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Consider the following aqueous solutions and assume 100% ionization in electrolytes
1. 0.1 m urea 2 . 0.04 m Al2(SO4)3
3. 0.05 m CaCl2 4. 0.005 m NaCl
3. 0.05 m CaCl2 4. 0.005 m NaCl
The correct statement regarding the above solutions is
- a)Freezing point will be lowest for solution 1
- b)Freezing point will be highest for solution 4
- c)Boiling point will be highest for solution 3
- d)Vapour presure will be highest for solution 2
Correct answer is option 'D'. Can you explain this answer?
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Explanation:
The freezing point depression and boiling point elevation of a solution depend on the number of solute particles in the solution. The greater the number of solute particles, the greater the effect on the colligative properties of the solution.
1. 0.1 m urea: Urea is a non-electrolyte and does not dissociate into ions in water. Therefore, it does not increase the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be the least for this solution.
2. 0.04 m Al2(SO4)3: Aluminum sulfate dissociates into three ions (2Al3+ and 3SO42-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1.
3. 0.05 m CaCl2: Calcium chloride dissociates into three ions (1Ca2+ and 2Cl-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1 and 2.
4. 0.005 m NaCl: Sodium chloride dissociates into two ions (1Na+ and 1Cl-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1 but lower than solution 2 and 3.
Therefore, the correct statement regarding the above solutions is that the vapour pressure will be highest for solution 2 as it has the highest number of solute particles. Higher the number of solute particles, the lower the vapour pressure.
The freezing point depression and boiling point elevation of a solution depend on the number of solute particles in the solution. The greater the number of solute particles, the greater the effect on the colligative properties of the solution.
1. 0.1 m urea: Urea is a non-electrolyte and does not dissociate into ions in water. Therefore, it does not increase the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be the least for this solution.
2. 0.04 m Al2(SO4)3: Aluminum sulfate dissociates into three ions (2Al3+ and 3SO42-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1.
3. 0.05 m CaCl2: Calcium chloride dissociates into three ions (1Ca2+ and 2Cl-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1 and 2.
4. 0.005 m NaCl: Sodium chloride dissociates into two ions (1Na+ and 1Cl-) in water. Therefore, it increases the number of solute particles in the solution. Hence, the freezing point depression and boiling point elevation will be higher than solution 1 but lower than solution 2 and 3.
Therefore, the correct statement regarding the above solutions is that the vapour pressure will be highest for solution 2 as it has the highest number of solute particles. Higher the number of solute particles, the lower the vapour pressure.
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Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer?
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Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. 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 Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. 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 Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer?.
Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. 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 Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. 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 Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer?.
Solutions for Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
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Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer?, a detailed solution for Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice Consider the following aqueous solutions and assume 100% ionization in electrolytes1. 0.1 m urea 2 . 0.04 m Al2(SO4)33. 0.05 m CaCl2 4. 0.005 m NaClThe correct statement regarding the above solutions isa)Freezing point will be lowest for solution 1b)Freezing point will be highest for solution 4c)Boiling point will be highest for solution 3d)Vapour presure will be highest for solution 2Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice Class 12 tests.
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