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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]
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
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.
A chloroanion is an anion that contains an element and chlorine atoms. They are also known as complex chlorides. They can occur in salts, or in solution, but not as pure acids. They mostly can be considered as chlorometallates [1] which are a subclass of halometallates.
The anhydrous form is predicted to be isostructural with cobalt(II) perchlorate, based on the IR spectrum and the Raman spectrum of the compound. [3]The hexahydrate consists of discreet [Mn(H 2 O) 6] 2+ octahedrons and perchlorate anions with lattice constants a = 7.85 Å, b = 13.60 Å and c = 5.30 Å.
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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.