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The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Henri Moissan's 1892 record of fluorine gas color, viewed end-on in a 5‑m tube. Air (1) is on the left, fluorine (2) is in the middle, chlorine (3) is on the right. Fluorine forms diatomic molecules (F 2) that are gaseous at room temperature with a density about 1.3 times that of air. [1] [note 1] Though sometimes cited as yellow-green, pure
Fluorene / ˈ f l ʊər iː n /, or 9H-fluorene is an organic compound with the formula (C 6 H 4) 2 CH 2. It forms white crystals that exhibit a characteristic, aromatic odor similar to that of naphthalene. Despite its name, it does not contain the element fluorine, but rather it comes from the violet fluorescence it exhibits.
NiF 2 is prepared by treatment of anhydrous nickel(II) chloride with fluorine at 350 °C: [2]. NiCl 2 + F 2 → NiF 2 + Cl 2. The corresponding reaction of cobalt(II) chloride results in oxidation of the cobalt, whereas nickel remains in the +2 oxidation state after fluorination because its +3 oxidation state is less stable.
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.
The saturation with respect to water cannot be measured much below –50 °C, so manufacturers should use one of the following expressions for calculating saturation vapour pressure relative to water at the lowest temperatures – Wexler (1976, 1977), [1] [2] reported by Flatau et al. (1992)., [3] Hyland and Wexler (1983) or Sonntag (1994 ...
1.151 g/mL Melting point: 152 to 155 °C (306 to 311 °F; 425 to 428 K) Solubility in water. Practically insoluble [2] Hazards NFPA 704 (fire diamond) 0. 0. 0.
In solutions containing the fluoride ion, F −, it forms the fluoride complexes SnF 3 −, Sn 2 F 5 −, and SnF 2 (OH 2). [26] Crystallization from an aqueous solution containing NaF produces compounds containing polynuclear anions, e.g. NaSn 2 F 5 or Na 4 Sn 3 F 10 depending on the reaction conditions, rather than NaSnF 3. [20] The compound ...