Pure 6 extreme formula1/23/2024 ![]() H 2SiF 6 → 2 HF + SiF 4 SiF 4 + 2 H 2O → 4 HF + SiO 2 Use This acid can be degraded to release HF thermally and by hydrolysis: Hydrogen fluoride is typically produced by the reaction between sulfuric acid and pure grades of the mineral fluorite: CaF 2 + H 2SO 4 → 2 HF + CaSO 4Ībout 20% of manufactured HF is a byproduct of fertilizer production, which generates hexafluorosilicic acid. A Hammett acidity function ( H 0) of −21 is obtained with antimony pentafluoride (SbF 5), forming fluoroantimonic acid. Like water, HF can act as a weak base, reacting with Lewis acids to give superacids. Which forms an extremely acidic liquid ( H 0 = −15.1). In liquid anhydrous HF, self-ionization occurs: 3 HF ⇌ H 2F + + HF − 2 However concentrated solutions are strong acids, because bifluoride anions are predominant, instead of ion pairs. When dilute, hydrofluoric acid behaves like a weak acid, unlike the other hydrohalic acids, due to the formation of hydrogen-bonded ion pairs. HF and H 2O similaritiesīoiling points of the hydrogen halides (blue) and hydrogen chalcogenides (red): HF and H 2O break trends.įreezing point of HF/ H 2O mixtures: arrows indicate compounds in the solid state.Īqueous solutions of HF are called hydrofluoric acid. H 2O with melting point −40 ☌ (−40 ☏), which is 44 ☌ (79 ☏) above the melting point of pure HF. Hydrogen fluoride forms a monohydrate HF. In contrast, the other hydrogen halides exhibit limiting solubilities in water. HF is miscible with water (dissolves in any proportion). Structure and reactions The structure of chains of HF in crystalline hydrogen fluoride. In 1771 Carl Wilhelm Scheele prepared the aqueous solution, hydrofluoric acid in large quantities, although hydrofluoric acid had been known in the glass industry before then.įrench chemist Edmond Frémy (1814–1894) is credited with discovering hydrogen fluoride (HF) while trying to isolate fluorine. The gas can also cause blindness by rapid destruction of the corneas. Hydrogen fluoride is an extremely dangerous gas, forming corrosive and penetrating hydrofluoric acid upon contact with moisture. Due to strong and extensive hydrogen bonding, it boils at near room temperature, much higher than other hydrogen halides. HF is also widely used in the petrochemical industry as a component of superacids. It is the principal industrial source of fluorine, often in the form of hydrofluoric acid, and is an important feedstock in the preparation of many important compounds including pharmaceuticals and polymers, e.g. It is a very poisonous, colorless gas or liquid that dissolves in water to yield an aqueous solution termed hydrofluoric acid. Hydrogen fluoride (fluorane) is an inorganic compound with chemical formula H F.
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