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(D) On dilution,the volume of the solution increases,which reduces the inter-ionic attractions. Additionally,for weak electrolytes,the degree of disso

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Degree of ionisation of the electrolyte

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(D) On dilution,the volume of the solution increases,which reduces the inter-ionic attractions. Additionally,for weak electrolytes,the degree of dissociation increases with dilution. However,the primary reason for the increase in equivalent conductance for both strong and weak electrolytes is the increase in the degree of dissociation (for weak electrolytes) and the reduction in inter-ionic attraction (for strong electrolytes). Among the given options,the increase in the degree of ionisation is the most significant factor for the observed increase in equivalent conductance.

The increase in equivalent conductance of an electrolyte solution with dilution is due to the increase in

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Assertion : On increasing dilution,the specific conductance keeps on increasing.
Reason : On increasing dilution,the degree of ionization of a weak electrolyte increases and the mobility of ions also increases.

At $25\,^{\circ}C$,the molar conductivity at infinite dilution for electrolytes $KOH$,$KCl$ and $BaCl_2$ are $248 \times 10^{-4}$,$126 \times 10^{-4}$ and $280 \times 10^{-4}\,S\,m^2\,mol^{-1}$ respectively. Calculate $\Lambda _m^{\infty}$ for $Ba(OH)_2$ (in $S\,m^2\,mol^{-1}$).

The conductivity of $0.20 \ M \ KCl$ solution at $300 \ K$ is $0.0248 \ \Omega^{-1} \ cm^{-1}$. What is its molar conductivity?

Which of the following concentrations of $KCl$ solution has the lowest value of equivalent conductivity (in $M$)?

How can the ionic conductivity of an unknown solution be determined?

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