Variation of Specific, Equivalent and Molar Conductivities with Concentration

Q. The molar conductivities at infinite dilution of $AgN{O}_3$ and $NaCl$ are 116.0 and 110.0 $Sc{m}^{2}mo{l}^{-1}$ respectively. The conductivity of $AgCl$ in water is $8.42\times {10}^{-6}Sc{m}^{–1}$ and of water used is $1.16\times {10}^{-6}Sc{m}^{–1}$. The solubility of $AgCl$ is $6.0\times {10}^{-5}mol/L$. Find the molar conductivity at infinite dilution of $NaN{O}_3$ ($inSc{m}^{-1}mo{l}^{-1}$) in the solution.

Q. The molar conductivities of $AgN{O}_3,NaCl$ and $NaN{O}_3$ at infinite dilution are 116.0, 110.0 and $105.0Sc{m}^{2}mo{l}^{–1}$ , respectively. The conductivity of $AgCl$ in water is $8.42\times {10}^{-6}Sc{m}^{–1}$ and of water used is $1.16\times {10}^{–6}Sc{m}^{-1}$. Find the solubility of AgCl in $mollitr{e}^{–1}$

1. $7.92\times {10}^{-5}$
2. $9.58\times {10}^{-6}$
   
3. $6.96\times {10}^{-5}$
   
4. $6.0\times {10}^{-5}$

Q.

Which of the following statements is correct for a strong electrolyte :

1. ${\lambda }_m$ increases linearly with $C^{\frac{1}{2}}$

2. ${\lambda }_m$ increases linearly with $C^2$

3. ${\lambda }_m$ decreases linearly with $C^2$

4. ${\lambda }_m$ decreases linearly with $C^{\frac{1}{2}}$

Q. In a conductometric titration experiment, a solution of $0.1{\text{M Ba(OH)}}_2$ is titrated against a solution of $0.1{\text{M MgSO}}_4$ and the conductance of the mixture is continuously measured. The correct variation of conductance of the reaction mixture with the titration volume of ${\text{MgSO}}_4$ is best represented by

1. 
2. 
3. 
4. 

Q. Molar conductivity decreases with decrease in concentration

1. True
2. False

Q. ${\wedge }_m={\wedge }_m^o-k\sqrt{C}$ is valid for

1. Weak electrolytes only
2. strong electrolytes only
3. both weak and strong electrolytes
4. Non electrolytes

Q. The molar conductivities of $AgN{O}_3,NaCl$ and $NaN{O}_3$ at infinite dilution are 116.0, 110.0 and $105.0Sc{m}^{2}mo{l}^{–1}$ , respectively. The conductivity of $AgCl$ in water is $8.42\times {10}^{-6}Sc{m}^{–1}$ and of water used is $1.16\times {10}^{–6}Sc{m}^{-1}$. Find the solubility of AgCl in $mollitr{e}^{–1}$

1. $7.92\times {10}^{-5}$
2. $9.58\times {10}^{-6}$
   
3. $6.96\times {10}^{-5}$
   
4. $6.0\times {10}^{-5}$