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A 0.472 g sample of an alloy of tin and bismuth is dissolved in sulfuric acid to...
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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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.
`Sn^(2+) rarr Sn^(4+)+2e ----(1)`
`MnO_4+8H^++5e rarr Mn^(2+)+4H_2O -----(2)`
`2MnO_4+16H^++5Sn^(2+) rarr 2Mn^(2+)+8H_2O+5Sn^(4+)`
so the balance reaction is as above.
Posted by jeew-m on July 20, 2013 at 5:40 PM (Answer #1)
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