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Sodium bromate can be produced from a solution of sodium carbonate and bromine using chlorine gas as the oxidising agent. [1] 6 Na 2 CO 3 + Br 2 + 5 Cl 2 → 2 NaBrO 3 + 10 NaCl + 6 CO 2. It may also be produced by the electrolytic oxidation of aqueous sodium bromide. [2]
The bromate anion, BrO − 3, is a bromine-based oxoanion. A bromate is a chemical compound that contains this ion. Examples of bromates include sodium bromate (NaBrO 3) and potassium bromate (KBrO 3). Bromates are formed many different ways in municipal drinking water. The most common is the reaction of ozone and bromide: Br − + O 3 → BrO ...
Sodium tartrate – C 4 H 4 Na 2 O 6; Sodium tellurite – Na 2 TeO 3; Sodium tetrachloroaluminate – NaAlCl 4; Sodium tetrafluoroborate – NaBF 4; Sodium thioantimoniate – Na 3 (SbS 4)·9H 2 O; Sodium thiocyanate – NaSCN; Sodium thiosulfate – Na 2 S 2 O 3; Sodium tungstate – Na 2 WO 4; Sodium uranate – Na 2 O 7 U 2; Sodium zincate ...
Sodium perbromate can be prepared by reacting sodium bromate with fluorine and sodium hydroxide: [1] NaBrO 3 + F 2 + 2 NaOH → NaBrO 4 + 2 NaF + H 2 O. References
Ammonium bromate is a very unstable compound that slowly decomposes at −5 °C and explodes at 54 °C. The decomposition proceeds as follows: [4] [5] NH 4 BrO 3 → NH 4 NO 3 + 2 Br 2 + O 2 + N 2 O + 6 H 2 O NH 4 BrO 3 → N 2 + Br 2 + O 2 + 4 H 2 O
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.
Sodium hypobromite can be isolated as an orange solid. A secondary reaction, where hypobromite spontaneously disproportionates to bromide (bromine oxidation state −1) and bromate (bromine oxidation state +5) takes place rapidly at 20 °C and slowly at 0 °C. 3 BrO − → 2 Br − + BrO − 3
The most important of these salts are the diperiodatonickelates, in which nickel exhibits the +4 oxidation state: these are powerful oxidising agents, capable of oxidising bromate to perbromate. The first periodatonickalates discovered were sodium nickel periodate (NaNiIO 6 ·0.5H 2 O) and potassium nickel periodate (KNiIO 6 ·0.5H 2 O). P.