21. Can a solution of 1M cuso4 stored in a Nickel metal vessel E^° Ni2+/Ni=-0.25V & E^° cu2+/Cu=+0.34V

Open in App

Solution

Suggest Corrections

Similar questions

Q. In which metal container, the aqueous solution of

C u {S O}_{4}

can be stored?

E_{{C u}^{2 +} / C u}^{o} = 0.34 V

E_{{F e / F e}^{2 +}}^{o} = 0.44 V, E_{{A l / A l}^{3 +}}^{o} = 1.66 V

E_{N i / {N i}^{2 +}}^{o} = 0.25 V, E_{{A g}^{+} / A g}^{o} = 0.80 V

Can 1M $N i S O_{4}$ be stored in a vessel of copper? Given that $E_{\frac{{N i}_{2 +}}{N i}}^{0}$ = -1.20 V and E°Cu2+/Cu =0.34V

Q. Calculate the

E

and

E^{\circ}

of the cell

N i | N i^{2 +} | | C u^{2 +} | C u

from the following half-cell reactions:

N i^{2 +} + 2 e^{-} \to N i; E^{\circ} = - 0.25 v o l t

C u^{2 +} + 2 e^{-} \to C u; E^{\circ} = + 0.34 v o l t

(Given:

[N i^{2 +}] = 1 M

and

[C u^{2 +}] = 10^{- 3} M)

The SRP values of Zn, Ag, Ni and Cu electrodes are -0.76V, 0.80V, 0.25V and 0.34V respectively in which container $C u S O_{4}$ solution should be stored:

Given;

E_{C u^{2 +} | C u}^{⊖} = 0.34 V, E_{Z n^{2 +} | Z n}^{⊖} = - 0.76 V

E_{A g^{\oplus} | A g}^{⊖} = 0.80 V

Assertion: Copper sulphate solution can be stored in silver vessel.

Reason:

E_{c e l l}^{⊖}

is positive.

Join BYJU'S Learning Program