hydrogen fluoride oor Indonesies
hydrogen fluoride
en
(chemistry) a colourless fuming liquid or gas, having a molecular formula of HF; it dissolves in water to form hydrofluoric acid and has many industrial uses including the production of teflon and the refining of uranium; it corrodes skin, flesh and bone, and any skin contact must be avoided
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Asam fluorida
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chemical compound
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Hexafluorosilicic acid can release hydrogen fluoride when evaporated, so it has similar risks.
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The direct reaction of hydrogen with fluorine and chlorine gives hydrogen fluoride and hydrogen chloride, respectively.
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Many commercially important organic compounds are fluorinated electrochemically using hydrogen fluoride as the source of fluorine.
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The potassium bifluoride is needed because anhydrous hydrogen fluoride does not conduct electricity.
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Hydrogen fluoride is a highly dangerous gas, forming corrosive and penetrating hydrofluoric acid upon contact with moisture.
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Hydrogen fluoride is itself an example of a non-systematic name of this nature.
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Hydrogen fluoride boils near room temperature, much higher than other hydrogen halides.
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This is treated with 93% sulfuric acid to produce calcium sulfate, hydrogen fluoride (HF) and phosphoric acid.
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In the latter method, actinium metal is treated with hydrogen fluoride vapors at 700 °C in an all-platinum setup.
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Many of the binary compounds that it forms (called fluorides) are themselves highly toxic, including soluble fluorides and especially hydrogen fluoride.
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On passing hydrogen fluoride gas (in excess) through the salt, ammonium fluoride absorbs the gas to form the addition compound ammonium bifluoride.
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Upon contact with moisture, including tissue, hydrogen fluoride immediately converts to hydrofluoric acid, which is highly corrosive and toxic, and requires immediate medical attention upon exposure.
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The hydrogen halides are diatomic molecules with no tendency to ionize in the gas phase (although liquified hydrogen fluoride is a polar solvent somewhat similar to water).
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This chemical was synthesized by mixing argon and hydrogen fluoride on a caesium iodide surface at 8 K (−265 °C), and exposing the mixture to ultraviolet radiation.
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Some materials are dangerous to use as a gas; for example, fluorine is highly reactive and industrial chemistry requiring fluorine often uses hydrogen fluoride (or hydrofluoric acid) instead.
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Antimony pentafluoride is prepared by the reaction of antimony pentachloride with anhydrous hydrogen fluoride: SbCl5 + 5 HF → SbF5 + 5 HCl It can also be prepared from antimony trifluoride and fluorine.
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Nitrogen trifluoride (NF3, first prepared in 1928) is a colourless and odourless gas that is thermodynamically stable, and most readily produced by the electrolysis of molten ammonium fluoride dissolved in anhydrous hydrogen fluoride.
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The overall process is one of hydrometallurgy and begins with a leaching step; in which the ore is treated with hydrofluoric acid and sulfuric acid to produce water-soluble hydrogen fluorides, such as the heptafluorotantalate.
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The infrared spectrum of the resulting gas mixture shows that it definitely contains chemical bonds, albeit very weak ones; thus, it is argon fluorohydride, and not a supermolecule or a mixture of argon and hydrogen fluoride.
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In the sublimation, the salt decomposes to ammonia and hydrogen fluoride, and the two gases can recombine to give ammonium fluoride, i.e. the reaction is reversible: F ⇌ NH3 + HF This substance is commonly called "commercial ammonium fluoride".
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High-purity silver(I) fluoride can be produced by the heating of silver carbonate to 310 °C under a hydrogen fluoride environment, in a platinum tube: Ag2CO3 + 2HF → 2AgF + H2O + CO2 Laboratory routes to the compound typically avoid the use of gaseous hydrogen fluoride.
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The hydrogen halides are colourless gases at standard conditions for temperature and pressure (STP) except for hydrogen fluoride, which boils at 19 °C. Alone of the hydrogen halides, hydrogen fluoride exhibits hydrogen bonding between molecules, and therefore has the highest melting and boiling points of the HX series.
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Care must be taken, however, when using enthalpies of vaporization to measure the strength of intermolecular forces, as these forces may persist to an extent in the gas phase (as is the case with hydrogen fluoride), and so the calculated value of the bond strength will be too low.
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Germanium difluoride can be synthesized by reacting germanium tetrafluoride with powdered germanium at 150–300 °C. Germanium tetrafluoride can be prepared by reaction of germanium with fluorine or hydrogen fluoride: Ge + 2 F2 → GeF4 It is also formed during the thermal decomposition of a complex salt, Ba: Ba(GeF6) → GeF4 + BaF2 Germanium tetrafluoride is a noncombustible, strongly fuming gas with a garlic odor.
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The pure tantalum hydrogen fluoride solution is then neutralised with aqueous ammonia to give hydrated tantalum oxide (Ta2O5(H2O)x), which is calcinated to tantalum pentoxide (Ta2O5) as described in these idealized equations: H2 + 5 H2O + 7 NH3 → 0.5 Ta2O5(H2O)5 + 7 NH4F Ta2O5(H2O)5 → Ta2O5 + 5 H2O Natural pure tantalum oxide is known as the mineral tantite, although it is exceedingly rare.
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