Question:
How is the molar conductivity of an electrolytic solution calculated?
How is the molar conductivity of an electrolytic solution calculated?
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Molar conductivity is conductivity divided by molar concentration, with a factor of 1000 for unit conversion.
Updated On: Nov 12, 2026
- molar concentration / electrolytic conductivity
- electrolytic conductivity x 1000 / molar concentration
- electrolytic conductivity multiplied by molar concentration
- molar concentration / square of electrolytic conductivity x 1000
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
Molar conductivity is the conductance of all ions produced from 1 mole of electrolyte.
Step 2: Derivation
Conductivity \(\kappa\) is in \(\text{S cm}^{-1}\) and concentration \(c\) in \(\text{mol L}^{-1}\). One litre is 1000 \(\text{cm}^{3}\), so the volume containing 1 mole is \(\dfrac{1000}{c}\text{ cm}^{3}\).
Step 3: Result
\(\Lambda_m=\kappa\times\dfrac{1000}{c}\), in \(\text{S cm}^{2}\text{ mol}^{-1}\).
Final Answer:
Molar conductivity equals conductivity times 1000 divided by molar concentration. \[ \boxed{\text{(B) }\text{electrolytic conductivity}\times1000/\text{molar concentration}} \]
Molar conductivity is the conductance of all ions produced from 1 mole of electrolyte.
Step 2: Derivation
Conductivity \(\kappa\) is in \(\text{S cm}^{-1}\) and concentration \(c\) in \(\text{mol L}^{-1}\). One litre is 1000 \(\text{cm}^{3}\), so the volume containing 1 mole is \(\dfrac{1000}{c}\text{ cm}^{3}\).
Step 3: Result
\(\Lambda_m=\kappa\times\dfrac{1000}{c}\), in \(\text{S cm}^{2}\text{ mol}^{-1}\).
Final Answer:
Molar conductivity equals conductivity times 1000 divided by molar concentration. \[ \boxed{\text{(B) }\text{electrolytic conductivity}\times1000/\text{molar concentration}} \]
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