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Dihydrate salt (NaBr·2H 2 O) crystallize out of water solution below 50.7 °C. [8] NaBr is produced by treating sodium hydroxide with hydrogen bromide. Sodium bromide can be used as a source of the chemical element bromine. This can be accomplished by treating an aqueous solution of NaBr with chlorine gas: 2 NaBr + Cl 2 → Br 2 + 2 NaCl
The classic case is sodium bromide, which fully dissociates in water: NaBr → Na + + Br −. Hydrogen bromide, which is a diatomic molecule, takes on salt-like properties upon contact with water to give an ionic solution called hydrobromic acid. The process is often described simplistically as involving formation of the hydronium salt of bromide:
Bromates are formed many different ways in municipal drinking water. The most common is the reaction of ozone and bromide: Br − + O 3 → BrO − 3. Electrochemical processes, such as electrolysis of brine without a membrane operating to form hypochlorite, will also produce bromate when bromide ion is present in the brine solution.
Organobromides are the most common organohalides in nature, even though the concentration of bromide is only 0.3% of that for chloride in sea water, because of the easy oxidation of bromide to the equivalent of Br +, a potent electrophile. The enzyme bromoperoxidase catalyzes this reaction. [52]
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]
(Nonetheless, nitrogen tribromide is named as a bromide as it is analogous to the other nitrogen trihalides.) [4] Bromination of metals with Br 2 tends to yield lower oxidation states than chlorination with Cl 2 when a variety of oxidation states is available. Bromides can be made by reaction of an element or its oxide, hydroxide, or carbonate ...
Hypobromous acid has a pK a of 8.65 and is therefore only partially dissociated in water at pH 7. Like the acid, hypobromite salts are unstable and undergo a slow disproportionation reaction to yield the respective bromate and bromide salts. 3 BrO − (aq) → 2 Br − (aq) + BrO − 3 (aq)
At 20 °C the reaction is rapid. [2] Br 2 + 2 OH − (aq) → Br − + BrO − + H 2 O. In this reaction the bromine disproportionates (some undergoes reduction and some oxidation) from oxidation state 0 (Br 2) to oxidation state −1 (Br −) and oxidation state +1 (BrO −). Sodium hypobromite can be isolated as an orange solid.