Wikipedia

Fluoroboric acid

Fluoroboric acid or tetrafluoroboric acid (archaically, fluoboric acid) is an inorganic compound with the simplified chemical formula H+[BF4]−. Unlike other strong acids like H2SO4 or HClO4, the pure (solvent free) tetrafluoroboric acid (more precisely, pure hydrogen tetrafluoroborate H[BF4]) does not exist. The term "fluoroboric acid" refers to a range of chemical compounds, depending on the solvent. The H+ in the simplified formula of fluoroboric acid represents the solvated proton. The solvent can be any suitable Lewis base. For instance, if the solvent is water, fluoroboric acid can be represented by the formula [H3O]+[BF4]− (oxonium tetrafluoroborate), although more realistically, several water molecules solvate the proton: [H(H2O)n]+[BF4]−. The ethyl ether solvate is also commercially available, where the fluoroboric acid can be represented by the formula [H((CH3CH2)2O)n]+[BF4]−, where n is most likely 2.

Fluoroboric acid
Canonical, skeletal formula of oxonium tetrafluoroborate
Oxonium tetrafluoroborate
Names
Preferred IUPAC name
Tetrafluoroboric acid[1]
Other names
  • Fluoboric acid
  • Fluoroboric acid
  • Hydrogen tetrafluoroborate
  • Oxonium tetrafluoroboranuide
  • Oxonium tetrafluoridoborate(1-)
  • Oxonium tetrafluoroborate
Identifiers
  • 14219-41-1 ([H3O]+[BF4]−) ☒N
  • 16872-11-0 (solvent free) checkY
  • 80628-99-5 ([H5O2]+[BF4]−) ☒N
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.037.165 Edit this at Wikidata
EC Number
  • 240-898-3
21702
MeSH Fluoroboric+acid
RTECS number
  • ED2685000
UNII
UN number 1775
  • InChI=1S/BF4H/c2-1(3,4)5/h2H ☒N
    Key: YKRRMQXMWYXWJW-UHFFFAOYSA-N ☒N
  • F[B-](F)(F)[FH+]
  • [H+].F[B-](F)(F)F
Properties
H[BF4]
Molar mass 87.81 g·mol−1
Appearance Colourless liquid
Melting point −90 °C (−130 °F; 183 K)
Boiling point 130 °C (266 °F; 403 K)
Acidity (pKa) ~1.8 (MeCN solution)[2]
Hazards
GHS labelling:
GHS05: Corrosive
Danger
H314
P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Safety data sheet (SDS) External MSDS
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

It is mainly produced as a precursor to other fluoroborate salts.[3] It is a strong acid. Fluoroboric acid is corrosive and attacks the skin. It is available commercially as a solution in water and other solvents such as diethyl ether. It is a strong acid with a weakly coordinating, non-oxidizing conjugate base.[2] It is structurally similar to perchloric acid, but lacks the hazards associated with oxidants.

Structure and production edit

Pure H[BF4] has been described as a "nonexistent compound", as a sufficiently "naked" proton is expected to abstract a fluoride from the tetrafluoroborate ion to give hydrogen fluoride and boron trifluoride:

H+[BF4]− → HF + BF3

The same holds true for the superacids that are known by the simplified formulas H[PF6] and H[SbF6].[4][5] However, a solution of BF3 in HF is highly acidic, having an approximate speciation of [H2F]+[BF4]− (fluoronium tetrafluoroborate) and a Hammett acidity function of −16.6 at 7 mol % BF3, easily qualifying as a superacid.[6] Although the solvent-free H[BF4] has not been isolated, its solvates are well characterized. These salts consist of protonated solvent as a cation, e.g., H3O+ and H5O+2, and the tetrahedral BF−4 anion. The anion and cations are strongly hydrogen-bonded.[7]

 
Subunit of crystal structure of [H3O]+[BF4]− highlighting the hydrogen bonding between the cation and the anion

Aqueous solutions of H[BF4] are produced by dissolving boric acid in aqueous hydrofluoric acid.[8][9] Three equivalents of HF react to give the intermediate boron trifluoride and the fourth gives fluoroboric acid:

B(OH)3 + 4 HF → H3O+ + BF−4 + 2 H2O

Anhydrous solutions can be prepared by treatment of aqueous fluoroboric acid with acetic anhydride.[10]

Acidity edit

The acidity of fluoroboric acid is complicated by the fact that its name refers to a range of different compounds, e.g. [H(CH3CH2)2O]+[BF4]− (dimethyloxonium tetrafluoroborate), [H3O]+[BF4]− (oxonium tetrafluoroborate), and HF·BF3 (hydrogen fluoride-boron trifluoride 1:1 adduct) – each with a different acidity. The aqueous pKa is quoted as −0.44.[3] Titration of [N((CH2)3CH3)4]+[BF4]− (tetrabutylammonium tetrafluoroborate) in acetonitrile solution indicates that H[BF4], i.e., HF·BF3, has a pKa of 1.6 in that solvent. Its acidity is thus comparable to that of fluorosulfonic acid.[2]

Applications edit

Fluoroboric acid is the principal precursor to fluoroborate salts, which are typically prepared by treating the metal oxides with fluoroboric acid. The inorganic salts are intermediates in the manufacture of flame-retardant materials and glazing frits, and in electrolytic generation of boron. H[BF4] is also used in aluminum etching and acid pickling.

Organic chemistry edit

H[BF4] is used as a catalyst for alkylations and polymerizations. In carbohydrate protection reactions, ethereal fluoroboric acid is an efficient and cost-effective catalyst for transacetalation and isopropylidenation reactions. Acetonitrile solutions cleave acetals and some ethers. Many reactive cations have been obtained using fluoroboric acid, e.g. tropylium tetrafluoroborate (C7H7+[BF4]−), triphenylcarbenium tetrafluoroborate (Ph3C]+[BF4]−), triethyloxonium tetrafluoroborate (Et3O]+[BF4]−), and benzenediazonium tetrafluoroborate ([PhN2]+[BF4]−).

Electroplating edit

Solutions of H[BF4] are used in the electroplating of tin and tin alloys. In this application, methanesulfonic acid is displacing the use of H[BF4].[11] Fluoroboric acid is also used for high-speed electroplating of copper in fluoroborate baths.[12]

Safety edit

H[BF4] is toxic and attacks skin and eyes. It attacks glass.[3] It hydrolyzes, releasing corrosive, volatile hydrogen fluoride.[11]

Other fluoroboric acids edit

A series of fluoroboric acids is known in aqueous solutions. The series can be presented as follows:[13]

  • H+[B(OH)4]− (hydrogen tetrahydroxyborate) (not a fluoroboric acid)
  • H+[BF(OH)3]− (hydrogen fluoro(trihydroxy)borate)
  • H+[BF2(OH)2]− (hydrogen difluoro(dihydroxy)borate)
  • H+[BF3(OH)]− (hydrogen trifluoro(hydroxy)borate)
  • H+[BF4]− (hydrogen tetrafluoroborate)

See also edit

References edit

  1. ^ IUPAC. "Nomenclature of Inorganic Chemistry". Retrieved 2021-04-08.
  2. ^ a b c Kütt, A., et al., "Equilibrium Acidities of Superacids", J. Org. Chem. 2010, volume 76, pp. 391-395. doi:10.1021/jo101409p
  3. ^ a b c Gregory K. Friestad, Bruce P. Branchaud "Tetrafluoroboric Acid" E-Eros Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rt035
  4. ^ Juhasz, Mark; Hoffmann, Stephan; Stoyanov, Evgenii; Kim, Kee-Chan; Reed, Christopher A. (2004-10-11). "The Strongest Isolable Acid". Angewandte Chemie International Edition. 43 (40): 5352–5355. doi:10.1002/anie.200460005. ISSN 1433-7851. PMID 15468064.
  5. ^ Reed, Christopher A. (2005). "Carborane acids. New "strong yet gentle" acids for organic and inorganic chemistry" (PDF). Chem. Commun. (13): 1669–1677. doi:10.1039/B415425H. ISSN 1359-7345. PMID 15791295.
  6. ^ Olah, George A.; Surya Prakash, G. K.; Sommer, Jean; Molnar, Arpad (2009-02-03). Superacid chemistry. Olah, George A. (George Andrew), 1927-2017,, Olah, George A. (George Andrew), 1927-2017. (2nd ed.). Hoboken, N.J. ISBN 9780471596684. OCLC 191809598.{{cite book}}: CS1 maint: location missing publisher (link)
  7. ^ Mootz, D.; Steffen, M. "Crystal structures of acid hydrates and oxonium salts. XX. Oxonium tetrafluoroborates H3OBF4, [H5O2]BF4, and [H(CH3OH)2]BF4", Zeitschrift für Anorganische und Allgemeine Chemie 1981, vol. 482, pp. 193-200. doi:10.1002/zaac.19814821124
  8. ^ Brotherton, R. J.; Weber, C. J.; Guibert, C. R.; Little, J. L. "Boron Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a04_309. ISBN 978-3527306732.
  9. ^ Flood, D. T. (1933). "Fluorobenzene" (PDF). Organic Syntheses. 13: 46; Collected Volumes, vol. 2, p. 295.
  10. ^ Wudl, F.; Kaplan, M. L., "2,2′-Bi-L,3-Dithiolylidene (Tetrathiafulvalene, TTF) and its Radical Cation Salts" Inorg. Synth. 1979, vol. 19, 27. doi:10.1002/9780470132500.ch7
  11. ^ a b Balaji, R.; Pushpavanam, Malathy (2003). "Methanesulphonic acid in electroplating related metal finishing industries". Transactions of the Imf. 81 (5): 154–158. doi:10.1080/00202967.2003.11871526. S2CID 91584456.
  12. ^ Barauskas, Romualdas "Ron" (January 1, 2000). "Copper plating". Metal Finishing. 98 (1): 234–247. doi:10.1016/S0026-0576(00)80330-X. ISSN 0026-0576. Retrieved July 21, 2022.
  13. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

Further reading edit

  • Albert, R.; Dax, K.; Pleschko, R.; Stütz, A. E. (1985). "Tetrafluoroboric acid, an efficient catalyst in carbohydrate protection and deprotection reactions". Carbohydrate Research. 137: 282–290. doi:10.1016/0008-6215(85)85171-5.
  • Bandgar, B. P.; Patil, A. V.; Chavan, O. S. (2006). "Silica supported fluoroboric acid as a novel, efficient and reusable catalyst for the synthesis of 1,5-benzodiazepines under solvent-free conditions". Journal of Molecular Catalysis A: Chemical. 256 (1–2): 99–105. doi:10.1016/j.molcata.2006.04.024.
  • Heintz, R. A.; Smith, J. A.; Szalay, P. S.; Weisgerber, A.; Dunbar, K. R. (2002). Homoleptic Transition Metal Acetonitrile Cations with Tetrafluoroborate or Trifluoromethanesulfonate Anions. Inorganic Syntheses. Vol. 33. pp. 75–83. doi:10.1002/0471224502. ISBN 9780471208259.
  • Housecroft, C. E.; Sharpe, A. G. (2004). Inorganic Chemistry (2nd ed.). Prentice Hall. p. 307. ISBN 978-0-13-039913-7.
  • Meller, A. (1988). "Boron". Gmelin Handbook of Inorganic Chemistry. Vol. 3. New York: Springer-Verlag. pp. 301–310.
  • Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds (1st ed.). Boca Raton: CRC Press. p. 1203. ISBN 9780849386718.
  • Wamser, C. A. (1948). "Hydrolysis of Fluoboric Acid in Aqueous Solution". Journal of the American Chemical Society. 70 (3): 1209–1215. doi:10.1021/ja01183a101.
  • Wilke-Dörfurt, E.; Balz, G. (1927). "Zur Kenntnis der Borfluorwasserstoffsäure und ihrer Salze". Zeitschrift für Anorganische und Allgemeine Chemie. 159 (1): 197–225. doi:10.1002/zaac.19271590118.

External links edit

Retrieved from "https://en.wikipedia.org/w/index.php?title=Fluoroboric_acid&oldid=1187485942"