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Fewer ions per unit volume carry the current, so conductivity drops as you dilute.
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E = E° − (RT/nF) ln Q
At 298 K this becomes E = E° − (0.059/n) log Q.
For a cell, Q uses the product and reactant ion concentrations.
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• Electrode potential at any concentration: E = E° − (0.059/n) log Q at 298 K.
• For a Daniell cell, Q = [Zn²⁺]/[Cu²⁺], so diluting Cu²⁺ lowers Ecell.
• At equilibrium Ecell = 0, which gives log Kc = nE°/0.059.
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Conductivity and molar conductivity both change with the concentration of the electrolyte.
Conductivity always decreases with decrease in concentration, for both weak and strong electrolytes.
This is because the number of ions per unit volume that carry the current decreases on dilution.
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