For a cell reaction Cu(s) + 2Ag⁺(aq) → Cu ²⁺+ 2 Ag⁺ (aq) the standard cell potential is 0.46V . By doubling the concentration of Copper(II) ions, The standard cell potential will get:-

double

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increases by less than two

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Halved

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no change

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Solution

The correct option is D
no change

The standard cell potential does not change with the concentration of ions (electrolytes).

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Similar questions

C u (s) + 2 A g^{+} (a q .) \to C u^{2 +} (a q .) + 2 A g (s)

E_{c e l l}^{\circ} = 0.46 V

C u^{2 +}, E_{c e l l}^{\circ}

2 A g^{+} (a q .) + C u (s) ⇌ C u^{2 +} (a q .) + 2 A g (s)

E^{\circ}

0.46 V

C u_{(s)} + 2 A g_{(a q)}^{+} \to C u_{(a q)}^{2 +} + 2 A g_{(s)}

E_{c e l l}^{o} = + 0.46

C u^{2 +}

E_{c e l l}^{o}

2 A g^{+} (a q .) + C u (s) ⇌ C u^{2 +} (a q .) + 2 A g (s) (E_{c e l l}^{\circ} = + 0.46 V)

C u (s) | C u^{2 +} (a q) | | A g^{+} (a q) | A g (s)

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