Question

# Which of the following represent the plot of Λm vs √C for a strong electrolyte (KCl)? Λm - Molar conductivity C - concentration of electrolyte

A
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B
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C
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D
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Solution

## The correct option is B For strong electrolyte molar conductivity increases with dilution due to decrease in ion- ion force of attraction. As strong electrolytes are mostly in ionized state, no abrupt change in the number of ions with dilution. Thus, Λm increases slowly with dilution. In concentrated solution there will be a strong attraction between ions which slows down the movement of ion. On dilution of strong electrolyte, distance between the ions increases which results in decrease in ion-ion attraction. So, there will be overall increase in molar conductance of the solution. Variation in molar conductivity of strong electrolyte due to ion-ion interaction is given by an empirical relation proposed by kohlrausch. Λm=Λ0m−A√C Λm - Molar conductivity Λ0m - Limiting molar conductivity C is concentration of electrolyte A is constant for a given solvent and temperature. Λm=Λ0m−A√C This equation is in the form of straight line equation, y=c+mx ∴ Plot of Λm vs √C Intercept : Λ0m Slope : −A Thus, the extrapolation of line gives Λ0m for strong electrolytes.

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