Variation of Molar Conductivity With Concentration

Determine the degree of ionization and pH of a $0.05 \mathrm{M}$ of ammonia solution. The ionization constant of ammonia is $1.77 \times {10}^{-5}$.

The molar conductivity of a solution at infinite dilution is known as _____ molar conductivity.

The dissociation of a weak electrolyte increases on dilution.

In the relationship, ${\mathrm{\lambda }}_{\mathrm{c}}={\mathrm{\lambda }}_{\infty }-\left(\mathrm{B}\right)\sqrt{\mathrm{C}}$, the equivalent conductance of $\mathrm{NaCl}$ at concentration $\mathrm{C}$ related with the equivalent conductance at _____.

Conductivity of a solution decreases with dilution, whereas molar conductivity increases with dilution.

Dilution increases the conductivity of the weak electrolyte. How does the conductivity of ionic solution measured?

The dissociation constant is inversely proportional to the square root of its concentration. Prove it.

How does the dilution affect the conductivity of the strong electrolytes?

Express the effect of dilution on molar conductivity of the strong electrolyte.

Molar conductivity of ionic solution depends on _____.(temperature/distance between electrodes)

Molar conductivity of ionic solution depends on _____.

How does the variation in molar conductivity of an electrolyte with concentration differs for strong and weak electrolytes?

How does molar conductivity of an electrolyte vary with concentration?

The constant 'A' in the equation  ${\mathrm{\lambda }}_{\mathrm{m}}^0={\mathrm{\lambda }}_{\mathrm{m}}+\mathrm{A}\sqrt{\mathrm{C}}$ is depends on- 

Given,

$\mathrm{\lambda }$ of $0.01 \mathrm{M} {\mathrm{MgCl}}_2 \mathrm{is} 220 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$

$\mathrm{\lambda }°$ of ${\mathrm{MgCl}}_2 \mathrm{is} 240 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$

$\mathrm{\lambda }°$ of ${\mathrm{Mg}}^{2+} \mathrm{is} 100 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$

All above measurements are done in an electrolytic cell. Assuming ${\mathrm{MgCl}}_2$ to be a strong electrolyte which of the following is/are incorrect?

Equivalent conductance of 1M CH₃COOH is 10 ohm^-1 cm² equiv^-1 and that at infinite dilution is 200 ohm^-1 cm², equiv^-1. Hence % ionisation of CH₃COOH is :

For strong electrolytes the plot of molar conductance $vs\sqrt{C}$ is

The ${\mathrm{p}}^{\mathrm{H}}$ of $0.005 \mathrm{M}$ acid solution. What is the percentage ionization of the acid?

The equivalent conductance of NaCl at concentration C and at infinite dilution are ${\lambda }_{\text{C}}$ and ${\lambda }_{\infty }$, respectively. The correct relationship between ${\lambda }_{\text{C}}$ and ${\lambda }_{\infty }$ is given as :
(where the constant B is positive)

Conductivity of 0.00241 M acetic acid is 7.896 x 10^-5 S cm^-1 
Calculate its molar conductivity. If ${\Lambda }_{\text{m}}^{\text{o}}$ for acetic acid is 390.5 S cm² mol^-1, what is its dissociation constant ?