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Chem355 Cell Constant and Determinant of Molar Conductance of MgSO4, Schemes and Mind Maps of Chemistry

Middle East Technical UniversityChemistry

Report Sheet Author:Gülden Karaçam

Typology: Schemes and Mind Maps

2024/2025

Uploaded on 04/10/2025

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CHEM 355
PHYSICAL CHEMISTRY LABORATORY
EXPERIMENT NUMBER: 1
NAME OF THE EXPERIMENT: Cell Constant and Determination of Molar
Conductance of MgSO4
DATE OF THE EXPERIMENT: 14.03.2025
NAME OF THE ASSISTANT: Çağatay Can
GROUP NUMBER: 9
STUDENT NAME SURNAME: Gülden Karaçam
GROUP MEMBERS: A. Safa Çomoğlu, Furkan Vural
SECTION: 3 (Friday Afternoon)
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CHEM 355

PHYSICAL CHEMISTRY LABORATORY

EXPERIMENT NUMBER: 1

NAME OF THE EXPERIMENT: Cell Constant and Determination of Molar

Conductance of MgSO 4

DATE OF THE EXPERIMENT: 14.03.

NAME OF THE ASSISTANT: Çağatay Can

GROUP NUMBER: 9

STUDENT NAME SURNAME: Gülden Karaçam

GROUP MEMBERS: A. Safa Çomoğlu, Furkan Vural

SECTION: 3 (Friday Afternoon)

CALCULATIONS

1. From equation 3, we can calculate the cell constant (B);

B = κ

G

S

cm

×

14.13 ms

×

1000 ms 1 S =0.9122 cm − 1

2. From equation 3, we can calculate the specific conductance of 0.0125M

of MgSO 4 solution;

κ = B ×G =0.9122 cm − 1 × 2.33 ms ×

1 S

1000 ms

=¿ 2.13*10-3^ S.cm-

Applying the same procedure to other solutions,

Concentration (M) Specific Conductance (S.cm

-

From equation 4, we can calculate molar conductivity of 0.0125M of

MgSO 4 solution;

κ c

− 3 S. cm − 1 0.0125 mol / L

×

1000 cm 3 1 L =170.4 S. cm 2

. mol − 1

Applying the same procedure to other solutions,

Concentration (M) Molar conductivity (S.cm

2

.mol

-

Applying the same procedure for other solutions of monochloroacetic acid;

Concentration (M) Molar conductivity (S.cm^2 .mol-1)

0.004 0.006 0.008 0.01 0.012 0.014 0.016 0.018 0.02 0. 0

f(x) = 0.302917985970754 x − 0.

Λ*c vs 1/Λ graph

1/Λ (mol/S.cm2) Λ*c (S/cm)

From the graph, Λ *c=Kd Λ 0

2

/ Λ -Kd Λ 0

Kd Λ 0

2

=0.3029 and Kd Λ 0 =0.

Divide this values; Λ 0 =432.

Kd=0.0007/432.9=1.61*10-6mol/L

From the equation 6, we calculated the degree of dissociation for every

solution;

αmean= Λ / Λ 0 =0.

From the equation 7,

Kdmean= Λ^2 c/ Λ 0 ( Λ 0 - Λ )= 1.6810-

Theoretical value of Kd of monochloroacetic acid is 1.35*

. Therefore,

percent error is;

( 1.68−1.35) × 10 −^3

1.35 × 10

− 3 ∗^100 =%^ 24.

Theoretical value of Λ 0 for MgSO 4 is 106 S.cm

2

.mol

. Therefore, percent error is;

Theoretical value of Λ 0 for monochloroacetic acid is 389 S.cm^2 .mol-1. Therefore

percent error is;

QUESTIONS

1. According to the Ostwald law the degree of dissociation (α) of a weak

electrolyte is inversely proportional to the square root of molar

concentration.

2. The nature of the electrolyte (weak or strong), temperature of the

solution and concentration of the solution affect the conductivity.

3. Because it is soluble and stable salt. Sodium sulfate, sodium chloride

or sodium bicarbonate salts can be used for calibration because they

are also stable salts.

4. When different concentration of solutions are compared we must use

specific conductance and molar conductivity for more accurate and

useful results. Also, comparing different types of electrolytes (in this

case weak and strong) these values is more reliable instead of

conductance.

5. Theoretical value of Kd of monochloroacetic acid is 1.35*

Therefore, percent error is;

( 1.68−1.35) × 10 −^3

1.35 × 10

− 3 ∗^100 =%^ 24.

Theoretical value of Λ 0 for MgSO 4 is 106 S.cm^2 .mol-1. Therefore, percent error is;

Theoretical value of Λ 0 for monochloroacetic acid is 389 S.cm

2

.mol

. Therefore

percent error is;