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The depression of freezing point of a solution of acetic acid in benzene is – 0.2°C. If the molality of acetic acid is 0.1 m, then find the ratio of the normal mass to the abnormal mass. (Assume Kf of acetic acid = 4.0°C m-1)
- a)1.5
- b)0.8
- c)0.5
- d)0.2
Correct answer is option 'C'. Can you explain this answer?
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The depression of freezing point of a solution of acetic acid in benze...
Dependent on the concentration of acetic acid in the solution. The depression of freezing point, also known as the freezing point depression, is a colligative property that is proportional to the molal concentration of solute particles in the solution.
The equation that relates the depression of freezing point (ΔTf) to the molal concentration of solute particles (m) is:
ΔTf = Kf * m
Where:
ΔTf is the depression of freezing point,
Kf is the cryoscopic constant for the solvent (benzene),
m is the molal concentration of solute particles.
The depression of freezing point occurs because the solute particles disrupt the crystal lattice structure of the solvent, making it more difficult for the solvent to freeze. As a result, the freezing point of the solution is lower than that of the pure solvent.
In the case of acetic acid in benzene, the depression of freezing point will increase as the concentration of acetic acid in the solution increases. This is because a higher concentration of solute particles leads to a greater disruption of the solvent crystal lattice and a larger depression of freezing point.
It is important to note that the depression of freezing point is not specific to acetic acid and benzene, but rather a general property of solutions and solvents. The specific values of Kf and the extent of depression of freezing point will vary depending on the solute and solvent involved.
The equation that relates the depression of freezing point (ΔTf) to the molal concentration of solute particles (m) is:
ΔTf = Kf * m
Where:
ΔTf is the depression of freezing point,
Kf is the cryoscopic constant for the solvent (benzene),
m is the molal concentration of solute particles.
The depression of freezing point occurs because the solute particles disrupt the crystal lattice structure of the solvent, making it more difficult for the solvent to freeze. As a result, the freezing point of the solution is lower than that of the pure solvent.
In the case of acetic acid in benzene, the depression of freezing point will increase as the concentration of acetic acid in the solution increases. This is because a higher concentration of solute particles leads to a greater disruption of the solvent crystal lattice and a larger depression of freezing point.
It is important to note that the depression of freezing point is not specific to acetic acid and benzene, but rather a general property of solutions and solvents. The specific values of Kf and the extent of depression of freezing point will vary depending on the solute and solvent involved.
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The depression of freezing point of a solution of acetic acid in benze...
Given,
Depression in freezing point(ΔT) = -0.2 °C
Molality of the solution(m) = 0.1 m
Freezing point depression constant (Kf) = 4.0 °C m-1
Let the Van’t Hoff factor = i
We know that, ΔT = i x Kf x m
0.2 = i x 4 x 0.1
i = 0.2/0.4 = 0.5
Therefore, the ratio between the normal mass and abnormal mass, which is equal to the Van’t Hoff factor is equal to 0.5.
Depression in freezing point(ΔT) = -0.2 °C
Molality of the solution(m) = 0.1 m
Freezing point depression constant (Kf) = 4.0 °C m-1
Let the Van’t Hoff factor = i
We know that, ΔT = i x Kf x m
0.2 = i x 4 x 0.1
i = 0.2/0.4 = 0.5
Therefore, the ratio between the normal mass and abnormal mass, which is equal to the Van’t Hoff factor is equal to 0.5.
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The depression of freezing point of a solution of acetic acid in benzene is – 0.2°C. If the molality of acetic acid is 0.1 m, then find the ratio of the normal mass to the abnormal mass. (Assume Kf of acetic acid = 4.0°C m-1)a)1.5b)0.8c)0.5d)0.2Correct answer is option 'C'. Can you explain this answer?
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The depression of freezing point of a solution of acetic acid in benzene is – 0.2°C. If the molality of acetic acid is 0.1 m, then find the ratio of the normal mass to the abnormal mass. (Assume Kf of acetic acid = 4.0°C m-1)a)1.5b)0.8c)0.5d)0.2Correct answer is option 'C'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about The depression of freezing point of a solution of acetic acid in benzene is – 0.2°C. If the molality of acetic acid is 0.1 m, then find the ratio of the normal mass to the abnormal mass. (Assume Kf of acetic acid = 4.0°C m-1)a)1.5b)0.8c)0.5d)0.2Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The depression of freezing point of a solution of acetic acid in benzene is – 0.2°C. If the molality of acetic acid is 0.1 m, then find the ratio of the normal mass to the abnormal mass. (Assume Kf of acetic acid = 4.0°C m-1)a)1.5b)0.8c)0.5d)0.2Correct answer is option 'C'. Can you explain this answer?.
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