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.

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 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.

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.

1.5 g of chalk was treated with 10 " mL of " 4 N HCl. The chalk was dissolved and the solution was made to 100 mL. 25 " mL of " this solution required 18.75 " mL of " 0.2 N NaOH solution for comjplete neutralisation. Calculate the percentage of pure CaCO_3 in the sample of chalk.

0.2828 g of iron wire was dissolved in excess dilute H_(2)SO_(4) and the solution was made upto 100mL. 20mL of this solution required 30mL of N/(30)K_(2)Cr_(2)O_(7) solution for exact oxidation. Calculate percent purity of Fe in wire.

1.575 g of oxalic acid (COOH)_(2).xH_(2)O are dissolved in water and the volume made up to 250 mL. On titration 16.68 mL of this solution requires 25 mL of N/15 NaOH solution for complete neutralisation. Calculate the value of x.

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.

7.5 g of an acid are dissolved per litre of the solution. 20 mL of this acid solution required 25 mL of N//15 NaOH solution for complete neutralization. Calculate the equivalent mass of the acid.

If 100mL of 0.1M urea solution is mixed with 100mL of 0.2M glucose solution at 300K. Calculate osmotic pressure?

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