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A 0.472 g sample of an alloy of tin and bismuth is dissolved in sulfuric acid to...

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roshan-rox | Valedictorian

Posted July 20, 2013 at 5:31 PM via web

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A 0.472 g sample of an alloy of tin and bismuth is dissolved in sulfuric acid to produce tin(II) and bismuth(III) ions. This solution is diluted to the mark in a 100 mL volumetric flask and 25.00 mL aliquots are titrated with a 0.0107 M solution of KMnO4, forming tin(IV) and manganese(II) ions. (The bismuth ions are unaffected during this titration.)

a.  Write a balanced equation for the reaction of the MnO4- ion with Sn(II) in acid solution.

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jeew-m | College Teacher | (Level 1) Educator Emeritus

Posted July 20, 2013 at 5:40 PM (Answer #1)

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As explained in the question when potassium permanganate is used there is no change in the oxidation state of Bismuth. It remains at +3. Theoxidation state of Tin will increase from +2 to +4 while Mn will reduce its oxidation number from +7 to +2.

 

Oxidation reaction

`Sn^(2+) rarr Sn^(4+)+2e ----(1)`

 

Redox reaction

`MnO_4+8H^++5e rarr Mn^(2+)+4H_2O -----(2)`

 

`(1)xx5+(2)xx2`

`2MnO_4+16H^++5Sn^(2+) rarr 2Mn^(2+)+8H_2O+5Sn^(4+)`

 

so the balance reaction is as above.

 

 

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