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Hydrofluoric acid is a solution of hydrogen fluoride (HF) in water.Solutions of HF are colorless, acidic and highly corrosive.A common concentration is 49% (48-52%) but there are also stronger solutions (e.g. 70%) and pure HF has a boiling point near room temperature.
Aqueous solutions of HF are called hydrofluoric acid. When dilute, hydrofluoric acid behaves like a weak acid, unlike the other hydrohalic acids, due to the formation of hydrogen-bonded ion pairs [H 3 O + ·F −]. However concentrated solutions are strong acids, because bifluoride anions are predominant, instead
Thus, the usual ionization constant for hydrofluoric acid (10 −3.15) understates the acidity of concentrated solutions of HF. The effect of homoassociation is often high in nonaqueous solutions, wherein dissociation is often low. Carboxylic acids and phenols exhibit this effect, [3] for example in sodium diacetate.
Organofluorine compounds are pervasive. Many drugs, many polymers, refrigerants, and many inorganic compounds are made from fluoride-containing reagents. Often fluorides are converted to hydrogen fluoride, which is a major reagent and precursor to reagents. Hydrofluoric acid and its anhydrous form, hydrogen fluoride, are particularly important. [4]
Buffered oxide etch (BOE), also known as buffered HF or BHF, is a wet etchant used in microfabrication.It is a mixture of a buffering agent, such as ammonium fluoride NH 4 F, and hydrofluoric acid (HF).
"If hydrofluoric acid or modified hydrofluoric acid is released, then it forms into a ground-hugging toxic cloud that travels with the wind," Schwartz said. "It can cause death and permanent ...
Hydrofluoric acid is complicated because its strength depends on the concentration owing to the effects of homoconjugation. As solutions in non-aqueous solvents, such as acetonitrile , the hydrogen halides are only modestly acidic however.
The pH of a simple solution of an acid in water is determined by both and the acid concentration. For weak acid solutions, it depends on the degree of dissociation, which may be determined by an equilibrium calculation. For concentrated solutions of acids, especially strong acids for which pH < 0, the value is a better measure of acidity than ...