Conductance in Electrolytic Solutions

$1\times {10}^{-5} \mathrm{M} {\mathrm{AgNO}}_3$ is added to $1 \mathrm{L}$ of saturated solution of $\mathrm{AgBr}$. The conductivity of this solution at $298 \mathrm{K}$ is $\_\_\_\_\_\_\_\times {10}^{-8} \mathrm{S} {\mathrm{m}}^{-1}$.

[Given : ${\mathrm{K}}_{\mathrm{sp}}\left(\mathrm{AgBr}\right)=4.9\times {10}^{-13}$ at $298 \mathrm{K}$

${\lambda }_{{\mathrm{Ag}}^{+}}^0=6\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}$

${\lambda }_{{\mathrm{Br}}^{-}}^0=8\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}$

$\left.{\lambda }_{{\mathrm{NO}}_3^{-}}^0=7\times {10}^{-3}{\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}\right]$

The resistivity of a $0.8\mathrm{M}$ solution of an electrolyte is $5\times {10}^{-3}\mathrm{\Omega cm}$. Its molar conductivity is ${10}^4{\mathrm{\Omega }}^{-1} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. (Nearest integer)

Following figure shows dependence of molar conductance of two electrolytes on concentration. ${\mathrm{\Lambda }}_{\mathrm{m}}^0$ is the limiting molar conductivity.

The number of Incorrect statement(s) from the following is _____

(A) ${\mathrm{\Lambda }}_{\mathrm{m}}^0$ for electrolyte $\mathrm{A}$ is obtained by extrapolation
(B) For electrolyte $\mathrm{B}, {\mathrm{\Lambda }}_{\mathrm{m}} \mathrm{Vs} \sqrt{\mathrm{c}}$  graph is a straight line with intercept equal to ${\mathrm{\Lambda }}_{\mathrm{m}}^0$
(C) At infinite dilution, the value of degree of dissociation approach zero for electrolyte $\mathrm{B}$.
(D) ${\mathrm{\Lambda }}_{\mathrm{m}}$ for any electrolyte $\mathrm{A}$ or $\mathrm{B}$ can be calculated using $\mathrm{\lambda }°$ for individual ions.

Choose the correct representation of conductometric titration of benzoic acid vs sodium hydroxide.

Resistance of a conductivity cell (cell constant $129{ \mathrm{m}}^{-1}$) filled with $74.5\mathrm{ppm}$ solution of $\mathrm{KCl}$ is $100 \mathrm{\Omega }$ (labelled as solution $1$). When the same cell is filled with $\mathrm{KCl}$ solution of $149\mathrm{ppm}$, the resistance is $50 \mathrm{\Omega }$ (labelled as solution $2$). The ratio of molar conductivity of solution $1$ and solution $2$ is i.e. $\frac{{\wedge }_1}{{\wedge }_2}=\mathrm{x}\times {10}^{-3}$. The value of $\mathrm{x}$ is____Given, molar mass of $\mathrm{KCl}$ is $74.5 \mathrm{g}{ \mathrm{mol}}^{-1}$)

The molar conductivity of a conductivity cell filled with $10$ moles of $20 \mathrm{mL} \mathrm{NaCl}$ solution is ${\mathrm{\Lambda }}_{\mathrm{m}1}$ and that of $20$ moles another identical cell heaving $80 \mathrm{mL} \mathrm{NaCl}$ solution is ${\mathrm{\Lambda }}_{\mathrm{m}2}$, The conductivities exhibited by these two cells are same.

The relationship between ${\mathrm{\Lambda }}_{\mathrm{m}2}$ and ${\mathrm{\Lambda }}_{\mathrm{m}1}$ is

Given below are two statements:

Statement I: For $\mathrm{KI}$, molar conductivity increases steeply with dilution.

Statement II: For carbonic acid, molar conductivity increases slowly with dilution. In the light of the above statements, choose the correct answer from the options given below

The solubility product of a sparingly soluble salt ${\mathrm{A}}_2{\mathrm{X}}_3$ is $1.1\times {10}^{-23}$. If specific conductance of the solution is $3\times {10}^{-5}{\mathrm{Sm}}^{-1}$, the limiting molar conductivity of the solution is $\mathrm{a}\times {10}^{-3} \mathrm{S} {\mathrm{m}}^2 {\mathrm{mol}}^{-1}$. The value of $\mathrm{a}$ is:

The resistance of a conductivity cell containing $0.01 \mathrm{MKCl}$ solution at $298 \mathrm{K}$ is $1750 \mathrm{\Omega }$. If the conductivity of $0.01 \mathrm{MKCl}$ solution at $298 \mathrm{K}$
is $0.152\times {10}^{-3} \mathrm{S}{ \mathrm{cm}}^{-1}$, then the cell constant of the conductivity cell is____$\times {10}^{-3}{ \mathrm{cm}}^{-1}$

The resistance of conductivity cell with cell constant $1.14{ \mathrm{cm}}^{-1}$, containing $0.001\mathrm{M} \mathrm{KCl}$ at $298 \mathrm{K}$ is $1500\Omega$. The molar conductivity of $0.001\mathrm{M} \mathrm{KCl}$ solution at $298 \mathrm{K}$ in $\mathrm{S} {\mathrm{cm}}^2{ \mathrm{mol}}^{-1}$ is (Integer answer)

Match List - I with List - II :

Given below are two statements:
Statement I : The limiting molar conductivity of $\mathrm{KCl}$ (strong electrolyte) is higher compared to that of $\mathrm{CH}_{3} \mathrm{COOH}$ (weak electrolyte).
Statement II : Molar conductivity decreases with decrease in concentration of electrolyte.

In the light of the above statements, choose the most appropriate answer from the options given below:

The conductivity of a weak acid$\mathrm{HA}$ of concentration $0.001 \mathrm{mol}{ \mathrm{L}}^{-1}$ is $2.0\times {10}^{-5} \mathrm{S}{ \mathrm{cm}}^{-1}$. If ${\Lambda }_{\mathrm{m}}^0\left(\mathrm{HA}\right)=190 \mathrm{S}{ \mathrm{cm}}^2{ \mathrm{mol}}^{-1},$ the ionization constant $\left({\mathrm{K}}_{\mathrm{a}}\right)$ of $\mathrm{HA}$ is equal to $\_\_\_\_$ $\times {10}^{-6}$
(Round off to the Nearest Integer)

A $5.0 \mathrm{m} \mathrm{mol} {\mathrm{dm}}^{-3}$ aqueous solution of $\mathrm{KCl}$ has a conductance of $0.55 \mathrm{mS}$ when measured in a cell constant $1.3{ \mathrm{cm}}^{-1}$. The molar conductivity of this solution is _______ ${\mathrm{mSm}}^2{ \mathrm{mol}}^{-1}$. (Round off to the Nearest Integer)

A $\mathrm{KCl}$ solution of conductivity $0.14 \mathrm{S}{ \mathrm{m}}^{-1}$ shows a resistance of $4.19\mathrm{\Omega }$ in a conductivity cell. If the same cell is filled with an $\mathrm{HCl}$ solution, the resistance drops to $1.03\Omega$. The conductivity of the HCl solution is ____$\times {10}^{-2} \mathrm{S}{ \mathrm{m}}^{-1}$. (Round off to the Nearest Integer).

The molar conductivity at infinite dilution of barium chloride, sulphuric arid and hydrochloric acid are $280, 860$ $426 {\mathrm{Scm}}^2{\mathrm{mol}}^{-1}$ respectively. The molar conductivity at infinite dilution of barium sulphate is ___ ${\mathrm{Scm}}^2{ \mathrm{mol}}^{-1}$ ( Round off to the Nearest Integer).

The variation of molar conductively with concentration of an electrolyte (X) in aqueous solution is shown in the given figure.

The electrolyte X is :

Which one of the following graphs between molar conductivity $\left({\mathrm{\Lambda }}_{\mathrm{m}}\right)$ versus $\sqrt{\mathrm{C}}$ is correct?

Consider the statements $\mathrm{S}1$ and $\mathrm{S}2$ :
$\mathrm{S}1$ : Conductivity always increases with decreases in the concentration of electrolyte.
$\mathrm{S}2$ : Molar conductivity always increases with decreases in the concentration of electrolyte.
The correct option among the following

The equivalent conductance of $\mathrm{NaCl}$ 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)