization by Crystal Structure Analysis | journal = [[Angewandte Chemie, International Edition in English]] | year = 1988 | volume = 27 | pages = 391–392 | doi = 10.1002/anie.198803911 | issue = 3}}</ref> As mentioned above, SbF<sub>6</sub><sup>−</sup> is classified as weakly basic; the larger monoanion Sb<sub>2</sub>F<sub>11</sub><sup>−</sup> would be expected to be still weaker. |
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===Comparison with other acids=== |
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The following values{{Citation needed|date=March 2009}} are based upon the [[Hammett acidity function]]. Acidity is indicated by large negative values of H<sub>0</sub>. |
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* Fluoroantimonic acid (1990) (H<sub>0</sub> Value = −31.3) |
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* [[Magic acid]] (1974) (H<sub>0</sub> Value = −19.2) |
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* [[Carborane superacid]] (1969) (H<sub>0</sub> Value = −18.0) |
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* [[Fluorosulfuric acid]] (1944) (H<sub>0</sub> Value = −15.1) |
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* [[Triflic acid]] (1940) (H<sub>0</sub> Value = −14.9) |
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==Applications== |
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{{Main|Superacid#Applications}} |
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This extraordinarily strong acid protonates nearly all [[organic compound]]s. In 1967, Bickel and Hogeveen showed that HF-SbF<sub>5</sub> will remove H<sub>2</sub> from [[isobutane]] and methane from [[neopentane]]:<ref>{{cite journal | author = Bickel, A. F.; Gaasbeek, C. J.; Hogeveen, H.; Oelderik, J. M.; Platteeuw, J. C. | title = Chemistry and spectroscopy in strongly acidic solutions: reversible reaction between aliphatic carbonium ions and hydrogen | journal = [[Chemical Communications]] | year = 1967 | volume = 1967 | pages = 634–5 | doi = 10.1039/C19670000634 | issue = 13}}</ref><ref>{{cite journal | author = Hogeveen, H.; Bickel, A. F. | title = Chemistry and spectroscopy in strongly acidic solutions: electrophilic substitution at alkane-carbon by protons | journal = [[Chemical Communications]] | year = 1967 | volume = 1967 | pages = 635–6 | doi = 10.1039/C19670000635 | issue = 13}}</ref> |
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:(CH<sub>3</sub>)<sub>3</sub>CH + H<sup>+</sup> → (CH<sub>3</sub>)<sub>3</sub>C<sup>+</sup> + H<sub>2</sub> |
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:(CH<sub>3</sub>)<sub>4</sub>C + H<sup>+</sup> → (CH<sub>3</sub>)<sub>3</sub>C<sup>+</sup> + CH<sub>4</sub> |
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==Safety== |
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HF-SbF<sub>5</sub> is rapidly and explosively decomposed by water. It reacts with virtually all known solvents.<ref name=Olah/> [[Solvent]]s that have been proven to be compatible with HF-SbF<sub>5</sub> are [[sulfuryl chloride fluoride|SO<sub>2</sub>ClF]] and liquefied [[sulfur dioxide]]. [[Chlorofluorocarbon]]s have also been used as solvents. Containers for |
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HF-SbF<sub>5</sub> are made of [[Polytetrafluoroethylene|PTFE]]. |
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==See also== |
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* [[Fluoroboric acid]] |
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* [[Fluorosulfuric acid]] |
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==References== |
==References== |
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{{Reflist}} |
{{Reflist}} |
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== See also == |
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[[Category:Antimony compounds]] |
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*[[Lithium oxide]] |
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[[Category:Fluorides]] |
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[[Category:Inorganic compounds]] |
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{{Lithium compounds}} |
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[[Category:Superacids]] |
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[[Category:Superbases]] |
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[[cs:Kyselina fluoroantimoničná]] |
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[[Category:Lithium compounds]] |
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[[de:Fluor-Antimonsäure]] |
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[[es:Ácido fluoroantimónico]] |
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[[fr:Acide fluoroantimonique]] |
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[[it:Acido fluoroantimonico]] |
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[[he:חומצה פלואורואנטימונית]] |
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[[ja:フルオロアンチモン酸]] |
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[[pl:Kwas fluoroantymonowy]] |
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[[pt:Ácido fluorantimônico]] |
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[[ro:Acid fluoroantimonic]] |
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[[sr:Fluoroantimonska kiselina]] |
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[[sh:Fluoroantimonska kiselina]] |
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[[fi:Fluoriantimonihappo]] |
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[[tr:Floroantimonik asit]] |
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[[zh:氟銻酸]] |