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Calcium chloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century. [11] It was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum [12]) because it was synthesized during the distillation of ammonium chloride with lime and was nonvolatile (while the former appeared to sublime); in more modern times (18th-19th cc.) it was called ...
For instance, water warms when treated with CaCl 2 (anhydrous calcium chloride) as a consequence of the large heat of hydration. However, the hexahydrate, CaCl 2 ·6H 2 O cools the water upon dissolution. The latter happens because the hydration energy does not completely overcome the lattice energy, and the remainder has to be taken from the ...
The notation "hydrated compound⋅n H 2 O", where n is the number of water molecules per formula unit of the salt, is commonly used to show that a salt is hydrated. The n is usually a low integer, though it is possible for fractional values to occur. For example, in a monohydrate n = 1, and in a hexahydrate n = 6.
Sodium chloride-20 1 to 3 ratio of salt to ice. Dry ice: Tetrachloroethylene-22 Dry ice: Carbon Tetrachloride-23 Dry ice: 1,3-Dichlorobenzene-25 Dry ice: o-Xylene-29 Liquid N 2: Bromobenzene-30 Dry ice: m-Toluidine-32 Dry ice: 3-Heptanone-38 Ice: Calcium chloride hexahydrate -40 1 to 0.8 ratio of salt to ice. Dry ice: Acetonitrile-41 Dry ice ...
calcium chloride: 10043–52–4 CaCl 2 •6H 2 O: calcium chloride hexahydrate: 7774–34–7 CaCl 2 O 2: calcium hypochlorite: 7778–54–3 CaCr 2 O 7: calcium chromate: 14307–33–6 CaF 2: calcium fluoride: 7789–75–5 CaHPO 4: calcium hydrogenorthophosphate: 7757–93–9 CaH 2: calcium hydride: 7789–78–8 Ca(H 2 PO 2) 2: calcium ...
The cobalt chloride mentioned above occurs as [Co(H 2 O) 6] 2+ and Cl −. In tin chloride, each Sn(II) center is pyramidal (mean O/Cl−Sn−O/Cl angle is 83°) being bound to two chloride ions and one water. The second water in the formula unit is hydrogen-bonded to the chloride and to the coordinated water molecule.
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
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.