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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively:
- a)0.2 m urea
- b)0.1 m glucose
- c)0.1 m MgSO4
- d)0.1 m BaCI2
Correct answer is option 'A'. Can you explain this answer?
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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation i...
Whenever we dissolve nonvolatile solute (ki) in a volatile solvent (such as H20), the vapour pressure of the resulting solution is always less than the vapour pressure of the solvent because in a pure solvent the entire surface is occupied by molecules of the solvent but in the solution, the surface has both solute and solvent molecules. There-by, the number of solvent molecules gets reduced. Consequently the number of solvent molecules escaping from the surface is corresponding reduced. Thus the vapour pressure is also reduced.
on adding water.,the vapour pressure of the solution will increase on account of increase in the number of volatile component on the surface (H20).
on adding water.,the vapour pressure of the solution will increase on account of increase in the number of volatile component on the surface (H20).
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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation i...
Solution:
In order to determine whether a compound undergoes dissociation or association in a particular solvent, we need to consider the nature of the solute and the solvent.
a) Urea (0.2 m)
Urea is a non-ionic compound, meaning it does not dissociate into ions in solution. Therefore, it does not undergo dissociation in any solvent.
b) Glucose (0.1 m)
Glucose is also a non-ionic compound and does not dissociate into ions in solution. Therefore, it does not undergo dissociation in any solvent.
c) MgSO4 (0.1 m)
MgSO4 is an ionic compound and dissociates into Mg2+ and SO4^2- ions in solution. Therefore, it undergoes dissociation in all solvents.
d) BaCl2 (0.1 m)
BaCl2 is also an ionic compound and dissociates into Ba2+ and 2Cl- ions in solution. Therefore, it undergoes dissociation in all solvents.
a) KI (1.0 molal)
KI is an ionic compound and dissociates into K+ and I- ions in solution. Therefore, it undergoes dissociation in all solvents.
Based on the above analysis, we can conclude that option 'A' (0.2 m urea) is the correct answer. Urea does not undergo dissociation in any solvent, while all the other compounds undergo dissociation in all solvents.
In order to determine whether a compound undergoes dissociation or association in a particular solvent, we need to consider the nature of the solute and the solvent.
a) Urea (0.2 m)
Urea is a non-ionic compound, meaning it does not dissociate into ions in solution. Therefore, it does not undergo dissociation in any solvent.
b) Glucose (0.1 m)
Glucose is also a non-ionic compound and does not dissociate into ions in solution. Therefore, it does not undergo dissociation in any solvent.
c) MgSO4 (0.1 m)
MgSO4 is an ionic compound and dissociates into Mg2+ and SO4^2- ions in solution. Therefore, it undergoes dissociation in all solvents.
d) BaCl2 (0.1 m)
BaCl2 is also an ionic compound and dissociates into Ba2+ and 2Cl- ions in solution. Therefore, it undergoes dissociation in all solvents.
a) KI (1.0 molal)
KI is an ionic compound and dissociates into K+ and I- ions in solution. Therefore, it undergoes dissociation in all solvents.
Based on the above analysis, we can conclude that option 'A' (0.2 m urea) is the correct answer. Urea does not undergo dissociation in any solvent, while all the other compounds undergo dissociation in all solvents.
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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer?
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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer?.
Solutions for An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
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An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer?, a detailed solution for An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer? has been provided alongside types of An aqueous solution is 1.0 molal in KI. Which undergoes dissociation in one solvent and association in other solvent is respectively: a)0.2 m urea b)0.1 m glucose c)0.1 m MgSO4 d)0.1 m BaCI2Correct answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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