Kohlrausch's Law and its Application

The molar conductance and the specific conductance of an electrolyte are related by the formula

The molar conductance of $0.01 \mathrm{M}$ electrolyte is $124 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ at $298 \mathrm{K}$. Calculate its specific conductance.

The specific conductance of $0.01 \mathrm{M}$ of an electrolyte is $1.24\times {10}^{-3} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$ at $298 \mathrm{K}$. Calculate the molar conductance.

Calculate the molar conductance of $0.02 \mathrm{M}$ solution of an electrolyte which has a resistance of $310 \mathrm{ohm}$ at $298 \mathrm{K}$. Cell constant is $0.68 {\mathrm{cm}}^{-1}$.

The equivalent conductivity of acetic acid at infinite dilution is $387 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{eq}}^{-1}$. At the same temperature, for $0.001 \mathrm{M}$ solution of acetic acid, it is $55 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{eq}}^{-1}$. What is the degree of dissociation of $0.1 \mathrm{N}$ acetic acid? Assume $1-\mathrm{\alpha }\approx 1$

$$\begin{gathered} \mathrm{A} : 1.5\% \\ \mathrm{B} : 1.35\% \\ \mathrm{C} : 2\% \end{gathered}$$

Enter your correct answer as A, B or C.

If the value of molar conductivities at infinite dilution for ${\mathrm{CH}}_3\mathrm{COOH}$, $\mathrm{HCl}$ and $\mathrm{NaCl}$ are $390.5, 425.4$and $126.4 \mathrm{S} {\mathrm{cm}}^2{\mathrm{mol}}^{-1}$ respectively at $298 \mathrm{K}$. Calculate the molar conductivity at infinite dilution of ${\mathrm{CH}}_3\mathrm{COONa}$ in $\mathrm{S} {\mathrm{cm}}^2{\mathrm{mol}}^{-1}$. (Just mention the value, no requirement of units in the answer).

The maximum molar conductivities of ${\mathrm{X}}^{+3}$ and ${\mathrm{Y}}^{-}$ ions are $200$ and $100 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ respectively. The molar conductivity of ${\mathrm{XY}}_3$ at infinite dilution is :-

Define limiting molar conductivity $\left(\mathrm{\Lambda }{°}_{\mathrm{m}}\right)$.

${\wedge }_{\mathrm{m} \left({\mathrm{NH}}_4\mathrm{OH}\right)}^0$ is equal to _____.

What is the molar conductivity of $\mathrm{AgI}$ at zero concentration if the ${\wedge }_0$ values of $\mathrm{NaI}, {\mathrm{AgNO}}_3$ and ${\mathrm{NaNO}}_3$ are respectively $126.9 {\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$, $133.4 {\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$, $121.5 {\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$?

How is the molar conductivity of strong electrolytes at zero concentration determined by graphical method? Why is this method not useful for weak electrolytes?

The molar conductivities at zero concentrations of ${\mathrm{NH}}_4\mathrm{Cl}, \mathrm{NaOH}$ and $\mathrm{NaCl}$ are respectively $149.7{\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}, 248.1{\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$ and $126.5{\mathrm{\Omega }}^{-1}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}.$ What is the molar conductivity of ${\mathrm{NH}}_4\mathrm{OH}$ at zero concentration?

The equivalent conductance of $\text{1}\text{M}$ benzoic acid is $\text{12.8 }\mathrm{o}\mathrm{h}{\mathrm{m}}^{-1}\mathrm{c}{\mathrm{m}}^2$ and if the conductance of benzoate ion and ${\mathrm{H}}^{+}$ ion at infinite dilution are $42$ and $\text{288.42}\hspace{0.33em}\mathrm{o}\mathrm{h}{\mathrm{m}}^{-1}\mathrm{c}{\mathrm{m}}^2$ respectively. Calculate percentage of degree of dissociation.
Report your answer by rounding upto nearest whole number.

The ionization constant of a weak monobasic acid is $25\times 10^{–6}$ while the equivalent conductance of its $0.01\mathrm{ }\mathrm{M}$ solution is $19.6\mathrm{ }\mathrm{S}\mathrm{c}{\mathrm{m}}^2\mathrm{e}{\mathrm{q}}^{–1}$ . The equivalent conductance of the electrolyte at infinite dilution $\left(\mathrm{i}\mathrm{n}\mathrm{ }\mathrm{S}\mathrm{c}{\mathrm{m}}^2\mathrm{e}{\mathrm{q}}^{–1}\right)$ will be

The conductivity of $0.001028 mol L^{-1}$ acetic acid is $4.95\times {10}^{-5}S c{m}^{-1}.$ Find out its dissociation constant if ${\wedge }_m$ for acetic acid is $390.5\mathrm{ }\mathrm{S}\mathrm{ }{\mathrm{cm}}^2{\mathrm{mol}}^{-1}.$

At 298 K, the molar conductivities at infinite dilution $\left({\wedge }_{\text{m}}^{\text{o}}\right)$ of $\text{N}{\text{H}}_4\text{C}\text{l},\text{K}\text{O}\text{H}$ and $\text{K}\text{C}\text{l}$ are 152.8, 272.6 and 149.8 S $\text{c}{\text{m}}^2\text{m}\text{o}{\text{l}}^{-1}$ respectively. The ${\wedge }_{\text{m}}^{\text{o}}$ of $\text{N}{\text{H}}_4\text{O}\text{H}$ in $\text{S}\text{c}{\text{m}}^2\text{m}\text{o}{\text{l}}^{-1}$ and % dissociation of 0.01 M $\text{N}{\text{H}}_4\text{O}\text{H}$ with ${\wedge }_{\text{m}}=25.1\text{S}\text{c}{\text{m}}^2\text{m}\text{o}{\text{l}}^{-1}$ at the same temperature are

Find out ionisation constant of a weak acid (HA) in terms of ${\mathrm{\Lambda }}_{\text{m}}^{\text{o}}$ and ${\mathrm{\Lambda }}_{\text{m}}^{\text{c}}$? (Given $\text{"}\alpha \text{"}$ can not be ignored with respect to1).

Which statement is not correct for Kohlrausch law?

The equivalent conductivity of $0.1\mathrm{ }\mathrm{M}$ weak acid is $100\mathrm{ }$times lesser than that at infinite dilution. The degree of dissociation of weak electrolyte at $0.1\mathrm{ }\mathrm{M}$ is -

The limiting molar conductivities ${\wedge }^{0\mathrm{ }}$for $\mathrm{NaCl},\mathrm{ }\mathrm{KBr}$ and $\mathrm{KCl}$ are $126, 152$ and $150\mathrm{ }{\mathrm{Scm}}^2{\mathrm{mol}}^{-1}$ respectively. The ${\wedge }^0$ for $\mathrm{NaBr}$ is: