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What happens to the concentration of Ag^...

What happens to the concentration of `Ag^(+)` ions in a solution of `AgNO_(3)` when it is electrolysed in presence of Ag-electrodes?

Text Solution

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The concentration of `A^(+)` remains constant. Although `Ag^(+)` is reduced at the silver cathode to form Ag, the same amount of `Ag^(+)` is produced in the solution through oxidation of Ag at the Ag - anode.
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Write the cathode and anode reactions for the electrolysis of aqueous AgNO_(3) solution in presence of Ag - electrodes.

Knowledge Check

  • What happens when concentration of solutes decrease in guard cells?

    A
    Water potential decreases
    B
    Water potential increase
    C
    Osmotic pressure increase
    D
    none of the above

  • Best reagent for the conversion of AgNO_(3) to Ag -

    A
    `HCIO_(4)`
    B
    `H_(3)PO_(2)`
    C
    `HIO_(4)`
    D
    `I_(2)`

  • In an aqueous solution containing Cu^(2+), Ag^(+), Sn^(2+) and Hg_(2)^(2+) ions, the concentration of each ion is 1 (M). Electrolysis of the solution is carried out in presence of inert electrodes. Given: E_(Hg_(2)^(2+)|Hg)^(@)=+0.79V and E_(Sn^(2+)|Sn)^(@)=-0.14V . If the voltage applied on the electrodes is gradually increased, then the metal that will deposit first and that at the end of the process at the cathode, respectively, are -

    A
    Sn, Ag
    B
    Cu, Hg
    C
    Cu, Sn
    D
    Ag, Sn

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