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1.0 g of Fe2O3 solid of 55.2% purity is ...

1.0 g of `Fe_2O_3` solid of `55.2%` purity is dissolved in acid. The solution is reduced by heating with Zn dust. The resultant solution is cooled and made up to 100 mL. An aliquot of 25 " mL of " this solution requires 17 " mL of " 0.0167 M solution of an oxidant. Calculate the number of electrons taken up by oxidant in the above titration.

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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.

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A sample of 1.0g of solid Fe_(2)O_(3) of 80% purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7mL of a 0.1M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

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A 3.00 g sample containing Fe_(3)O_(4), Fe_(2)O_(3) and an inert impure substance, is treated with excess of KI solution in presence of dilute H_(2)SO_(4) . The entire iron is converted into Fe^(2+) along with the liberation of iodine. The resulting solution is diluted to 100 mL. A 20 mL of the dilute solution requires 11.0 mL of 0.5 M Na_(2)S_(2)O_(3) solution to reduce the iodine, present. A 50 mL of the dilute solution after complete extraction of the iodine required 12.80 mL of 0.25 M KMnO_(4) solution in dilute H_(2)SO_(4) medium for the oxidation of Fe^(2+) . Calculate the % of Fe_(2)O_(3) "and" Fe_(3)O_(4) in the original sample.

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25.0 g of FeSO_(4).7H_(2)O was dissolved in water containing dilute H_(2)SO_(4) and the volume was made up to 1.0 L. 25.0 " mL of " this solution requried 20 " mL of " an (N)/(10) KMnO_(4) solution for complete oxidation the percentage of FeSO_(4)7H_(2)O in the acid solution is

AAKASH INSTITUTE ENGLISH-REDOX REACTIONS-Assignment (Section I) (Subjective Type Questions)
  1. Balance the chemical equation by the oxidation number method. (ix) ...

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  2. A solution is prepared by dissolving 60 g of sodium chloride in 400 g ...

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  3. Balance the following reaction by the oxidation number method - MnO(...

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  4. Balance the equation by lon-electron method (ii) MnO(4)^(-) + H(2)C(...

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  5. Balance the equation by lon-electron method (iii) Cu^(2+) + SO(2) to...

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  6. Balance the equation by lon-electron method N(2)O(4) + BrO(3)^(-) to...

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  7. Balance the equation by lon-electron method (v) Br^(-) + BrO(3)^(-) ...

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  8. In acidic medium moles of KMnO4required to oxidise 1.5 moles of Cu2S w...

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  9. Balance the equation by lon-electron method (vii) S+ OH^(+) to S^(2-...

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  10. Balance the equation by lon-electron method Al + NO(3)^(-) to Al(OH...

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  11. Balance the equation by lon-electron method Cr(2)O(7)^(2-) + Fe^(2+)...

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  12. The density of a molal solution of NaOH is 1.110 g mL^(-1). The molari...

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  13. What is the weight of sodium bromate and molarity of solution to prepa...

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  14. 12 litre of H2 and 11.2 litre of Cl2 are mixed and exploded. The compo...

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  15. What is the weight of sodium bromate and molarity of solution to prepa...

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  16. 5.7 g of bleaching powder was suspended in 500 mL of water. 25 mL of t...

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  17. Borax in water gives the following: B4O7^(2-)+7H2Oto4H2BO3+2overset(...

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  18. 1.0 g of AgNO3 is dissolved in 50 " mL of " water It is titrated with ...

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  19. A solution contains Na(2)CO(3) and NaHCO(3). 10 mL of the solution req...

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  20. 1.0 g of Fe2O3 solid of 55.2% purity is dissolved in acid. The solutio...

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