When bromine gas reacts with aqueous sodium hydroxide, the equilibrium represented by the equation:

When bromine gas reacts with aqueous sodium hydroxide, the equilibrium represented by the equation:

Br₂(aq) + 2OH^-(aq) $_{\leftarrow}^{\rightarrow}$ Br^-(aq) + OBr^-(aq) + H₂O(l) is established. What observations would be made if a few drops of sulphuric (VI) acid were added to the equilibrium mixture? Explain.

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The mixture would turn brown due to excess Br₂(g). H⁺ ions removes OH^- ions from the mixture, and equilibrium shifts to the left.

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johnmulu answered the question on February 15, 2017 at 07:40

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