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Is it twenty quadrillion or twenty quintillion times stronger than sulfuric acid? WP:V! Hyenaste 06:13, 1 March 2006 (UTC)
Twenty QUINtillion. At least that's what Guiness claimed, and what other websites listed as well. -anonymous user
This page conflicts with superacid. Superacid says fluroanitmonic acid is only 1016 times as strong as sulfuric acid, but this page says it is 2 times 1019 times as strong. Should a contradiction be flagged on the two pages? Mathwhiz90601 03:00, 4 February 2007 (UTC)
How is this stored? It seems worth answering on the main page, if anyone knows. Amber388 03:44, 13 September 2006 (UTC)
It can be stored in teflon containers. Teflon is the single strongest carbon-fluorine bond in chemistry. Otherwise, even messing with fluoroantimonic acid, as much as even exposing it to light, might cause some serious problems. — Preceding unsigned comment added by IrisFall ( talk • contribs) 03:57, 15 April 2017 (UTC)
Is this acid merely strong or is it corrosive as well? 129.44.209.60 21:25, 26 October 2006 (UTC)
It says that Fluoroantimonic acid is stored in teflon. And, I know what one of you were talking about when you brought up another acid that was extremely powerful, and not very corrosive. It's called a carborane acid. But fluoroantimonic acid is pretty much the most corrosive substance known.(UTC)
It says..."It reacts with virtually all known solvents." What's the example for which this acid does not react with? -- HappyCamper 00:15, 30 October 2006 (UTC).
Does anyone know where I can get this stuff or the ingredients? Thx. -- 74.134.8.244 19:15, 26 May 2007 (UTC)
Yeah it's extremely lethal. Basically any exposure of the acid to the human body via breathing or skin contact is going to be too corrosive and too toxic that it is lethal with no countermeasure to survive. The acid can also eat through glass and many other types of containment. It shouldn't be handled directly by humans. I'm pretty sure the chemical engineers use extended pole grippers and mechanical grippers to indirectly handle it and they only handle it if they have to. 70.127.116.20 ( talk) — Preceding undated comment added 08:25, 28 April 2015 (UTC)
As I understand it, the sentence that was just reverted is trying to say "when you react the superacid with a hydrocarbon, you get hydrogen gas expelled from the system, with the hydrocarbon ultimately losing a hydrogen to become a carbocation". There are many words for that, but I don't think "protonation" is one of them. Maybe the article on protonation is incorrect, but here is an excerpt: "Upon protonating a substrate, the mass and the charge of the species each increase by one unit." It seems to me that the hydrocarbon doesn't *receive* the extra proton - the net reaction seems to involve *losing* a hydrogen it already had. (okay, the superacid is obviously not a base so I can see why you would object to using the word "deprotonation" here, but surely "protonation" is even more misleading? seems to me this reaction is kind of analogous to a hydride group leaving the carbon, rather than what you would call a "protonation") ugen64 06:21, 16 November 2007 (UTC)
I'd say the first step is indeed a protonation, followed by the elimination of H2. Usage is correct. --
Rifleman 82
11:12, 16 November 2007 (UTC)
Will it dissolve noble metals like Gold or Platinum —Preceding unsigned comment added by 84.69.220.228 ( talk) 18:59, 18 March 2008 (UTC)
I doubt it. It'd certainly remove the electrons binding the gold together. But there's nothing to shepherd the gold out, since the fluorines are all tightly bonded. A tiny amount of gold would be dissolved, as with nitric acid, but it wouldn't be removed from the strong attractive forces of the rest of the gold. -- Ytaker ( talk) 18:30, 16 October 2008 (UTC)
Yeah, it can easily dissolve gold and platinum. Evan aqua regia, which is thousand times weaker than it can dissolve gold or platinum. — Preceding unsigned comment added by 2401:4900:3627:8D3C:FD69:FC72:6E5E:581A ( talk) 15:59, 31 August 2019 (UTC)
What is the pH of HSbF6? Professor M. Fiendish, Esq. 02:23, 3 September 2009 (UTC)
- The pH is -30. Aryan Gaikwad — Preceding unsigned comment added by 120.61.3.230 ( talk) 02:42, 26 November 2013 (UTC)
I question the pH value given: pH is a function of concentration (e.g., 0.1 Molar solution of HCl has a pH of 1.). Also, unless I messed up my math, this implies something like 10^30 moles of H+ per liter of solution (which I sort of think is physically impossible). Scienda ( talk) —Preceding undated comment added 01:31, 8 April 2018 (UTC)
I thing HAuF6 will be even more acidic than HSbF6, since the ionization energy of [AuF6-(10 eV) is much greater than that of [SbF6-(6 eV). Just some thoughts...-- Anoop.m ( talk) 16:20, 28 September 2009 (UTC)
How about HIF8, based on iodine heptafluoride? 2.229.113.29 ( talk) 12:05, 27 November 2011 (UTC)
Forgive me if I'm totally working on the wrong principles, but here's an idea: HF + CuF11 = HCuF12. If my baseless speculation is right, the icosahedron shape of the fluorine atoms will make it very difficult for the protons to reattach once they're off. Will the highly charged ion of Cu11+ do much? —Preceding unsigned comment added by 72.178.12.19 ( talk) 04:50, 29 September 2009 (UTC)
Ahem, the so-called helium hydride ion is not an acid, any more than the hydroxonium (H3O+) ion is an acid in its own right, but merely a proton carrier. 86.146.199.9 ( talk) 19:36, 30 October 2009 (UTC)
Has anyone tried that? Stonemason89 ( talk) 19:33, 20 August 2010 (UTC)
I just learned from Proton_affinity_(data_page) that xenon has a higher proton affinity than HF. Since fluoronium cations are already known, it seems like the answer may be "yes" for xenon, although xenonium cations wouldn't be particularly stable even if we could create them. Stonemason89 ( talk) 23:42, 22 August 2010 (UTC)
No. See [1]. Protons hop from anion to anion in superacids via the Grotthuss mechanism, just as they do in water. This accounts for ionic conductance in liquid fluoroantimonic acid, without having to postulate real H+ ions of the sort one finds in hydrogen plasmas. S B H arris 00:46, 27 February 2011 (UTC)
According to the article itself, The salts tend to crytallize in dimers with briding halogens, something like digold hexachloride, save that antimony has more valence, so you get diantimony-fluoride-11 anions, with 3c-2e bonds between Sb's and a single bridging fluorine between them, sharing a single set of bonding electrons. The two related products have been crystallised from HF-SbF5 mixtures, analyzed by single crystal X-ray crystallography, show the formulas [H2F+][Sb2F11−] and [H3F2+][Sb2F11−]. In both salts the anion is Sb2F11−. Go figure. Here the energetics to go to FHF+ and FHFHF+ are so great that they leave the Sb's sharing one fluorine. Still, it's another indication of how much more that H+ would rather be in a 2-D fluorine sandwich or chain, than floating around with nothing. S B H arris 09:39, 27 February 2011 (UTC)
I think HSbCl6 would be even stronger because HF is a part of fluoroantimonic acid and HF itself isn't even included as a strong acid.HCl is strong though some folks said Hcl isn't as corrosive. Just saying. — Preceding unsigned comment added by 76.124.224.179 ( talk) 23:16, 4 July 2012 (UTC)
pKa is frequently used with anhydrous solvents, most notably in the famous Bordwell table of pKas in DMSO. -- Ben ( talk) 10:04, 6 July 2012 (UTC)
I doubt that this material decomposes in water. What is it supposed to do? SbF6- is reasonably happy in water. Yes, the reaction would be exothermic, but that detail is irrelevant. One could say that H2SO4 decomposes in water since the molecule (HO)2SO2 converts to hydronium+SO3(OH)-, but we dont use decomposition in that way.-- Smokefoot ( talk) 13:12, 30 September 2012 (UTC)
I think the chemical formula was horribly wrong, it should have been HSbF6. I fixed it. That other chemical be called dihydrogen heptafluoroantimonate, and it could not be made from hydrogen fluoride and antimony pentafluoride. Scientific Alan 2 (Click here to talk) (What have I done?) (Me) 14:04, 28 May 2013 (UTC)
It seems that there is no melting point of this compound mentioned in article.-- 5.15.187.229 ( talk) 10:37, 11 November 2015 (UTC)
Actually, there are stronger acids than fluoroantimonic acid since 2013. See /info/en/?search=Carborane_acid. Thus the article should be edited as it says that this is the strongest acid. Apelsinas128 ( talk) 12:26, 15 May 2017 (UTC)
Actually, it they say it's the strongest because its more corrosive than Carborane — Preceding unsigned comment added by Fire blazr ( talk • contribs) 23:11, 5 August 2017 (UTC)
Carborane acid is 1 million times stronger than sulfuric acid, but fluoroantimonic acid is 10 QUADRILLION times stronger than sulfuric acid. So no, carborane acid is NOT stronger than fluoroantimonic acid. ScamsAreHorrible172 ( talk) 07:02, 12 October 2017 (UTC)
Fluoroantimonic acid is the second strongest superacid, second only to helonium. This should be completely wrong statement. I believe many carborane super acids are stronger than fluoroantimonic acid. Not sure about their silicon and germanium analogues and azaboranes. Neonium (HNe+) should also be much much stronger than HSbF6. Argonium and kryptonium should also be even stronger. Anoop Manakkalath ( talk) 00:13, 8 December 2022 (UTC)
What is this "hydrofluoric solution" that is mentioned in the Safety section? There is no article by that name, while "hydrofluoric" redirects to hydrogen fluoride, and the only solution of that (using water) is the superacid known as hydrofluoric acid. Does this mean that "fluoroantimonic acid in a hydrofluoric solution" means mixing fluoroantimonic acid in hydrofluoric acid instead of water (which would be an aqueous solution)? MarqFJA87 ( talk) 21:34, 6 September 2017 (UTC)
This stuff seems pretty horrible. Is it actually used for anything, other than as a chemical curiosity? KarlM ( talk) 09:54, 25 March 2018 (UTC)
You can also store it (saw video of shipping container from Sigma-Aldrich) in perfluoroalkoxy alkane containers, (PFA, like the PFA everyone screams about that is used in Teflon pans). 2600:1700:4CA1:3C80:4877:C0B6:1088:FF80 ( talk) 20:00, 2 January 2021 (UTC)
Why is the space-filling image inconsistent with the other two in the infobox? (one hydrogen atom vs two hydrogen atoms). IronGargoyle ( talk) 20:14, 29 May 2021 (UTC)
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Is it twenty quadrillion or twenty quintillion times stronger than sulfuric acid? WP:V! Hyenaste 06:13, 1 March 2006 (UTC)
Twenty QUINtillion. At least that's what Guiness claimed, and what other websites listed as well. -anonymous user
This page conflicts with superacid. Superacid says fluroanitmonic acid is only 1016 times as strong as sulfuric acid, but this page says it is 2 times 1019 times as strong. Should a contradiction be flagged on the two pages? Mathwhiz90601 03:00, 4 February 2007 (UTC)
How is this stored? It seems worth answering on the main page, if anyone knows. Amber388 03:44, 13 September 2006 (UTC)
It can be stored in teflon containers. Teflon is the single strongest carbon-fluorine bond in chemistry. Otherwise, even messing with fluoroantimonic acid, as much as even exposing it to light, might cause some serious problems. — Preceding unsigned comment added by IrisFall ( talk • contribs) 03:57, 15 April 2017 (UTC)
Is this acid merely strong or is it corrosive as well? 129.44.209.60 21:25, 26 October 2006 (UTC)
It says that Fluoroantimonic acid is stored in teflon. And, I know what one of you were talking about when you brought up another acid that was extremely powerful, and not very corrosive. It's called a carborane acid. But fluoroantimonic acid is pretty much the most corrosive substance known.(UTC)
It says..."It reacts with virtually all known solvents." What's the example for which this acid does not react with? -- HappyCamper 00:15, 30 October 2006 (UTC).
Does anyone know where I can get this stuff or the ingredients? Thx. -- 74.134.8.244 19:15, 26 May 2007 (UTC)
Yeah it's extremely lethal. Basically any exposure of the acid to the human body via breathing or skin contact is going to be too corrosive and too toxic that it is lethal with no countermeasure to survive. The acid can also eat through glass and many other types of containment. It shouldn't be handled directly by humans. I'm pretty sure the chemical engineers use extended pole grippers and mechanical grippers to indirectly handle it and they only handle it if they have to. 70.127.116.20 ( talk) — Preceding undated comment added 08:25, 28 April 2015 (UTC)
As I understand it, the sentence that was just reverted is trying to say "when you react the superacid with a hydrocarbon, you get hydrogen gas expelled from the system, with the hydrocarbon ultimately losing a hydrogen to become a carbocation". There are many words for that, but I don't think "protonation" is one of them. Maybe the article on protonation is incorrect, but here is an excerpt: "Upon protonating a substrate, the mass and the charge of the species each increase by one unit." It seems to me that the hydrocarbon doesn't *receive* the extra proton - the net reaction seems to involve *losing* a hydrogen it already had. (okay, the superacid is obviously not a base so I can see why you would object to using the word "deprotonation" here, but surely "protonation" is even more misleading? seems to me this reaction is kind of analogous to a hydride group leaving the carbon, rather than what you would call a "protonation") ugen64 06:21, 16 November 2007 (UTC)
I'd say the first step is indeed a protonation, followed by the elimination of H2. Usage is correct. --
Rifleman 82
11:12, 16 November 2007 (UTC)
Will it dissolve noble metals like Gold or Platinum —Preceding unsigned comment added by 84.69.220.228 ( talk) 18:59, 18 March 2008 (UTC)
I doubt it. It'd certainly remove the electrons binding the gold together. But there's nothing to shepherd the gold out, since the fluorines are all tightly bonded. A tiny amount of gold would be dissolved, as with nitric acid, but it wouldn't be removed from the strong attractive forces of the rest of the gold. -- Ytaker ( talk) 18:30, 16 October 2008 (UTC)
Yeah, it can easily dissolve gold and platinum. Evan aqua regia, which is thousand times weaker than it can dissolve gold or platinum. — Preceding unsigned comment added by 2401:4900:3627:8D3C:FD69:FC72:6E5E:581A ( talk) 15:59, 31 August 2019 (UTC)
What is the pH of HSbF6? Professor M. Fiendish, Esq. 02:23, 3 September 2009 (UTC)
- The pH is -30. Aryan Gaikwad — Preceding unsigned comment added by 120.61.3.230 ( talk) 02:42, 26 November 2013 (UTC)
I question the pH value given: pH is a function of concentration (e.g., 0.1 Molar solution of HCl has a pH of 1.). Also, unless I messed up my math, this implies something like 10^30 moles of H+ per liter of solution (which I sort of think is physically impossible). Scienda ( talk) —Preceding undated comment added 01:31, 8 April 2018 (UTC)
I thing HAuF6 will be even more acidic than HSbF6, since the ionization energy of [AuF6-(10 eV) is much greater than that of [SbF6-(6 eV). Just some thoughts...-- Anoop.m ( talk) 16:20, 28 September 2009 (UTC)
How about HIF8, based on iodine heptafluoride? 2.229.113.29 ( talk) 12:05, 27 November 2011 (UTC)
Forgive me if I'm totally working on the wrong principles, but here's an idea: HF + CuF11 = HCuF12. If my baseless speculation is right, the icosahedron shape of the fluorine atoms will make it very difficult for the protons to reattach once they're off. Will the highly charged ion of Cu11+ do much? —Preceding unsigned comment added by 72.178.12.19 ( talk) 04:50, 29 September 2009 (UTC)
Ahem, the so-called helium hydride ion is not an acid, any more than the hydroxonium (H3O+) ion is an acid in its own right, but merely a proton carrier. 86.146.199.9 ( talk) 19:36, 30 October 2009 (UTC)
Has anyone tried that? Stonemason89 ( talk) 19:33, 20 August 2010 (UTC)
I just learned from Proton_affinity_(data_page) that xenon has a higher proton affinity than HF. Since fluoronium cations are already known, it seems like the answer may be "yes" for xenon, although xenonium cations wouldn't be particularly stable even if we could create them. Stonemason89 ( talk) 23:42, 22 August 2010 (UTC)
No. See [1]. Protons hop from anion to anion in superacids via the Grotthuss mechanism, just as they do in water. This accounts for ionic conductance in liquid fluoroantimonic acid, without having to postulate real H+ ions of the sort one finds in hydrogen plasmas. S B H arris 00:46, 27 February 2011 (UTC)
According to the article itself, The salts tend to crytallize in dimers with briding halogens, something like digold hexachloride, save that antimony has more valence, so you get diantimony-fluoride-11 anions, with 3c-2e bonds between Sb's and a single bridging fluorine between them, sharing a single set of bonding electrons. The two related products have been crystallised from HF-SbF5 mixtures, analyzed by single crystal X-ray crystallography, show the formulas [H2F+][Sb2F11−] and [H3F2+][Sb2F11−]. In both salts the anion is Sb2F11−. Go figure. Here the energetics to go to FHF+ and FHFHF+ are so great that they leave the Sb's sharing one fluorine. Still, it's another indication of how much more that H+ would rather be in a 2-D fluorine sandwich or chain, than floating around with nothing. S B H arris 09:39, 27 February 2011 (UTC)
I think HSbCl6 would be even stronger because HF is a part of fluoroantimonic acid and HF itself isn't even included as a strong acid.HCl is strong though some folks said Hcl isn't as corrosive. Just saying. — Preceding unsigned comment added by 76.124.224.179 ( talk) 23:16, 4 July 2012 (UTC)
pKa is frequently used with anhydrous solvents, most notably in the famous Bordwell table of pKas in DMSO. -- Ben ( talk) 10:04, 6 July 2012 (UTC)
I doubt that this material decomposes in water. What is it supposed to do? SbF6- is reasonably happy in water. Yes, the reaction would be exothermic, but that detail is irrelevant. One could say that H2SO4 decomposes in water since the molecule (HO)2SO2 converts to hydronium+SO3(OH)-, but we dont use decomposition in that way.-- Smokefoot ( talk) 13:12, 30 September 2012 (UTC)
I think the chemical formula was horribly wrong, it should have been HSbF6. I fixed it. That other chemical be called dihydrogen heptafluoroantimonate, and it could not be made from hydrogen fluoride and antimony pentafluoride. Scientific Alan 2 (Click here to talk) (What have I done?) (Me) 14:04, 28 May 2013 (UTC)
It seems that there is no melting point of this compound mentioned in article.-- 5.15.187.229 ( talk) 10:37, 11 November 2015 (UTC)
Actually, there are stronger acids than fluoroantimonic acid since 2013. See /info/en/?search=Carborane_acid. Thus the article should be edited as it says that this is the strongest acid. Apelsinas128 ( talk) 12:26, 15 May 2017 (UTC)
Actually, it they say it's the strongest because its more corrosive than Carborane — Preceding unsigned comment added by Fire blazr ( talk • contribs) 23:11, 5 August 2017 (UTC)
Carborane acid is 1 million times stronger than sulfuric acid, but fluoroantimonic acid is 10 QUADRILLION times stronger than sulfuric acid. So no, carborane acid is NOT stronger than fluoroantimonic acid. ScamsAreHorrible172 ( talk) 07:02, 12 October 2017 (UTC)
Fluoroantimonic acid is the second strongest superacid, second only to helonium. This should be completely wrong statement. I believe many carborane super acids are stronger than fluoroantimonic acid. Not sure about their silicon and germanium analogues and azaboranes. Neonium (HNe+) should also be much much stronger than HSbF6. Argonium and kryptonium should also be even stronger. Anoop Manakkalath ( talk) 00:13, 8 December 2022 (UTC)
What is this "hydrofluoric solution" that is mentioned in the Safety section? There is no article by that name, while "hydrofluoric" redirects to hydrogen fluoride, and the only solution of that (using water) is the superacid known as hydrofluoric acid. Does this mean that "fluoroantimonic acid in a hydrofluoric solution" means mixing fluoroantimonic acid in hydrofluoric acid instead of water (which would be an aqueous solution)? MarqFJA87 ( talk) 21:34, 6 September 2017 (UTC)
This stuff seems pretty horrible. Is it actually used for anything, other than as a chemical curiosity? KarlM ( talk) 09:54, 25 March 2018 (UTC)
You can also store it (saw video of shipping container from Sigma-Aldrich) in perfluoroalkoxy alkane containers, (PFA, like the PFA everyone screams about that is used in Teflon pans). 2600:1700:4CA1:3C80:4877:C0B6:1088:FF80 ( talk) 20:00, 2 January 2021 (UTC)
Why is the space-filling image inconsistent with the other two in the infobox? (one hydrogen atom vs two hydrogen atoms). IronGargoyle ( talk) 20:14, 29 May 2021 (UTC)