Consider the cell: Ni ∣ Ni²⁺ (?M) || Cu²⁺(0.136 M) ∣ Cu
Ni²⁺/Ni E° = -0.257 V
Cu²⁺/Cu E° = 0.340 V
The measured potential of the cell is 0.621 V. What is [Ni²⁺] at 25°C?

Question

Consider the cell: Ni ∣ Ni²⁺ (?M) || Cu²⁺(0.136 M) ∣ Cu Ni²⁺/Ni E° = -0.257 V Cu²⁺/Cu E° = 0.340 V The measured potential of the cell is 0.621 V. What is [Ni²⁺] at 25°C?

Quizplus · Accepted Answer

The cell potential is calculated using the Nernst equation. The standard cell potential (E°cell) is 0.340 V - (-0.257 V) = 0.597 V. The measured potential is 0.621 V, which is higher than the standard potential, indicating a lower concentration of Ni²⁺. Using the Nernst equation, solve for [Ni²⁺]: 0.621 V = 0.597 V - (0.0592/2)log([Ni²⁺]/0.136). Solving gives [Ni²⁺] = 2 × 10⁻² M.

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