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A 1.10 g sample of copper ore is dissolv...

A `1.10 g` sample of copper ore is dissolved and the `Cu^(2+)` of is treated with excess `KI`. The liberated `I_(2)` requires `12.12 mL` of `0.10M Na_(2)S_(2)O_(3)` solution for titration. Find the `%` copper by mass in ore.

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A 1.100 g sample of copper ore is dissolved and the Cu_((aq.))^(2+) is treated with excess KI . The liberated I_(2) requires 12.12 mL of 0.10M Na_(2)S_(2)O_(3) solution for titration. What is % copper by mass in the ore?

1.1 g of sample of copper ore is dissolved and Cu^(2+) (aq) is treated with KI the iodine thus liberated requried 12.12 cm^(3) of 0.1 M Na_(2)S_(2)O_(3) solution for tritration what is the percentage of copper in the ore ?

Knowledge Check

  • 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. A 1.1 g sample of copper ore is dissolved and Cu^(2+) (aq). is treated with Kl . l_(2) liberated required 12.12" ml of " 0.1 M Na_(2)S_(2)O_(3) solution for titration . The % of Cu in the ore is

    A
    `2.5%`
    B
    `7%`
    C
    `5.8%`
    D
    `4.2%`

  • 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 dilute acetic acid and treated with excess Kl. The liberated iodine requires 11.3 ml of 0.05 N Na_(2)S_(2)O_(3) solution for complete reduction. Find out the molar ratio of Cu^(2+) to C_(2)O_(4)^(2-) in the compound. Write down the balanced redox reactions involved in the above titration.

    A
    `0.25`
    B
    `0.5`
    C
    2
    D
    4

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    1.1 g of sample of copper ore is dissolved and Cu^(2+) (aq) is treated with KI the iodine thus liberated requried 12.12 cm^(3) of 0.1 M Na_(2)S_(2)O_(3) solution for tritration what is the percentage of copper in the ore ?

    A 0.276 g impure sample of copper ore is dissolved and Cu^(2+) is titrated with KI solution. I_(2) liberated required 40 mL of 0.1 M Na_(2) S_(2) O_(3) solution for titration. What is the % of impurities in the ore ?

    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 .

    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.

    A solution of 0.2 g of a compound containing Cu^(2+) and C_(2)O_(4)^(2-) ions on titration with 0.02M KMnO_(4) in presence of H_(2)SO_(4) consumes 22.6mL oxidant. The resulting solution is neutralized by Na_(2)CO_(3) , acidified with dilute CH_(3)COOH and titrated with excess of KI . The liberated I_(2) required 11.3 mL "of" 0.05M Na_(2)S_(2)O_(3) for complete reduction. Find out mole ratio of Cu^(2+) and C_(2)O_(4)^(2+) in compound.

    When 100 mL of an aqueous of H_(2)O_(2) is titrated with an excess of KI solution in dilute H_(2)O_(2) , the liberated I_(2) required 50 mL of 0.1 M Na_(2) S_(2)O_(3) solution for complete reaction. Calculate the percentage strength and volume strength of H_(2)O_(2) solution.

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