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Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:
[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]
[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]
- a)50%
- b)60%
- c)70%
- d)80%
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
Solute A associates in water. When 0.7 g of solute A is dissolved in 4...
°C. The freezing point depression constant for water (Kf) is 1.86 °C/m.
To calculate the molality of the solution, we need to find the moles of solute A and the mass of the solvent (water) in kg.
Moles of solute A = 0.7 g / molar mass of A
Assuming we don't know the molar mass of A, we can use its association factor (i) to calculate the effective molar mass:
i = (van't Hoff factor) = (moles of particles in solution) / (moles of solute dissolved)
Since A associates in water, the van't Hoff factor is greater than 1. Let's assume it's 2 for now:
i = 2 = (moles of particles) / (moles of A)
moles of particles = 2 x moles of A
moles of A = 0.7 g / (effective molar mass of A)
Substituting the second equation into the first:
2 = (moles of particles) / (0.7 g / effective molar mass of A)
Solving for the effective molar mass:
effective molar mass of A = 0.7 g / (2 x 2) = 0.175 g/mol
Now we can calculate the moles of solute A:
moles of A = 0.7 g / 0.175 g/mol = 4.0 mol
Next, we need to convert the mass of water to kg:
mass of water = 42.0 g = 0.042 kg
Now we can calculate the molality:
molality = moles of solute / mass of solvent (in kg)
molality = 4.0 mol / 0.042 kg = 95.2 m
Therefore, the molality of the solution is 95.2 m.
To calculate the molality of the solution, we need to find the moles of solute A and the mass of the solvent (water) in kg.
Moles of solute A = 0.7 g / molar mass of A
Assuming we don't know the molar mass of A, we can use its association factor (i) to calculate the effective molar mass:
i = (van't Hoff factor) = (moles of particles in solution) / (moles of solute dissolved)
Since A associates in water, the van't Hoff factor is greater than 1. Let's assume it's 2 for now:
i = 2 = (moles of particles) / (moles of A)
moles of particles = 2 x moles of A
moles of A = 0.7 g / (effective molar mass of A)
Substituting the second equation into the first:
2 = (moles of particles) / (0.7 g / effective molar mass of A)
Solving for the effective molar mass:
effective molar mass of A = 0.7 g / (2 x 2) = 0.175 g/mol
Now we can calculate the moles of solute A:
moles of A = 0.7 g / 0.175 g/mol = 4.0 mol
Next, we need to convert the mass of water to kg:
mass of water = 42.0 g = 0.042 kg
Now we can calculate the molality:
molality = moles of solute / mass of solvent (in kg)
molality = 4.0 mol / 0.042 kg = 95.2 m
Therefore, the molality of the solution is 95.2 m.
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Community Answer
Solute A associates in water. When 0.7 g of solute A is dissolved in 4...
Hence, the percentage association of solute A is 80%.
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Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer?
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Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer?.
Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer?.
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Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer?, a detailed solution for Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2°C. The percentage association of solute A in water is:[Given: Molar mass of A = 93 g mol-1. Molal depression constant of water is 1.86 K kg mol-1.]a)50%b)60%c)70%d)80%Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
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