The measured resistance of a conductance cell containing 7 . 5 × 10 - 3 M solution of KCl at 25 ° C was 1005 ohms. Calculate specific conductance. Cell constant = 1 . 25 cm - 1 .

Given, Resistance of a conductance cell, R = 1005 ohm . Cell constant of the cell, = 1 . 25 cm - 1 . Specific conductance is defined as the conductance between the opposite electrodes of one-centimetre cube of conductor. It can be calculated by, κ = 1 Resistance × cell constant . κ = 1 1005 × 1 . 25 = 0 . 001243 S cm - 1 . κ = 1 . 243 × 10 - 3 S cm - 1 .

The measured resistance of a conductance cell containing 7 . 5 × 10 - 3 M solution of KCl at 25 ° C was 1005 ohms. Calculate specific conductance. Cell constant = 1 . 25 cm - 1 .

Given, Resistance of a conductance cell, R = 1005 ohm . Cell constant of the cell, = 1 . 25 cm - 1 . Specific conductance is defined as the conductance between the opposite electrodes of one-centimetre cube of conductor. It can be calculated by, κ = 1 Resistance × cell constant . κ = 1 1005 × 1 . 25 = 0 . 001243 S cm - 1 . κ = 1 . 243 × 10 - 3 S cm - 1 .

In a conductivity cell, electrodes of 4 cm 2 area of cross-section are placed at a distance of 2 cm from each other. At 298 K , a M 100 solution of an electrolyte recorded a resistance of 350 Ω . Determine the molar conductivity of the electrolyte.

Area of electrode, a = 4 cm 2 Distance between the electrodes l = 2 cm Therefore, cell constant K cell = l a = 2 cm 4 cm 2 = 0 . 5 cm - 1 Resistance offered by the solution = 350 Ω Concentration of the solution = M 100 = 0 . 01 mol dm 3 Then, Conductivity of the solution κ = Cell constant Resistance = 0 . 5 cm - 1 350 Ω = 0 . 00143 Scm - 1 Molar conductivity λ m = 1000 κ C m = 1000 × 0 . 00143 Scm - 1 0 . 01 moldm - 3 = 143 Scm 2 mol - 1

The resistance of a conductivity cell containing 0 . 001 M KCl at 298 K is 1500 Ω if the conductance of 0 . 001 M KCl at 298 K is 0 . 146 × 10 - 3 S cm - 1 , what is the cell constant?

Cell constant is defined as the ratio of the distance between the electrodes divided by the area of cross-section of the electrode Given that Resistance = 1500 Ω k = 0 . 146 × 10 - 3 We know that, k = Gx , where k = conductivity , G = 1 R , x = cell constant 0 . 146 × 10 - 3 = 1 1500 × x x = 0 . 146 × 10 - 3 × 1500 = 0 . 219 cm - 1

What is the molar conductivity of 0 · 1 M NaCl if its conductivity is 1 . 06 × 10 - 2 Ω - 1 cm - 1 ?

1 · 06 × 10 2 Ω - 1 cm 2 mol - 1

1 · 06 × 10 - 2 Ω - 1 cm 2 mol - 1

9 · 4 × 10 - 2 Ω - 1 cm 2 mol - 1

5 · 3 × 10 3 Ω - 1 cm 2 mol - 1

EASY

Earn 100

The measured resistance of a conductance cell containing $7.5 \times 10^{- 3} M$ solution of $KCl$ at $25 ° C$ was $1005$ ohms. Calculate specific conductance. Cell constant $= 1.25 {cm}^{- 1}$ .

Important Questions on Electrochemistry

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The specific conductance of an aqueous

{KNO}_{3}

solution at

298 K,

for a fixed concentration is

0.024 {ohm}^{- 1} {cm}^{- 1} .

If the resistance of a cell containing this solution at

298 K

was found to be

85 ohm,

then find its cell constant.

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

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

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivities

(λ_{m}^{0})

at infinite dilution of

KBr, HBr

and

{KNH}_{2}

are

120.5, 420.6

and

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

respectively. Find the value of

λ_{m}^{0}

for

{NH}_{3}

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The S.I. unit of cell constant for conductivity cell is :

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivities of

NaOH, NaCl

and

{BaCl}_{2},

at infinite dilution are

2.481 \times 10^{- 2} {Sm}^{2} {mol}^{- 1} 1.265 \times 10^{- 2} {Sm}^{2} {mol}^{- 1}

and

2.800 \times 10^{- 2} {Sm}^{2} {mol}^{- 1}

respectively. The molar conductivity of

Ba {(OH)}_{2}

. at infinite dilution will be

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The resistance of a conductivity cell containing $0.001 M KCl$ solution at $298 K$ is $1500 ohm$ . What is the cell constant and molar conductivity of $0.001 M KCl$ solution, if the conductivity of this solution is $0.146 \times 10^{- 3} {ohm}^{- 1} {cm}^{- 1}$ at $298 K$ ?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The resistance of

0.01 M KCl

solution at

298 K

1500 Ω .

If the conductivity of

0.01 M KCl

solution at

298 K

0.1466 \times 10^{- 3} S {cm}^{- 1} .

The cell constant of the conductivity cell in

{cm}^{- 1}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Resistance of conductivity cell filled with

0.1 mol L^{- 1} KCl

solution is

100 ohm

. If the resistance of the same cell when filled with

0.03 mol L^{- 1} KCl

solution is

520 ohm

, calculate the conductivity and molar conductivity of

0.03 mol L^{- 1} KCl

solution. The conductivity of

0.1 mol L^{- 1} KCl

solution is

1.29 S m^{- 1}

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

If the resistivity of

0.1 M KCl

solution is

50 Ω cm .

What is its molar conductivity?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

KCl

solution of conductivity

0.14 S m^{- 1}

shows a resistance of

4.19 Ω

in a conductivity cell. If the same cell is filled with an

HCl

solution, the resistance drops to

1.03 Ω

. The conductivity of the HCl solution is ____

\times 10^{- 2} S m^{- 1}

. (Round off to the Nearest Integer).

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The resistance of a conductivity cell containing

0.001 MKCl

solution at

298 K

1500 Ω

. What is the cell constant if the conductivity of

0.001 MKCl

solution at

298 K

0.146 \times 10^{- 3} {Scm}^{- 1} .

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

Among the following, the plot that correctly represents the conductometric titration of

0.05 M

H_{2} {SO}_{4}

with

0.1 M {NH}_{4} OH

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The standard molar conductivity $Λ_{m}^{°}$ for $NaCl, HCl$ and ${CH}_{3} COONa$ are $126.4 S {cm}^{2} {mol}^{- 1}, 425.9 S {cm}^{2} {mol}^{- 1}$ and $91.0 S {cm}^{2} {mol}^{- 1}$ respectively. Calculate $Λ_{m}^{°}$ for ${CH}_{3} COOH$ .

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The limiting molar conductivities of the given electrolytes at $298 K$ follow the order

$λ_{(K^{+})}^{\circ} = 735 S {cm}^{2} {mol}^{- 1}, λ_{({Cl}^{-})}^{\circ} = 763 S {cm}^{2} {mol}^{- 1}, λ_{({Ca}^{2 +})}^{\circ} = 1190 S {cm}^{2} {mol}^{- 1}, λ_{({SO}_{4}^{2 -})}^{\circ} = 160.0 S {cm}^{2} {mol}^{- 1}$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

In a conductivity cell, electrodes of

4 {cm}^{2}

area of cross-section are placed at a distance of

2 cm

from each other. At

298 K

, a

\frac{M}{100}

solution of an electrolyte recorded a resistance of

350 Ω

. Determine the molar conductivity of the electrolyte.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The resistance of a conductivity cell containing

0.001 M

KCl

298 K

1500 Ω

if the conductance of

0.001 M

KCl

298 K

0.146 \times 10^{- 3} S {cm}^{- 1}

, what is the cell constant?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

What is cell constant? What is the relation between specific conductivity and cell constant?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

The molar conductivity at infinite dilution of barium chloride, sulphuric arid and hydrochloric acid are

280, 860

426 {Scm}^{2} {mol}^{- 1}

respectively. The molar conductivity at infinite dilution of barium sulphate is ___

{Scm}^{2} {mol}^{- 1}

( Round off to the Nearest Integer).

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

At a particular temperature, the ratio of molar conductance to specific conductance of

0.01 M

NaCl

solution is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Conductance in Electrolytic Solutions

What is the molar conductivity of

0 \cdot 1 M NaCl

if its conductivity is

1.06 \times 10^{- 2} Ω^{- 1} {cm}^{- 1}

The measured resistance of a conductance cell containing 7.5×10-3 M solution of KCl at 25 °C was 1005 ohms. Calculate specific conductance. Cell constant =1.25 cm-1.

Important Questions on Electrochemistry

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The measured resistance of a conductance cell containing $7.5 \times 10^{- 3} M$ solution of $KCl$ at $25 ° C$ was $1005$ ohms. Calculate specific conductance. Cell constant $= 1.25 {cm}^{- 1}$ .