Unit 9: Solution

What is Solution in Chemistry?

The “Solution” unit in Chemistry focuses on the study of homogeneous mixtures, where one substance (the solute) is uniformly distributed within another substance (the solvent). This unit explores how solutions are formed, their properties, and the factors affecting their concentration and behavior. Understanding solutions is essential for various applications, from chemical reactions to industrial processes and everyday life.

Key Topics in Solution:

• Types of Solutions: Examining different types of solutions based on the state of the solute and solvent, including solid, liquid, and gas solutions.
• Concentration: Understanding how to express and calculate the concentration of solutions using units such as molarity, molality, and percent composition.
• Solubility: Studying factors that affect the solubility of substances, including temperature, pressure, and the nature of the solute and solvent.
• Colligative Properties: Exploring properties that depend on the number of solute particles in a solution, such as boiling point elevation and freezing point depression.

Benefits of Studying Solutions:

• Understanding Mixtures: Provides insights into how different substances interact and form homogeneous mixtures, which is fundamental for various chemical processes.
• Practical Applications: Helps in preparing solutions with precise concentrations for experiments, industrial processes, and pharmaceutical applications.
• Analytical Skills: Enhances the ability to analyze and interpret data related to concentration, solubility, and solution behavior.

Mastering the “Solution” unit is crucial for understanding the formation, properties, and behavior of solutions in chemistry. This knowledge is fundamental for academic studies and has practical applications in chemistry, biology, medicine, and industry.

1. Molarity of pure water is

a. 1
b. 18
c. 55.5
d. 6

2. 18g glucose is dissolved in 90g of water. The relative lowering of vapor pressure is equal ti

a. 1/5
b. 5.1
c. 1/51
d. 6

3. A solution of glucose is 10% w/v. The volume in which its 1g mole is dissolved will be

a. 1 dm3
b. 1.8 dm3
c. 200 cm3
d. 900 cm3

4. An aqueous solution of ethanol in water may have vapor pressure

a. equal to that of water
b. equal to that of ethanol
c. more than that of water
d. less than that of water

5. An azeotropic mixture of two liquids boils at a lower temperature than either of them when

a. it is saturated
b. it shows positive deviation from Raoult’s law
c. it shows negative deviation from Raoult’s law
d. it is metastable

6. In azeotropic mixture showing positive deviation from Raoult’s law, the volume of the mixture is

a. slightly more than total volume of the components
b. slightly less than total volume of the components
c. equal to the total volume of the components
d. none

7. Which of the following solutions has the highest boiling point?

a. 5.85% solution of sodium chloride
b. 18% solution of glucose
c. 6% solution of urea
d. all have the same boiling point

8. Two solution of NaCl and KCl are prepared separately by dissolving same amount of solute in water. which of the following statements is true for these solutions?

a. KCl solution will have higher boiling point than NaCl solution
b. Both the solutions have different boiling points.
c. KCl and NaCl solutions possess same vapor pressure
d. KCl solution possesses lower freezing point than NaCl solution.

9 The molal boiling point constant is the ratio of the elevation in boiling point to

a. molarity
b. molality
c. mole fraction of solvent
d. mole fraction of solute

10. Colligative properties are the properties of

a. dilute solutions which behave as nearly ideal solutions
b. concentrated solutions which behave as nearly non- ideal solutions
c. both a and b
d. neither a and b