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HBrO + HClO → HBrO 2 + HCl [citation needed] 2 HBrO → HBrO 2 + HBr [citation needed] The latter is a disproportionation reaction. Another method of oxidizing hypobromous acid can be used: HBrO + H 2 O - 2e − → HBrO 2 + 2H + [citation needed] The oxidized bromine-containing acid need not contain oxygen originally, as in this ...
Addition of bromine to water gives hypobromous acid and hydrobromic acid (HBr(aq)) via a disproportionation reaction. Br 2 + H 2 O ↽ − ⇀ {\displaystyle {\ce {<=>>}}} HOBr + HBr In nature, hypobromous acid is produced by bromoperoxidases , which are enzymes that catalyze the oxidation of bromide with hydrogen peroxide: [ 2 ] [ 3 ]
A oxidation reaction between hypobromous acid (HBrO) and hypochlorous acid (HClO) can be used to produce bromous acid (HBrO 2) and hydrochloric acid (HCl). [citation needed] HBrO + HClO → HBrO 2 + HCl. A redox reaction of hypobromous acid (HBrO) can form bromous acid (HBrO 2) as its product: [citation needed] HBrO + H 2 O − 2e − → HBrO ...
There are several general reasons for this: (1) they may condense to form oligomers (e.g., H 2 CrO 4 to H 2 Cr 2 O 7), or dehydrate all the way to form the anhydride (e.g., H 2 CO 3 to CO 2), (2) they may disproportionate to one compound of higher and another of lower oxidation state (e.g., HClO 2 to HClO and HClO 3), or (3) they might exist ...
Hydrogen peroxide (H 2 O 2) can be used as HOCl scavenger whose byproducts do not interfere in the Pinnick oxidation reaction: HOCl + H 2 O 2 → HCl + O 2 + H 2 O. In a weakly acidic condition, fairly concentrated (35%) H 2 O 2 solution undergoes a rapid oxidative reaction with no competitive reduction reaction of HClO 2 to form HOCl. HClO 2 ...
Chlorous acid is an inorganic compound with the formula HClO 2. It is a weak acid. Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation state +5): 2 HClO 2 → HClO + HClO 3
Bromic acid, also known as hydrogen bromate, is an oxoacid with the molecular formula HBrO 3. It only exists in aqueous solution. [1] [2] It is a colorless solution that turns yellow at room temperature as it decomposes to bromine. [1] [3] Bromic acid and bromates are powerful oxidizing agents and are common ingredients in Belousov ...
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.
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