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

4 Sb (+3) + 2 Br (2) O (3) ----> 4 SbBr + 3 O(-2)

In the equation, place the valences in parentheses and the stoichiometric balance numbers so that the reaction is balanced, place them in bold.

Step-by-step explanation:

In this chemical equation it seems to me that the valences of BrO are wrong.

That is why I will complete the equation, demonstrating the chemical reaction, and also use the appropriate valences.

Assuming that Sb has a valence of +3 and that the Br that appears in the form of oxide with oxygen (valence -2) has a valence of +3 (because -3 does not exist as valence or oxidation state of bromine).