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Zinc granules are added in excess to 500...

Zinc granules are added in excess to `500mL` OF `1.0m` nickel nitrate solution at `25^(@)C` until the equilibrium is reached. If the standard reduction potential of `Zn^(2+)|Zn` and `Ni^(2+)|Ni` are `-0.75V` and `-0.24V`, respectively, find out the concentration of `Ni^(2+)` in solution at equilibrium.

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Zinc granules are added in excess to 500 mL of 1M Ni(NO_(3))_(2) solution of 25^(@)C untill the equilibrium is reached. If E_(Zn^(2+)//Zn)^(@) and E_(Ni^(2+)//Ni)^(@) are -0.75V and -0.24V respectively, find out the [Ni^(2+)] at equilibrium.

Calculate the standard potential of the cell ,If the standard electrode potentials of Zn^(2+)//Zn and Ag^(+) //Ag are -0.763 V and + 0.799 V respectively .

Standard reduction electrode potential of Zn^(2+)//Zn is -0.76V . This means:

The standard reduction potentials for Zn^(2+)//Zn,Ni^(2+)//Ni and Fe^(2+)//Fe are -0.76,-0.23 and -0.44V respectively. The reaction X+Y^(2+)to X^(2)+Y will be spontaneous when :

The standard reduction potential for Zn^(2+)//Zn, Ni^(2+)//Ni and Fe^(2+)//Fe are -0.76, -0.23 and 0.44V respectively. The reaction X + Y^(2) rarr X^(2+) + Y will be spontaneous when: