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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 bromate – NaBrO 3; Sodium bromide – NaBr; Sodium bromite – NaBrO 2; Sodium carbide – Na 2 C 2; Sodium carbonate – Na 2 CO 3; Sodium chlorate – NaClO 3; Sodium chloride – NaCl; Sodium chlorite – NaClO 2; Sodium cobaltinitrite – CoN 6 Na 3 O 12 [207] Sodium copper tetrachloride – Na 2 CuCl 4; Sodium cyanate – NaCNO ...
Sodium bromite is a sodium salt of bromous acid. Its trihydrate , NaBrO 2 ·3H 2 O, has been isolated in crystal form. It is used by the textile refining industry as a desizing agent for oxidative starch removal.
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
The agent used is sodium thiosulfate, and reacts according to the following equation: [2] AgX(s) + 2 Na 2 S 2 O 3 (aq) → Na 3 [Ag(S 2 O 3 ) 2 ](aq) + NaX(aq) An indefinite number of positive prints can be generated from the negative by passing light through it and undertaking the same steps outlined above.
Potassium bromate is classified as a category 2B carcinogen by the IARC. [6] The FDA allowed the use of bromate before the Delaney clause of the Food, Drug, and Cosmetic Act – which bans potentially carcinogenic substances – went into effect in 1958. Since 1991, the FDA has urged bakers to not use it, but has not mandated a ban.