A mixture of `FeO and Fe_2 O_3` is completely reacted with `100mL` of `0.25M` acidified `KMnO_4` solution. The resulting solution was then treated with Zn dust which converted `Fe^(3+)` of the solution to `fe^(2+)`. The `Fe^(2=)` required `100mL` of `0.10MK_2 Cr_2O_7` solution. Find out the weight `% Fe_2O_3` in the mixture.

A mixture of FeO and Fe_(2)O_(3) is completely reacted with 100 mL of 0.25 M acidified KMnO_(4) solution. The resultant solution was then treated with Zn dust which converted Fe^(3+) of the solution to Fe^(2+) .The Fe^(2+) required 1000 mL of 0.10 MK_(2)Cr_(2)O_(7) solution. Find out the weight % Fe_(2)O_(3) in the mixture.

Fe_2 O_3 + CO to

Which among FeO and Fe_2O_3 is more basic?

25 mL of a solution of Fe^(2+) ions was titrated with a solution of the oxidizing agent Cr_(2)O_(7)^(2-) . 50 mL of 0.01 M K_(2)Cr_(2)O_(7) solution was required. What is the molarity of the Fe^(2+) solution ?

A mixture of KMnO_(4) and K_(2)Cr_(2)O_(7) weighing 0.24 g on being treated with KI in acid solution liberates just sufficient I_(2) to react with 60 mL of 0.1 Na_(2)S_(2)O_(3) solution. Find out weight of KMnO_(4) and K_(2)Cr_(2)O_(7) in the mixture.

3 " mol of "a mixture of FeSO_(4) and Fe_(2)(SO_(4))_(3) requried 100 " mL of " 2 M KMnO_(4) solution in acidic medium. Hence, mole fraction of FeSO_(4) in the mixture is

A 4.0 g sample contained Fe_2O_3,Fe_3O_4 , and inert material. It was treated with an excess of aq KI solution in acidic medium, which reduced all iron to Fe^(2+) ions along with the liberation of iodine . The resulting solution was diluted to 50 mL and a 10 mL sample of it was taken the iodine liberated in the small sample was titrated with 12.0 " mL of " 0.5 M Na_2S_2O_3 solution. The iodine from another 25 mL was extracted, after which the Fe^(2+) ions were titrated with 16 " mL of " 0.25 M MnO_4^(ɵ) ions in H_2SO_4 solution. Calculate the mass of two oxides in the original mixture.

If acidified solution of K_(2)Cr_(2)O_(7) turm green on addition of a salt three salt may contain Fe^(2+) .

A mole of a mixture of Mohr's salt and Fe_2(SO_4)_3 requires 500mL of MK_2Cr_2O_7 for complete oxidation in acidic medium. The mole % of the Mohr's salt in the mixture is :

10.0 g of CaOCl_2 is dissolved in water to make 200 mL solution 20 " mL of " it is acidified with acetic acid and treated with KI solution the I_2 liberated required 40 " mL of " (M)/(20)Na_2S_2O_3 solution. Find the percentage of available chlorine.