With the help of a graph explain why it is not possible to determine λ m ∞ for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte.

It is not possible to determine λ m ∞ (limiting molar conductivity) for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte. Because weak electrolyte dissociated to a much lesser extent as compared to a strong electrolyte. There is a large increase in conductance with dilution near the infinite dilution, it is due the concentration of the weak electrolyte is reduced.

With the help of a graph explain why it is not possible to determine λ m ∞ for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte.

It is not possible to determine λ m ∞ (limiting molar conductivity) for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte. Because weak electrolyte dissociated to a much lesser extent as compared to a strong electrolyte. There is a large increase in conductance with dilution near the infinite dilution, it is due the concentration of the weak electrolyte is reduced.

The conductivity of 0 . 10 M solution of KCl at 298 K is 0 . 0129 S cm - 1 . Calculate its molar conductivity.

Given: The concentration of the solution = 0 . 10 M The conductivity of the solution k = 0 . 0129 S cm - 1 = 1 . 29 × 10 - 2 ohm - 1 cm - 1 Molar conductivity, ∧ m = k × 1000 M ohm - 1 cm 2 mol - 1 = 1 . 29 × 10 - 2 × 1000 0 . 10 ohm - 1 cm 2 mol - 1 = 129 ohm - 1 cm 2 mol - 1

The molar conductivity of 0 . 05 M BaCl 2 solution at 25 ° C is 223 Ω - 1 cm 2 mol - 1 . What is its conductivity?

Given, Concentration ( C ) = 0 . 05 M Molar conductivity ( λ m ) = 223 Ω - 1 cm 2 mol - 1 As we know, Molar conductivity, λ m = 1000 × k C ⋯ ⋯ ⋯ ⋯ ( i ) ∴ k = λ m × C 1000 ⋯ ⋯ ⋯ ⋯ ⋯ ( ii ) Put all the values in equation ii , = 223 × 0 . 05 1000 = 0 . 01115 S cm - 1 or Ω - 1 cm - 1 Therefore, the molar conductivity of BaCl 2 solution is 0 . 01115 S cm - 1 or Ω - 1 cm - 1 .

Match List - I with List - II : List - I (Parameter) List - II (Unit) (a) Cell constant (i) S cm 2 mol - 1 (b) Molar conductivity (ii) Dimensionless (c) Conductivity (iii) m - 1 (d) Degree of dissociation of electrolyte (iv) Ω - 1 m - 1

(a)-(iii), (b)-(i), (c)-(iv), (d)-(ii)

(a)-(iii), (b)-(i), (c)-(ii), (d)-(iv)

(a)-(iii), (b)-(iv), (c)-(i), (d)-(ii)

(a)-(ii), (b)-(i), (c)-(iii), (d)-(iv)

MEDIUM

Earn 100

With the help of a graph explain why it is not possible to determine $λ_{m}^{\infty}$ for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte.

Important Questions on Electrochemistry

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivities of

HCl, NaCl, {CH}_{3} COOH

and

{CH}_{3} COONa

at infinite dilution follow the order

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

291 K

, saturated solution of

{BaSO}_{4}

was found to have a specific conductivity of

3.648 \times 10^{- 6} {ohm}^{- 1} {cm}^{- 1}

and that of water being used is

1.25 \times 10^{- 6} {ohm}^{- 1} {cm}^{- 1}

. If the ionic conductance's of

{Ba}^{2 +}

and

{SO}_{4}^{2 -}

are

110

and

136.6 {ohm}^{- 1} {cm}^{2} {mol}^{- 1}

respectively, the solubility of

{BaSO}_{4}

291 K

will be [Atomic masses of

Ba - 137, S - 32, 0 - 16]

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

In the plot of molar conductivity $(\land_{m})$ vs square root of concentration $(c^{1 / 2})$ , following curves are obtained for two electrolytes A and B :

Question Image

Answer the following :
Predict the nature of electrolytes A and B.

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The specific conductivity of a solution containing

5

g of anhydrous

{BaCl}_{2}

( molecular weight

= 208

) in

1000 {cm}^{3}

of a solution is found to be

0.0058 {ohm}^{- 1} {cm}^{- 1}

. Calculate the molar and equivalent conductivity of the solution.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The pair of electrolytes that possess same value for the constant

(A)

in the Debye - Huckel - Onsagar equation,

λ_{m} = λ_{m} ° - A \sqrt{C}

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Define the equivalent conductivity.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The resistance of conductivity cell with cell constant

1.14 {cm}^{- 1}

, containing

0.001 M KCl

298 K

1500 Ω

. The molar conductivity of

0.001 M KCl

solution at

298 K

S {cm}^{2} {mol}^{- 1}

is (Integer answer)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The conductivity of

0.10 M

solution of

KCl

298 K

0.0129 S {cm}^{- 1}

. Calculate its molar conductivity.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The graph of

\sqrt{C} vs \land_{m}

for an aqueous solution of which substance is not obtained as a straight line?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Given below are two statements:
Statement I : The limiting molar conductivity of $KCl$ (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:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

State Kohlrausch law of independent migration of ions. Write an expression for the molar conductivity of acetic acid at infinite dilution according to Kohlrausch. law.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Give a reason for the following.
Conductivity of dilute hydrochloric acid is greater than that of acetic acid.

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Define molar conductivity of a solution. Explain how molar conductivity changes with change in concentration of solution for a weak and a strong electrolyte.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivity of a

0.5 mol {dm}^{- 3}

solution of

A g N O_{3}

with electrolytic conductivity of

5.76 \times 10^{- 3} S c m^{- 1}

298 K

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivity of

0.05 M {BaCl}_{2}

solution at

25 ° C

223 Ω^{- 1} {cm}^{2} {mol}^{- 1}

. What is its conductivity?

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Define the following and write the formula and unit :

Equivalent conductivity

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Distinguish between electronic conduction and electrolytic conduction.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Match List - I with List - II :

	List - I (Parameter)		List - II (Unit)
(a)	Cell constant	(i)	$S {cm}^{2} {mol}^{- 1}$
(b)	Molar conductivity	(ii)	Dimensionless
(c)	Conductivity	(iii)	$m^{- 1}$
(d)	Degree of dissociation of electrolyte	(iv)	$Ω^{- 1} m^{- 1}$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Which one of the following graphs between molar conductivity

(Λ_{m})

versus

\sqrt{C}

is correct?

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Resistance of 0.2 M solution of an electrolyte is

50 Ω

. The specific conductance of the solution is

{1.4 S m}^{-1}

. The resistance of 0.5 M solution of the same electrolyte is

280 Ω

. The molar conductivity of 0.5 M solution of the electrolyte in

{S m}^{2} {mol}^{-1}

is :

With the help of a graph explain why it is not possible to determine λm∞ for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte.

Important Questions on Electrochemistry

Learn and Prepare for any exam you want !

With the help of a graph explain why it is not possible to determine $λ_{m}^{\infty}$ for a weak electrolyte by extrapolating the concentration-molar conductance curve as for strong electrolyte.