A 1 g sample of Fe_(2)O_(3) solid of 55.2% purity is dissolved in acid and reduced by heating the solution with zinc dust. The resultant solution is cooled and made upto 100 mL. An aliquot of 25 mL of this solution requires 17 mL of 0.0167M solution of an oxidant for titration. Calculate no.of electrons taken up by oxidant in the above titration.

A 1 g sample of Fe_(2)O_(3) solid of 55.2% purity is dissolved in acid

1.	A 1 g sample of Fe_(2)O_(3) solid of 55.2% purity is dissolved in acid and reduced by heating the solution with zinc dust. The resultant solution is cooled and made upto 100 mL. An aliquot of 25 mL of this solution requires 17 mL of 0.0167M solution of an oxidant for titration. Calculate no.of electrons taken up by oxidant in the above titration.
Answer» Solution :Weight of `Fe_(2)O_(3) = 0.552 g ` Number of eq. OD `Fe_(2)O_(3) = (0.552)/80 {:(,Fe_(2)O_(3)to,2FeO),("+6",," +4"),(eq. wt . of ,Fe_(2)O_(3)= 160/2,=80):}` Let the number of electrons taken upby the oxidant in the reaction be n ( i..ethe CHANGE in oxidation number ) ` :. ` NORMALITYOF the oxidant = 0.0167 n N ` :. ` m.e of 25 mL of `Fe^(2+)`solution= 0.0167 n xx 17 ` :. ` m.eof 100 mLof `Fe^(2+)`solution= `(68 xx 0.0167 n)/(1000)` eq . of `Fe_(2)O_(3) ` = eq of FEO `(0.552)/80 = (68 xx 0.167n)/1000 n = 6`