A mixture containing `0.05` mole of `K_2Cr_2O_7 and 0.02` mole of `KMnO_4` was treated with excess of `KI` in acidic madium. The librated iodine required `1.0L` of `NaS_2 O_3` solution for titration. Concentration of `Na_2 S_2 O_3` solution was :

A mixture contaning 0.05 moleof K_(2)Cr_(2)O_(7) and 0.02 "mole of" KMnO_(4) was treated eoith excess of KI in acidic medium. The liberated iodine required 1.0L "of" Na_(2)S_(2)O_(3) solution for titration. Concentration of Na_(2)S_(2)O_(3) solution was:

0.5g mixture of K_2Cr_2 O_7 and KMnO_4 was treated with excess of KI in acidic medium. Iodine liberated required 150cm^3 of 0.1N solution of thiosulphate solution for titration. Find the percentage of K_2 Cr_2 O_7 in the mixture :

0.5 g mixture of K_(2)Cr_(2)O_(7) and KMnO_(4) was treated with excess of KI in acidic medium. Iodine liberated required 100 cm^(3) of 0.15N sodium thiosulphate solution for titration. Find the per cent amount of each in the mixture.

0.5 gmixture of K_(2)Cr_(2)O_(7) and KMnO_(4) was treated with excess of KI in acidic medium. Iodine liberated required 150 cm^(3) of 0.10 N solution of thiosulphate solution for titration. Find trhe percentage of K_(2)Cr_(2)O_(7) in the mixture :

Free iodine is titrated against standard reducing agent usually with sodium thiosulphate , i.e. K_(2)Cr_(2)O_(7) + 6Kl + 7H_(2)SO_(4) to Cr_(2)(SO_(4))_(3) + 4K_(2) SO_(4) + 7H_(2)O+l_(2) 2CuSO_(4) + 4Kl to Cu_(2)l_(2) + 2K_(2)SO_(4) + l_(2) l_(2) + Na_(2)S_(2)O_(3) to 2Nal + Na_(2)S_(4)O_(6) In iodometric titration, starch solution is used as an indicator. Starch solution gives blue or violet colour with free iodine .At the end point , blue or violet colour disappears when iodine is completely changed to iodide. 50 ml of an aqueous solution of H_(2)O_(2) was treated with excess of Kl in dil. H_(2)SO_(4) . The liberated iodine required 20 ml of 0.1 N Na_(2)S_(2)O_(3) for complete reaction. The concentration of H_(2)O_(2) is

When 25 " mL of " an aqueous solution of H_2O_2 is titrated with an excess of KI solution in dilute H_2SO_4 , the liberated I_2 required 20 " mL of " 0.3 N Na_2S_2O_3 solution for complete reaction.volume strength of H_2O_2 solution.

10 g mixture of K_(2)Cr(2)O_(7) and KMnO_(4) was treated with excess of KI in acidic medium. Iodine liberated 100 cm^(3) of 2.2 N sodium thiosulphate solution for titration. If the mass percent of KMnO_(4) in the mixture Z, then what is the value of 2Z/5 ?

1.5 g of a mixture containing As_2O_5 , Na_2HAsO_3 , and some inert impurities is dissolved in water, and the solution is kept neutral by adding excess of NaHCO_3 . The solution when titrated with 0.1 M I_2 required 35.0 nL of it for complete titration. The solution is then acidified and excess of KI is added to it. The I_2 liberated required 35.0mL of 0.3 M Na_2S_2O_3 solution for complete titration. Find the percentage composition of the mixture (Atomic mass of As is 75, Na is 23 and O is 16.)

638.0 g of CuSO_(4) solution is titrated with excess of 0.2 M KI solution. The liberated I_(2) required 400 " mL of " 1.0 M Na_(2)S_(2)O_(3) for complete reaction. The percentage purity of CuSO_(4) in the sample is

A solution of 0.2 g of a compound containing Cu^(2+) "and" C_(2)O_(4)^(2-) ions on titration with 0.02 M KMnO_(4) in presence of H_(2)SO_(4) consumes 22.6 mL of the oxidant. The resultant solution is neutralized with Na_(2)CO_(3) acidified with dil. acetic acid and treated with excess KI. The liberated iodine requires 11.3 mL of 0.5 M Na_(2)S_(2)O_(3) solution for complete reduction. Find out the mole ratio of Cu^(2+) "to" C_(2)O_(4)^(2-) in the compound. Write down the balanced redox reactions involved in the above titrations.