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I have a set of NaCl solutions with concentrations ranging from 0.05 M to 0.1 M. I have been trying to calculate the conductivity of these solutions and compare the obtained values with the experimental ones obtained with a conductometer.

For this, I used the Kohlrausch's Law. But I observe some deviation on the values. I realized that the law may not apply for high concentrated solutions such as 0.1M. I read that since NaCl is a strong electrolyte, this law should still apply.

Is there a specific law or method to use to calculate the conductivity of concentrated solutions?

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You can use the Debye-Hückel-Onsager limiting law. For a strong electrolyte without the formation of ionic pairs, with $z_+ = |z_-|$, just like $\ce{NaCl}$: $$ \Lambda_m = \Lambda_m^\infty - (az_+^3 + bz_+^3\Lambda_m^\infty)(c/c^\circ)^{1/2}$$ For aqueous solutions at $25^\circ$C and $1$ atm: $a = 60.6 \, \Omega^{-1}\mathrm{cm}^2\,\mathrm{mol}^{-1}$, $b = 0.230$. For $\ce{NaCl}$, $\Lambda_m^\infty = 126.4 \, \Omega^{-1}\mathrm{cm}^2\,\mathrm{mol}^{-1}$.

References

Ira N. Levine, Physical Chemistry, 6th Ed.

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