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Potassium fluoride is prepared by reacting potassium carbonate with hydrofluoric acid. Evaporation of the solution forms crystals of potassium bifluoride. The bifluoride on heating yields potassium fluoride: K 2 CO 3 + 4 HF → 2 KHF 2 + CO 2 ↑ + H 2 O KHF 2 → KF + HF ↑. Platinum or heat resistant plastic containers are often used for ...
KC 2 H 3 O 2: potassium acetate: 127–08–2 KC 2 H 5 O: potassium ethoxide: 917–58–8 KC 3 H 5 O 2: potassium propionate: 327–62–8 KC 3 H 5 S 2 O: potassium xanthogenate: 140–89–6 KC 3 H 7 NS 2: potassium dimethyldithiocarbamate: 128–03–0 KC 4 H 5 O 6: potassium bitartrate: 868–14–4 KC 7 H 5 O 2: potassium benzoate: 582 ...
Solubility tables; Substance Formula 0 °C 10 °C 15 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Actinium(III) hydroxide
C 2 H 7 NO: ethanolamine: 141-43-5 C 2 H 7 NO 2: ammonium acetate: 631-61-8 C 2 H 7 NO 3 S: taurine: 107-35-7 C 2 O 4 2−: oxalate ion: CH 3 ClO 4: Methyl perchlorate: 17043-56-0 C 3 H 3 Cl 3: 1,1,3-Trichloropropene: 2567-14-8 C 3 H 3 O 4 −: malonate ion: 156-80-9 C 3 HN: cyanopolyyne: C 3 H 3 N: azete: 287-24-1 C 3 H 4: Propadiene: 463-49-0 ...
Potassium hexafluoronickelate(IV) is an inorganic compound with the chemical formula K 2 NiF 6. It can be produced through the reaction of potassium fluoride, nickel dichloride, and fluorine. It reacts violently with water, releasing oxygen. It dissolves in anhydrous hydrogen fluoride to produce a light-red solution.
Potassium bifluoride is the inorganic compound with the formula K[HF 2]. This colourless salt consists of the potassium cation (K +) and the bifluoride anion ([HF 2] −). The salt is used as an etchant for glass. Sodium bifluoride is related and is also of commercial use as an etchant as well as in cleaning products. [3]
Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and hydrofluoric acid containing small quantities of water. [7] [8] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide, with sodium fluoride as a side-product:
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]