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Question

The quantity of antimony in an ore can be determined by an oxidation‑reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that all of the antimony is in the form of Sb3+(aq) . The Sb3+(aq) is completely oxidized by an aqueous solution of BrO−3(aq) . Complete and balance the equation for this reaction in acidic solution.

Answer 1

Sb³⁺(aq) + BrO₃^-(aq) ==> Sb⁵⁺(aq) + Br^-(aq) .. unbalanced equation

Sb³⁺(aq) ==> Sb⁵⁺(aq) + 2e- .. oxidation half reaction

BrO₃^-(aq) + 6H⁺ + 6e- ==> Br^-(aq) + 3H₂O .. reduction half reaction

To balance the electrons, multiply oxidation reaction by 3 and then add the two reactions:

3Sb³⁺(aq) ==> 3Sb⁵⁺(aq) + 6e-

BrO₃^-(aq) + 6H⁺ + 6e- ==> Br^-(aq) + 3H₂O

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3Sb³⁺(aq) + BrO₃^-(aq) + 6H⁺ ==> 3Sb⁵⁺(aq) + Br^-(aq) + 3H₂O .. balanced redox equation