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Manganese(II) chlorate was produced by the reaction of manganese(II) sulfate and barium chlorate. [3] The water was removed by boiling in vacuum. Then the temperature was lowered to -80°C which resulted in a pink solid. Then it was cleaned with liquid nitrogen and potassium hydroxide to remove the decomposition products. [2]
Manganese(II) chloride is the dichloride salt of manganese, MnCl 2. This inorganic chemical exists in the anhydrous form, as well as the di hydrate (MnCl 2 ·2H 2 O) and tetrahydrate (MnCl 2 ·4H 2 O), with the tetrahydrate being the most common form.
They contain the (ClO 3 −) anion. The stock naming convention distinguishes four chlorates, based on the oxidation state of the chlorine within the oxyanion. The stock and common names are: Chlorate(I) = Hypochlorite; Chlorate(III) = Chlorite; Chlorate(V) = Chlorate; Chlorate(VII) = Perchlorate
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.
Another earlier process to produce chlorine was to heat brine with acid and manganese dioxide. 2 NaCl + 2H 2 SO 4 + MnO 2 → Na 2 SO 4 + MnSO 4 + 2 H 2 O + Cl 2. Using this process, chemist Carl Wilhelm Scheele was the first to isolate chlorine in a laboratory. The manganese can be recovered by the Weldon process. [11]
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The water treatment plant at Niagara Falls, New York first used chlorine dioxide for drinking water treatment in 1944 for destroying "taste and odor producing phenolic compounds." [ 17 ] : 4–17 [ 18 ] Chlorine dioxide was introduced as a drinking water disinfectant on a large scale in 1956, when Brussels , Belgium, changed from chlorine to ...
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