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Molar Conductance Determination of MgSO4 and Monochloroacetic Acid, Schemes and Mind Maps of Chemistry

Middle East Technical University Chemistry

This laboratory experiment focuses on determining the molar conductance of mgso4 and monochloroacetic acid using conductivity measurements. The experiment involves calculating the cell constant, specific conductance, and molar conductivity of the solutions. It also explores the relationship between molar conductivity and concentration, and the determination of the dissociation constant (kd) and degree of dissociation (α) for monochloroacetic acid. The experiment provides a practical understanding of conductivity measurements, electrolyte behavior, and the application of arrhenius's theory and ostwald's dilution law.

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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)

Partial preview of the text

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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

×

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

.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)

Molar Conductance Determination of MgSO4 and Monochloroacetic Acid, Schemes and Mind Maps of Chemistry

Related documents

Partial preview of the text

Download Molar Conductance Determination of MgSO4 and Monochloroacetic Acid and more Schemes and Mind Maps Chemistry in PDF only on Docsity!

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);

G

S

×

×

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

of MgSO 4 solution;

1 S

=¿ 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;

×

Applying the same procedure to other solutions,

Concentration (M) Molar conductivity (S.cm

.mol

Applying the same procedure for other solutions of monochloroacetic acid;

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

Λ*c vs 1/Λ graph

From the graph, Λ *c=Kd Λ 0

/ Λ -Kd Λ 0

Kd Λ 0

=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

.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

.mol