In a concentration cell, if the concentration of the anode is 0.1 M and the cath

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Question: In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1.0 M, what is the cell potential at 25°C?

Options:

Correct Answer: 0.118 V

Solution:

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(10) = 0.059 V.

In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1.0 M, what is the cell potential at 25°C?

In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1.0 M, what is the cell potential at 25°C?

Step 1: Identify the concentrations of the anode and cathode. The anode concentration is 0.1 M and the cathode concentration is 1.0 M.
Step 2: Use the formula for cell potential: E = (0.059 V/n) * log([Cathode]/[Anode]).
Step 3: Determine 'n', the number of electrons transferred in the reaction. For a concentration cell involving a simple metal ion, n is typically 2.
Step 4: Substitute the values into the formula: E = (0.059 V/2) * log(1.0/0.1).
Step 5: Calculate the log value: log(1.0/0.1) = log(10) = 1.
Step 6: Now calculate E: E = (0.059 V/2) * 1 = 0.059 V.

Concentration Cell – A type of electrochemical cell where the electrodes are made of the same material but are in different concentrations of electrolyte.
Nernst Equation – A formula used to calculate the cell potential based on the concentrations of the reactants and products.
Logarithmic Relationships – Understanding how to apply logarithms in the context of the Nernst equation to find cell potential.