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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.
Hydrogen fluoride is typically produced by the reaction between sulfuric acid and pure grades of the mineral fluorite: [14] CaF 2 + H 2 SO 4 → 2 HF + CaSO 4. About 20% of manufactured HF is a byproduct of fertilizer production, which generates hexafluorosilicic acid. This acid can be degraded to release HF thermally and by hydrolysis: H 2 SiF ...
The salt was prepared by Edmond Frémy by treating potassium carbonate or potassium hydroxide with hydrofluoric acid: 2 HF + KOH → K[HF 2] + H 2 O. With one more equivalent of HF, K[H 2 F 3] (CAS RN 12178-06-2, m.p. 71.7 °C [4]) is produced: HF + K[HF 2] → K[H 2 F 3] Thermal decomposition of K[HF 2] gives hydrogen fluoride: K[HF 2] → HF + KF
Sodium bifluoride reacts with water or moist skin to produce hydrofluoric acid. It also gives off hydrofluoric acid and hydrogen gas when it is heated to a gaseous state. The chemical can decompose upon contact with strong acids, strong bases, metal, water, or glass. [3] Sodium bifluoride also engages in violent reactions with chromyl chloride ...
There are several methods for synthesising rubidium fluoride. One involves reacting rubidium hydroxide with hydrofluoric acid: [1] RbOH + HF → RbF + H 2 O. Another method is to neutralize rubidium carbonate with hydrofluoric acid: [1] Rb 2 CO 3 + 2HF → 2RbF + H 2 O + CO 2. Another possible method is to react rubidium hydroxide with ammonium ...
Out of the four stable halogens, only fluorine and chlorine have reduction potentials higher than that of oxygen, allowing them to form hydrofluoric acid and hydrochloric acid directly through reaction with water. [17] The reaction of fluorine with water is especially hazardous, as an addition of fluorine gas to cold water will produce ...
Hexafluorosilic acid is only stable in hydrogen fluoride or acidic aqueous solutions. In any other circumstance, it acts as a source of hydrofluoric acid. Thus, for example, hexafluorosilicic acid pure or in oleum solution evolves silicon tetrafluoride until the residual hydrogen fluoride re-establishes equilibrium: [7] H 2 SiF 6 ⇌ 2 HF(l ...
The reaction is shown below: CsOH + HF → CsF + H 2 O. Using the same reaction, another way to create caesium fluoride is to treat caesium carbonate (Cs 2 CO 3) with hydrofluoric acid and again, the resulting salt can then be purified by recrystallization. The reaction is shown below: Cs 2 CO 3 + 2 HF → 2 CsF + H 2 O + CO 2