A mixture of 0.02 mole of `KBrO_(3)` and `0.001` mole of `KBr` was treated with excess of KI and acidified. The volume of 0.01M `Na_(2)S_(2)O_(3)` solution required to consume the liberated iodine will be :

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:

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:

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 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 containing 0.05 mol of K_(2)Cr_(2)O_(7) and 0.02 mol of KMnO_(4) was treated with excess of KI in acidic medium.The liberated iodine required 2.0 L of Na_(2)SO_(3) solution of titration. Concentration of Na_(2)S_(2)O_(3) solution was

A 0.5 g sample containing MnO_(2) is treated with HCl liberating Cl_(2) is passed into a solution of KI and 30.0 " mL of " 0.1 M Na_(2)S_(2)O_(3) are required to titrate the liberated iodine. Calculate the percentage of MnO_(2) is the sample.

A 0.5 g sample containing MnO_(2) is treated with HCl liberating Cl_(2) is passed into a solution of KI and 30.0 " mL of " 0.1 M Na_(2)S_(2)O_(3) are required to titrate the liberated iodine. Calculate the percentage of MnO_(2) is the sample.

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.