Conductance in Electrolytic Solutions

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S  $c{m}^2$  $mo{l}^{-1}.$  Calculate the conductivity of the solution.

The molar conductivity of a $1.5 \mathrm{M}$ solution of an electrolyte is found to be$138.9 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. Calculate the conductivity of the solution?

The resistance of a conductivity cell containing 0.001 M KCI solution at 298 K is 1500  $\Omega .$  The cell constant would be (if the conductivity of 0.001 M KCI solution at 298 K is  $0.146\times {10}^{-3}\text{S}{\text{cm}}^{-1}$  ):  

The conductivity of centimolar solution of $\mathrm{KCl}$ at $25°\mathrm{C}$ is $0.0210 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$ and the resistance of the cell containing the solution at $25°\mathrm{C}$ is $60 \mathrm{ohm}$. The value of cell constant is

The specific conductance of $0.0025\mathrm{M}$ acetic acid is $5\times {10}^{-5} \mathrm{S} {\mathrm{cm}}^{-1}$ at a certain temperature. The dissociation constant of acetic acid is ___________ $\times {10}^{-7}$.(Nearest integer)

Consider limiting molar conductivity of ${\mathrm{CH}}_3\mathrm{COOH}$ as $400 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$

The number of correct statements from the following is ___________

(A) Conductivity always decreases with decrease in concentration for both strong and weak electrolytes.

(B) The number of ions per unit volume that carry current in a solution increases on dilution.

(C) Molar conductivity increases with decrease in concentration.

(D) The variation in molar conductivity is different for strong and weak electrolytes.

(E) For weak electrolytes, the change in molar conductivity with dilution is due to decrease in degree of dissociation.

How many of the following statements are correct :
1. Conductivity decreases with increase in dilution, for both strong and weak electrolyte.
2. Molar conductivity increases with increase in dilution for both strong and weak electrolyte.
3. Molar conductivity increases with increase in '$\mathrm{\alpha }$' for weak electrolyte.
4. Change in molar conductivity is same for both strong and weak electrolyte with increase in dilution.

Draw a well labelled diagram for testing the conductivity of salt solution.

What is specific conductance of a solution ? How it varies with dilution?

Why the electrical conductivity of the solution produced by adding little sulphuric acid into pure water is more than the electrical conductivity of pure water?

Equal volumes of $0.015 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH} \& 0.015 \mathrm{M} \mathrm{NaOH}$ are mixed together. What would be the molar conductivity of mixture if conductivity of ${\mathrm{CH}}_3\mathrm{COONa}$ is $6.3\times {10}^{-4} \mathrm{S} {\mathrm{cm}}^{-1}$

A weak monobasic acid $\mathrm{HA}$ is $3\%$ dissociated in $0.02\mathrm{M}$ solution. The limiting molar conductivity at infinite dilution is $6.5\times {10}^{-2} \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. The molar conductivity of $0.5\mathrm{M}$ solution of this acid is

$0.2 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution is diluted to $0.02 \mathrm{M}$ ${\mathrm{H}}_2{\mathrm{SO}}_4$. Hence, the molar conductivity will be

Specific conductance of $0.1\mathrm{M} {\mathrm{HNO}}_3$ is $6.3\times {10}^{-2} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$. The molar conductance of the solution is

The molar conductivity is maximum for the solution of concentration

A potential difference of $20 \mathrm{V}$ applied to the ends of a column of $\frac{\mathrm{N}}{10} {\mathrm{AgNO}}_3$ solution, $4 \mathrm{cm}$ in diameter and $12 \mathrm{cm}$ in length gives a current of $1.198$ amperes. Calculate the specific and equivalent conductivity of the solution.