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The standard oxidation potential of Zn r...

The standard oxidation potential of `Zn` referred to SHE is 0.76 V and that of Cu is `-0.34V` at `25^(@)C` when excess of `Zn` is added to `CuSO_(4)`, Zn displaces `Cu^(2+)` till equilibrium is reached. What is the approx ratio of `Zn^(2+)` to `Cu^(2+)` ios at equilibrium?

Text Solution

Verified by Experts

The correct Answer is:
`[Zn^(2+)]//[Cu^(2+)]=2xx10^(37)`
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The standard oxidation potential of Zn referred to SHE is 0.76V and that of Cu is -0.34V at 25^(@)C . When excess of Zn is added to CuSO_(4),Zn diplaces Cu^(2+) till equilibrium is reached. What is the ratio of Zn^(2+) to Cu^(2+) ions at equilibrium?

The normal oxidation potential of zinc referred to the standard hydrogen electrode is 0.76 volt and that of copper is -0.34 volt at 25^(@)C . When excess of zinc is added to a solution of copper sulphate the zinc displace copper till equilibrium is reached. What is the ratio of concentration of Zn^(2+) to Cu^(2+) ions at equilibrium ?

Knowledge Check

  • The e.m.f of galvanic cell , with oxidation potentials of Zn = +0.76 V and that of Cu = -0.34 V , is ________.

    A
    `-1.1 V`
    B
    `+1.1V`
    C
    `+0.345 V`
    D
    `+0.76 V`

  • The emf of a galvanic cell with electrode potential of Zn=+0.76 V and that of Cu =-0.34 V is

    A
    `-1.1 V`
    B
    `+1.1 v`
    C
    `+0.34 V`
    D
    `+0.76 v`

  • The standard electrode potentials of Zn, Ag and Cu are -0.76, 0.80 and 0.34 volt respectively, then:

    A
    Ag can oxidised Zn and Cu
    B
    Ag can reduce `Zn^(2+)` and `Cu^(2+)`
    C
    Zn can reduce `Ag^(+)` and `Cu^(2+)`
    D
    Cu can oxidise Zn and Ag

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