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Chapter 5: Problem 14

Which of the following solution would exhibit abnormal colligative properties? (a) \(1 \mathrm{M}\) glucose (b) \(0.1 \mathrm{M} \mathrm{NaCl}\) (c) \(0.1 \mathrm{M}\) sucrose (d) 10 gram glass powder in water

Short Answer

Expert verified
Glass powder in water exhibits abnormal colligative properties.

Step by step solution

01

Understanding Colligative Properties

Colligative properties depend on the number of solute particles in a solution, not their identity. These include properties like boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure lowering.
02

Identifying Normal Solutes

From the choices, glucose, NaCl, and sucrose are common solutes that typically dissolve to form solutions with predictable colligative properties. Glucose and sucrose are non-electrolytes, while NaCl is an electrolyte that dissociates into ions.
03

Evaluating Each Choice

(a) A 1 M glucose solution is expected to show normal colligative properties for a non-electrolyte. (b) A 0.1 M NaCl solution will dissociate into Na鈦� and Cl鈦� ions, exhibiting normal colligative properties for an electrolyte. (c) A 0.1 M sucrose solution will behave typically for a non-electrolyte. (d) Glass powder does not dissolve in water; it forms a suspension, not a solution, and does not affect colligative properties.
04

Conclusion

Since glass powder does not dissolve and does not alter colligative properties in water, it represents an abnormal case as it cannot exhibit colligative properties in the way solutions do.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Non-electrolytes
Non-electrolytes are substances that dissolve in a solvent without dissociating into ions. They usually form solutions that do not conduct electricity. Common examples include organic molecules like glucose and sucrose. When non-electrolytes like these dissolve in water, the resulting solution exhibits predictable colligative properties. This happens because the solute particles do not split into smaller charged entities.
  • Non-electrolytes do not change the ionic strength of the solution.
  • They have a straightforward effect on colligative properties because the number of particles remains constant.
  • In solutions of non-electrolytes, properties such as boiling point elevation and freezing point depression depend solely on the concentration of the solute.
Hence, when you make a solution with glucose or sucrose, you can expect it to follow normal colligative behavior due to its nature as a non-electrolyte.
Electrolytes
Electrolytes, in contrast to non-electrolytes, are compounds that dissociate into ions when dissolved in water. This dissociation into positive and negative ions enables the solution to conduct electricity. A familiar example of an electrolyte is sodium chloride (NaCl), which dissociates into Na鈦� and Cl鈦� ions in solution.
  • Electrolytes increase the ionic strength of the solution, affecting properties like electrical conductivity.
  • In electrolytic solutions, colligative properties are affected by the number of ions formed.
  • A solution containing an electrolyte like NaCl will exhibit colligative properties based on the total number of ions in the solution, increasing effects like boiling point elevation and osmotic pressure.
It's important to note that electrolytic solutions can show more pronounced colligative properties due to the presence of multiple particles from dissociation.
Suspensions
Suspensions are mixtures where fine particles are dispersed throughout a liquid but do not dissolve. An example from our exercise is glass powder in water. Unlike true solutions, the particles in a suspension are large enough to be seen with the naked eye and are not affected by colligative properties.
  • Suspensions do not involve solute particles interacting on a molecular level with the solvent.
  • They do not alter boiling point, freezing point, or osmotic pressure because the particles don't dissolve.
  • Upon standing, particles in a suspension tend to settle out due to gravity, distinguishing them from colloids or solutions.
Thus, since suspensions like glass powder in water don't form homogeneous mixtures, they do not conform to the typical behaviors associated with colligative properties.

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Most popular questions from this chapter

A solution is obtained by dissolving \(6 \mathrm{~g}\) of urea (mol. wt = 60) in a litre solution, another solution is prepared by dissolving \(34.2 \mathrm{~g}\) of cane sugar (mol. \(\mathrm{wt}=342\) ) in a litre of solution at the same temperature The lowering of vapour pressure in the first solution is (a) same as that of second solution (b) double that of second solution (c) half that of second solution (d) nearly one fifth of the second solution

A pressure cooker reduces cooking time for food because (a) heat is more evenly distributed in the cooking space (b) boiling point of water involved in cooking is increased (c) the higher pressure inside the cooker crushes the food material (d) cooking involves chemical changes helped by a rise in temperature

A liquid is in equilibrium with its vapour at its boiling point. On the average, the molecules in the two phase have equal (a) intermolecular forces (b) potential energy (c) temperature (d) kinetic energy

KBr is \(80 \%\) dissociated in aqueous solution of \(0.5 \mathrm{M}\) concentration. (Given \(\mathrm{K}_{f}\) for water \(=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\) ). The solution freezes at (a) \(271.326 \mathrm{~K}\) (b) \(272 \mathrm{~K}\) (c) \(270.5 \mathrm{~K}\) (d) \(268.5 \mathrm{~K}\)

\(50 \mathrm{~mL}\) of \(10 \mathrm{~N} \mathrm{H}_{2} \mathrm{SO}_{4}, 25 \mathrm{~mL}\) of \(12 \mathrm{~N} \mathrm{HCl}\) and \(40 \mathrm{~mL}\) of \(5 \mathrm{~N} \mathrm{HNO}_{3}\) are mixed and the volume of the mixture is made \(1000 \mathrm{~mL}\) by adding water. The normality of resulting solution will be (a) \(9 \mathrm{~N}\) (b) \(4 \mathrm{~N}\) (c) \(1 \mathrm{~N}\) (d) \(2 \mathrm{~N}\)
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