The quantity of antimony in a sample can be determined by an oxidation–reduction titration with an oxidizing agent.
A 5.85 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+(aq). The Sb3+(aq) is completely oxidized by 26.6 mL of a 0.125 M aqueous solution of KBrO3(aq). The unbalanced equation for the reaction is:
BrO3-(aq) + Sb3+(aq) > Br-(aq) + Sb5+(aq) (unbalanced)
(A) Calculate the amount of antimony in the sample and its percentage in the ore.

The percentage is   k  %

Explanation:

From the question we are told that

    The mass of the stibnite is  

   The volume of   KBrO3(aq) is  

     The concentration  of   KBrO3(aq) is  

Now the balanced ionic  equation for this reaction is

The number of moles of   is  

substituting values

from the reaction we see that 1 mole of  reacts with 3 moles of  

so 0.003325 moles will react with x moles of  

Therefore

Now the molar mass of is a constant with a values of  

Generally the mass of   is mathematically represented as

substituting values

The percentage of  Sb(antimony) in the overall mass of the stibnite is mathematically evaluated as

            k  

           k  %

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation: