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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 ...
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 ...
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.
Lead(II) fluoride can be prepared by treating lead(II) hydroxide or lead(II) carbonate with hydrofluoric acid: [3]. Pb(OH) 2 + 2 HF → PbF 2 + 2 H 2 O Alternatively, it is precipitated by adding hydrofluoric acid to a lead(II) salt solution, or by adding a fluoride salt to a lead salt, such as potassium fluoride to a lead(II) nitrate solution, [4]
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
Potassium fluoroborate is obtained by treating potassium carbonate with boric acid and hydrofluoric acid. B(OH) 3 + 4 HF → HBF 4 + 3 H 2 O 2 HBF 4 + K 2 CO 3 → 2 KBF 4 + H 2 CO 3. Fluoroborates of alkali metals and ammonium ions crystallize as water-soluble hydrates with the exception of potassium, rubidium, and cesium.
Mold is a dangerous library pest because of the damage it causes to the collections. Mold thrives off of paper and books; these objects provide the fungi a source of nutrition, namely the sugar and starches present in the cellulose materials. [6] Mold feeds on cloth, leather, glues, adhesives, cellulose starch and starches in the sizing.
SbF 5 has also been used in the first discovered chemical reaction that produces fluorine gas from fluoride compounds: 4 SbF 5 + 2 K 2 MnF 6 → 4 KSbF 6 + 2 MnF 3 + F 2 The driving force for this reaction is the high affinity of SbF 5 for F − , which is the same property that recommends the use of SbF 5 to generate superacids.