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Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq), 0.25 M KBr (aq), 0.125 M Na3PO4 (aq). Which statement is true about these solutions, assuming all salts to be strong electrolytes ?
- a)They all have same osmotic pressure
- b)0.1 M Mg3(PO4)2 (aq) has higher osmotic pressure
- c)0.125 M Na3PO4 (aq) has higher osmotic pressure
- d)0.5M C2H5OH (aq)has higher osmotic pressure
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq),...
Option A
They all have the same osmotic pressure
effective molarity = Van't Hoff factor x molarity
0.5 M C2H5OH (aq) i =1
Effective molarity = 0.5
0.25 M KBr (aq) i = 2
Effective molarity = 0.5
0.1 M Mg3(PO4)2 (aq) i = 5
Effective molarity = 0.5 M
0.125 M Na3PO4 (aq)
Effective molarity = 0.5 M
Hence, all colligative properties are same.
Most Upvoted Answer
Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq),...
Solution:
Introduction:
Osmotic pressure is a colligative property that depends on the concentration of solute particles in a solution. It is defined as the pressure required to stop the flow of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration.
Explanation:
In this question, we are given four separate solutions with different concentrations. Let's analyze each solution to determine the osmotic pressure.
1. 0.5M C2H5OH (aq):
- Ethanol (C2H5OH) is a covalent compound that does not dissociate into ions in water.
- Since it does not dissociate, it does not contribute to the osmotic pressure.
- Therefore, the osmotic pressure of this solution is zero.
2. 0.1 M Mg3(PO4)2 (aq):
- Mg3(PO4)2 is a salt that dissociates into ions in water: 3Mg2+ and 2PO42-.
- The concentration of ions is calculated by multiplying the molarity by the number of ions produced: 3 x 0.1 M = 0.3 M Mg2+ and 2 x 0.1 M = 0.2 M PO42-.
- The osmotic pressure is directly proportional to the concentration of solute particles, so this solution has a higher osmotic pressure compared to the ethanol solution.
3. 0.25 M KBr (aq):
- KBr is also a salt that dissociates into ions in water: K+ and Br-.
- The concentration of ions is equal to the molarity: 0.25 M K+ and 0.25 M Br-.
- Compared to the previous solution, the concentration of ions is lower, so the osmotic pressure is lower.
4. 0.125 M Na3PO4 (aq):
- Na3PO4 is a salt that dissociates into ions in water: 3Na+ and PO43-.
- The concentration of ions is calculated by multiplying the molarity by the number of ions produced: 3 x 0.125 M = 0.375 M Na+ and 1 x 0.125 M = 0.125 M PO43-.
- The osmotic pressure is directly proportional to the concentration of solute particles, so this solution has a higher osmotic pressure compared to the KBr solution.
Conclusion:
Based on the analysis of the four solutions, it can be concluded that all the solutions have the same osmotic pressure except for the ethanol solution, which has a zero osmotic pressure. Therefore, option A is the correct answer.
Introduction:
Osmotic pressure is a colligative property that depends on the concentration of solute particles in a solution. It is defined as the pressure required to stop the flow of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration.
Explanation:
In this question, we are given four separate solutions with different concentrations. Let's analyze each solution to determine the osmotic pressure.
1. 0.5M C2H5OH (aq):
- Ethanol (C2H5OH) is a covalent compound that does not dissociate into ions in water.
- Since it does not dissociate, it does not contribute to the osmotic pressure.
- Therefore, the osmotic pressure of this solution is zero.
2. 0.1 M Mg3(PO4)2 (aq):
- Mg3(PO4)2 is a salt that dissociates into ions in water: 3Mg2+ and 2PO42-.
- The concentration of ions is calculated by multiplying the molarity by the number of ions produced: 3 x 0.1 M = 0.3 M Mg2+ and 2 x 0.1 M = 0.2 M PO42-.
- The osmotic pressure is directly proportional to the concentration of solute particles, so this solution has a higher osmotic pressure compared to the ethanol solution.
3. 0.25 M KBr (aq):
- KBr is also a salt that dissociates into ions in water: K+ and Br-.
- The concentration of ions is equal to the molarity: 0.25 M K+ and 0.25 M Br-.
- Compared to the previous solution, the concentration of ions is lower, so the osmotic pressure is lower.
4. 0.125 M Na3PO4 (aq):
- Na3PO4 is a salt that dissociates into ions in water: 3Na+ and PO43-.
- The concentration of ions is calculated by multiplying the molarity by the number of ions produced: 3 x 0.125 M = 0.375 M Na+ and 1 x 0.125 M = 0.125 M PO43-.
- The osmotic pressure is directly proportional to the concentration of solute particles, so this solution has a higher osmotic pressure compared to the KBr solution.
Conclusion:
Based on the analysis of the four solutions, it can be concluded that all the solutions have the same osmotic pressure except for the ethanol solution, which has a zero osmotic pressure. Therefore, option A is the correct answer.
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Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq), 0.25 M KBr (aq), 0.125 M Na3PO4 (aq). Which statement is true about these solutions, assuming all salts to be strong electrolytes ?a)They all have same osmotic pressureb)0.1 M Mg3(PO4)2 (aq) has higher osmotic pressurec)0.125 M Na3PO4 (aq) has higher osmotic pressured)0.5M C2H5OH (aq)has higher osmotic pressureCorrect answer is option 'A'. Can you explain this answer?
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Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq), 0.25 M KBr (aq), 0.125 M Na3PO4 (aq). Which statement is true about these solutions, assuming all salts to be strong electrolytes ?a)They all have same osmotic pressureb)0.1 M Mg3(PO4)2 (aq) has higher osmotic pressurec)0.125 M Na3PO4 (aq) has higher osmotic pressured)0.5M C2H5OH (aq)has higher osmotic pressureCorrect answer is option 'A'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq), 0.25 M KBr (aq), 0.125 M Na3PO4 (aq). Which statement is true about these solutions, assuming all salts to be strong electrolytes ?a)They all have same osmotic pressureb)0.1 M Mg3(PO4)2 (aq) has higher osmotic pressurec)0.125 M Na3PO4 (aq) has higher osmotic pressured)0.5M C2H5OH (aq)has higher osmotic pressureCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider separate solutions of 0.5M C2H5OH (aq), 0.1 M Mg3(PO4)2 (aq), 0.25 M KBr (aq), 0.125 M Na3PO4 (aq). Which statement is true about these solutions, assuming all salts to be strong electrolytes ?a)They all have same osmotic pressureb)0.1 M Mg3(PO4)2 (aq) has higher osmotic pressurec)0.125 M Na3PO4 (aq) has higher osmotic pressured)0.5M C2H5OH (aq)has higher osmotic pressureCorrect answer is option 'A'. Can you explain this answer?.
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