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100mL of 0.1M KMnO(4) is consumed in its...

100mL of 0.1M `KMnO_(4)` is consumed in its titration with oxalic acid in presence of dil. HCl whose excess amount was taken. The `Cl_(2)(g)` produced is reacted with excess of KI solution producing `I_(2)` which required 170mL of 0.2 M hypo solution for complete reaction. Calculate millimoles of oxalic acid consumed.

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10ml of 0.05M of KMnO_4 is titrated with 10ml oxalic acid. Find its strength

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 neutralised with Na_(2)CO_(2) acidfied with dilute acetic acid and treated with excess KI . The liberated I_(2) required 11.3 mL of 0.05 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 .

Knowledge Check

  • 10 moles of KMnO_(4) were consumed in each separate titration with oxalic acid, one in presence of H_(2)SO_(4) and other in presence of HCl. Identify the correct option.

    A
    25 moles of oxalic acid will be consumed in both cases.
    B
    25 moles of oxalic acid will be consumed in with `H_(2)SO_(4)` and with `HCl` more than 25 moles of oxalic acid will be consumed.
    C
    No oxalic acid will be consumed in case of HCl and less than 25 moles will be consumed in case of `H_(2)SO_(4)`
    D
    25 moles of oxalic acid will be consumed with `H_(2)SO_(4)` and less than 25 moles of oxalic acid will be consumed with HCl

  • 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
    `5%`
    B
    `10%`
    C
    `15%`
    D
    `20%`

  • What is the molarity of H_(2)O_(2) solution whose 100mL produce the 0.5 moles of I_(2) , when reacted with excess KI solution?

    A
    0.5M
    B
    1M
    C
    2.5M
    D
    5M

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    5g sample of brass was dissolved in one litre dil. H_(2)SO_(4) . 20 ml of this solution were mixed with KI, liberating I_(2) and Cu^(+) and the I_(2) required 20 ml of 0.0327 N hypo solution for complete titration. Calculate the percentage of Cu in the alloy.

    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.

    10.0 mL of 0.05 M KMnO4 solution was consumed in a titration with 10.0 mL of given oxalic acid dihydrate solution. The strength of given oxalic acid solution is ........ xx 10 ^(-2) g // L. (Round off to the nearest integer)

    50.0 g sample of brass is dissolved in 1 L dil H_2SO_4.20mL of this solution is mixed with KI, and the liberated I_2 required 20 " mL of " 0.5 M hypo solution for titration calculate the amount of Cu in the alloy.

    The amount of oxalic acid required to prepare 300 mL of 2.5 M solution is : (molar mass of oxalic acid = 90 g mol^(–1) ) :

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