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Write the balanced ionic equation which ...

Write the balanced ionic equation which represents the oxidation of iodine `(I^(-))` ion by per-manganate ion in basic medium to give iodine (I) and manganese dioxide `(MnO_(2))`.

Text Solution

Verified by Experts

Basic equation is
`MnO_(4)^(-)+I^(-)MnO_(2)+I_(2)` (Basic medium)
(a) `MnO_(4(aq))^(-)+I_((aq))^(-) to MnO_(2(s))+I_(2(s))` (Basic medium)
Reduction half cell
`MnO_(4)^(-)to MnO_(2)`
`MnO_(4)^(-)to MnO_(2)+2H_(2)O` (Oxygens balanced)
`MnO_(4)^(-)+4H_(2)O to MnO_(2)+2H_(2)O+4OH^(-)`
(Hydrogents balanced)
`MnO_(4)^(-)+2H_(2)O to MnO_(2)+4 OH^(-)`
`MnO_(4)^(-)+2H_(2)O+3e^(-)to MnO_(2)+4OH^(-)` (charge balanced)
Oxidation half cell
`I^(-)to I_(2)`
`2I^(-)to I_(2)` (Iodines balanced)
`2 I^(-)to I_(2)+2e^(-)` (Charge balanced)
`overset(2[MnO_(4)+2HO_(2)+3e^(-)to MnO_(2)+4OH])(3xx[2I^(-)to I_(2)+2e^(-)])/(2MnO_(4)^(-)+4 H_(2)O+6e^(-)to 2MnO_(2)+8OH^(-))`
`6I^(-)to 3I_(2)+6e^(-)`
`2MnO_(4)^(-)+4 H_(2)O+6I^(-)to 2MnO_(2)+3I_(2)+8OH^(-)`
The above equation is balanced equation .
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Knowledge Check

  • All titration which involves the direct titration of Iodine with a reducing agent are grouped under lodimetry. Iodimetry is employed to determine the strength of reducing agent such as sodium thio sulphate I_(2) + 2Na_(2)S_(2)O_(3) rarr 2I^(-)+S_(4)O_(6)^(-) If iodine is liberated as a result of chemical reaction involving oxidation of an idodide ion by a strong oxidizing agent in neutral or acidic medium the liberated iodine is then titrated with reducing agent. This titration is called lodometry. Todometry is used to estimate the strength of oxidizing agent. For example the estimation of Cu^(++) with thiosulphate. Cu^(+ +) +I^(-) Cu_(2)I_(2)+I_(2) , I_(2) +S_(2)O_(3)^(-) rarrS_(4)O_(6)^(-) +I^(-) Starch used as indicator near the end point which form blue colour complex with I_(3)^(-) . The blue colour disappears when When 159.50g of CuSO_4 in a solution is reacted with KI, then the liberated iodine required 100 ml 1 M Na_(2)S_(2)O_3 for complete reaction, then what is the percentage purity of sample used in making the solution.

    A
    `10%`
    B
    `20%`
    C
    ` 5%`
    D
    ` 30%`

  • All titration which involves the direct titration of Iodine with a reducing agent are grouped under lodimetry. Iodimetry is employed to determine the strength of reducing agent such as sodium thio sulphate I_(2) + 2Na_(2)S_(2)O_(3) rarr 2I^(-)+S_(4)O_(6)^(-) If iodine is liberated as a result of chemical reaction involving oxidation of an idodide ion by a strong oxidizing agent in neutral or acidic medium the liberated iodine is then titrated with reducing agent. This titration is called lodometry. Todometry is used to estimate the strength of oxidizing agent. For example the estimation of Cu^(++) with thiosulphate. Cu^(+ +) +I^(-) Cu_(2)I_(2)+I_(2) , I_(2) +S_(2)O_(3)^(-) rarrS_(4)O_(6)^(-) +I^(-) Starch used as indicator near the end point which form blue colour complex with I_(3)^(-) . The blue colour disappears when In the reaction, 2CuSO_(4) +4KI rarr Cu_(2)I_(2) + 2K_(2)SO_(4)+I_2 the ratio of equivalent weight of CuSO_4 to its molecular weight is:

    A
    `1//8`
    B
    `1//4`
    C
    `1//2`
    D
    1

  • All titration which involves the direct titration of Iodine with a reducing agent are grouped under lodimetry. Iodimetry is employed to determine the strength of reducing agent such as sodium thio sulphate I_(2) + 2Na_(2)S_(2)O_(3) rarr 2I^(-)+S_(4)O_(6)^(-) If iodine is liberated as a result of chemical reaction involving oxidation of an idodide ion by a strong oxidizing agent in neutral or acidic medium the liberated iodine is then titrated with reducing agent. This titration is called lodometry. Todometry is used to estimate the strength of oxidizing agent. For example the estimation of Cu^(++) with thiosulphate. Cu^(+ +) +I^(-) Cu_(2)I_(2)+I_(2) , I_(2) +S_(2)O_(3)^(-) rarrS_(4)O_(6)^(-) +I^(-) Starch used as indicator near the end point which form blue colour complex with I_(3)^(-) . The blue colour disappears when 10 mL of H_2O_2 solution on treatment with KI and titration of liberated I_2 required 10 mL of 1 N hypo . Thus H_2O_2 is :

    A
    1 N
    B
    5.6 volume
    C
    `17 gL^(-1)`
    D
    All are correct

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