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Potassium fluoride is the chemical compound with the formula KF. After hydrogen fluoride , KF is the primary source of the fluoride ion for applications in manufacturing and in chemistry. It is an alkali halide salt and occurs naturally as the rare mineral carobbiite .
CAS number KAlF 4: potassium tetrafluoroaluminate: 14484–69–6 KAlO 2: potassium aluminate: ... potassium fluoride: 7789–23–3 KH: potassium hydride: 7693–26–7
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
F 3 NO 2 S: difluoroaminosulfonyl fluoride: 13709-30-3 F 3 NO 3 S: difluoraminooxysulfonyl fluoride: 6816-12-2 F 3 NS: thiazyl trifluoride: 15930-75-3 F 3 NaSn: sodium trifluorostannate: 13782-22-4 F 3 Nd: neodymium trifluoride: 13709-42-7 F 3 OP: phosphoryl fluoride: 13478-20-1 F 3 OTa: tantalum monoxide trifluoride: 20263-47-2 F 3 OV ...
Potassium hexafluorozirconate can be prepared from precipitation from solutions: 2KF + ZrF 4 → K 2 ZrF 6 ↓ 2KCl + (NH 4) 2 ZrF 6 → K 2 ZrF 6 ↓ + 2NH 4 Cl. Also, in industry, it is obtained by sintering zirconium ore concentrates with K 2 SiF 6 at 600–700 °C. [3]
Potassium fluorosilicate is a chemical compound with the chemical formula K 2 [SiF 6]. When doped with potassium hexafluoromanganate(IV) ( K 2 [MnF 6 ] , with Mn 4+ ) it forms a narrow band red producing phosphor , (often abbreviated PSF or KSF), of economic interest due to its applicability in LED lighting and displays .
Potassium hexafluoroaluminate can be obtained by reacting fluoroaluminic acid (obtained by the reaction of anhydrous hydrogen fluoride and aluminum hydroxide) with potassium hydroxide at high temperature, followed by filtering, drying, melting, and crushing. 6HF + Al(OH) 3 → AlF 3 ·3HF + 3H 2 O AlF 3 ·3HF + 3KOH → K 3 AlF 6 + 3H 2 O
The bifluoride ion has a linear, centrosymmetric structure (D ∞h symmetry), with an F−H bond length of 114 pm. [1] The bond strength is estimated to be greater than 155 kJ/mol. [2] In molecular orbital theory, the atoms are modeled to be held together by a 3-center 4-electron bond (symmetrical hydrogen bond), [3] in a sort of hybrid between a hydrogen bond and a covalent bond.