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Login Register DeutschEnglishFrançaisEspañol Home Encyclopedia Fluoroboric_acid Fluoroboric acid Fluoroboric acid IUPAC name Tetrafluoroboric acid Other names Fluoroboric acid; Hydrogen Tetrafluoroborate; Hydrofluoroboric acid; Borofluoric acid Identifiers CAS number 16872-11-0 RTECS number ED2685000 Properties Molecular formula HBF4 Molar mass 87.8126 g/mol Appearance Clear liquid Density 1.36g/mL, liquid; 3.0 g/l, gas Melting point -90 °C Boiling point 130 °C Solubility in water Miscible Acidity (pKa) -0.4 Structure Crystal structure N/A Hazards MSDS External MSDS Main hazards Corrosive R-phrases 34 S-phrases 26-36/37/38-45 Flash point nonflammable Related Compounds Other anions Hexafluorophosphoric acid, Triflic acid Related compounds Potassium fluoroborate, nitrosonium fluoroborate, Hexafluorophosphate, Hydrogen fluoride Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references Fluoroboric acid is the chemical compound with the formula HBF4. It is the conjugate acid of tetrafluoroborate. It is available commercially as a solution in water and other solvents such as diethyl ether. With a strength comparable to nitric acid, fluoroboric acid is a strong acid with a weakly coordinating, non-oxidizing conjugate base. Additional recommended knowledge How to quickly check pipettes? Better weighing performance in 6 easy steps Daily Sensitivity Test Contents 1 Production 1.1 Salts 2 Applications 2.1 Organic chemistry 2.2 Galvanic cells 2.3 Metal plating 3 Safety 4 References Production Pure fluoroboric acid is unknown. Aqueous solutions of 45-50% HBF4 are produced by combining technical grade[citation needed] boric acid and hydrofluoric acid in aqueous solution at room temperature. Three equivalents of HF react to give the intermediate boron trifluoride and the fourth gives fluoroboric acid. B(OH)3 + 4 HF → H3O+ + BF4- + 2 H2O Aqueous solutions of fluoroboric acid can also be prepared by treating impure hexafluorosilicic acid with solid boric acid followed by removal of precipitated silicon dioxide.[citation needed] Anhydrous solutions can be prepared by treatment with acetic anhydride.[1] Salts Main article: Tetrafluoroborate Fluoroboric acid is the principal precursor to fluoroborate salts, which are typically prepared by acid-base reactions. The inorganic salts are intermediates in the manufacture of flame-retardant materials, glazing frits, and in electrolytic generation of boron. HBF4 is also used in aluminum etching and acid pickling. Applications Organic chemistry HBF4 is used as a catalyst in 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, while neat[citation needed] fluoroboric acid removes tert-butoxycarbonyl groups. Galvanic cells Aqueous HBF4 is used as an electrolyte in galvanic cell oxygen sensor systems which consist of an anode, cathode, and oxygen-permeable membrane. The solution of HBF4 is able to dissolve lead(II) oxide from the anode in the form of lead tetrafluoroborate while leaving the rest of the sys Metal plating A mixture of CrO3, HBF4, and sulfonic acids in conjunction with a cathode treatment give tin-plated steel. Tin(I) fluoroborate/fluoroboric acid mixtures and organic reagents are used as the electrolyte in the cathode treatment of the tin plating process. Similar processes of electrodeposition and electrolytic stripping are used to obtain specific metal alloys. Safety Aqueous fluoroboric acid is corrosive and will burn skin or eyes. Lab work should be conducted in a hood or well ventilated area. References Albert, R.; Dax, K.; Pleschko, R.; Stutz, A. E. Carbohydr. Res. 1985, 137, 282-290. Bandgar, B. P.; Patil, A. V.; Chavan, O.S. J. Mol. Catal. A: Chem. 2006, 256, 99-105. Heintz, R. A.; Smith, J. A.; Szalay, P. S.; Weisgerber, A.; Dunbar, K. R. Inorg. Synth. 2002, 33, 75. Housecroft, C E.; Sharpe, A. G. Inorganic Chemistry. 2nd ed. New York: Pearson Prentice Hall, 2005. 307. Meller, A. Gmelin Handbook of Inorganic Chemistry: Boron. Vol. 3. New York: Springer-Verlag, 1988. 301-310. Perry, D. L.; Phillips, S. L. Handbook of Inorganic Compounds. Boca Raton: CRC Press, 1995. 1203. Wamser, C. A. J. Am. Chem. Soc. 1948, 70, 1209-1215. Wilke-Doerfurt, E.; Balz, G. Z. Z. Anorg. Allg. Chem. 1927, 159, 224. Categories: Acids | Fluorine compounds | Boron compounds This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Fluoroboric_acid". A list of authors is available in Wikipedia. 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