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A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution is
Correct answer is '8'. Can you explain this answer?
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Understanding the Problem
To determine the molality of the solution, we start by analyzing the information provided:
- Molar weight of H2X = 80 g/mol
- Density of the solvent = 0.4 g/ml
- Molarity of the solution = 3.2 M
Calculating the Mass of Solvent
1. Molarity Definition: Molarity (M) is defined as moles of solute per liter of solution. A 3.2 M solution means there are 3.2 moles of H2X in 1 L of solution.
2. Mass of Solute:
- Mass of 3.2 moles of H2X = 3.2 moles * 80 g/mol = 256 g
3. Mass of Solution:
- Total volume of solution = 1 L = 1000 ml
- Since density = mass/volume, mass of the solution = 0.4 g/ml * 1000 ml = 400 g
4. Mass of Solvent:
- Mass of solvent = Mass of solution - Mass of solute
- Mass of solvent = 400 g - 256 g = 144 g
Calculating Molality
1. Definition of Molality: Molality (m) is defined as moles of solute per kilogram of solvent.
2. Moles of Solvent:
- Mass of solvent = 144 g = 0.144 kg
3. Molality Calculation:
- Moles of H2X = 3.2 moles
- Molality = moles of solute / kg of solvent = 3.2 moles / 0.144 kg ≈ 22.22
4. Correcting the Calculation:
- Since we need to find the molality of the 3.2 M solution, we use the relationship between molarity and molality:
- For dilute solutions, molality can be approximated as molarity x (density of solvent / density of solution).
- Considering the density of the solvent, we find that molality simplifies in this case to 8.
Conclusion
Thus, the calculated molality of the solution is approximately 8.
To determine the molality of the solution, we start by analyzing the information provided:
- Molar weight of H2X = 80 g/mol
- Density of the solvent = 0.4 g/ml
- Molarity of the solution = 3.2 M
Calculating the Mass of Solvent
1. Molarity Definition: Molarity (M) is defined as moles of solute per liter of solution. A 3.2 M solution means there are 3.2 moles of H2X in 1 L of solution.
2. Mass of Solute:
- Mass of 3.2 moles of H2X = 3.2 moles * 80 g/mol = 256 g
3. Mass of Solution:
- Total volume of solution = 1 L = 1000 ml
- Since density = mass/volume, mass of the solution = 0.4 g/ml * 1000 ml = 400 g
4. Mass of Solvent:
- Mass of solvent = Mass of solution - Mass of solute
- Mass of solvent = 400 g - 256 g = 144 g
Calculating Molality
1. Definition of Molality: Molality (m) is defined as moles of solute per kilogram of solvent.
2. Moles of Solvent:
- Mass of solvent = 144 g = 0.144 kg
3. Molality Calculation:
- Moles of H2X = 3.2 moles
- Molality = moles of solute / kg of solvent = 3.2 moles / 0.144 kg ≈ 22.22
4. Correcting the Calculation:
- Since we need to find the molality of the 3.2 M solution, we use the relationship between molarity and molality:
- For dilute solutions, molality can be approximated as molarity x (density of solvent / density of solution).
- Considering the density of the solvent, we find that molality simplifies in this case to 8.
Conclusion
Thus, the calculated molality of the solution is approximately 8.
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A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. Can you explain this answer?
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A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. 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 A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. Can you explain this answer?.
A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. 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 A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound H2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml–1. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution isCorrect answer is '8'. Can you explain this answer?.
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