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fluoboric acid - translation to greek
![[H3O]+[BF4]−}} highlighting the hydrogen bonding between the cation and the anion](https://commons.wikimedia.org/wiki/Special:FilePath/H3OBF4subunit.png?width=200 "[H3O]+[BF4]−}} highlighting the hydrogen bonding between the cation and the anion")
![Tartaric acid crystals drawn as if seen through an [[optical microscope]]](https://commons.wikimedia.org/wiki/Special:FilePath/TartrateCrystal.svg?width=200 "Tartaric acid crystals drawn as if seen through an [[optical microscope]]")
Definition
Wikipedia
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) 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.
It is mainly produced as a precursor to other fluoroborate salts. 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. It is structurally similar to perchloric acid, but lacks the hazards associated with oxidants.
