Chemistry Solution With All Terms And Memory Game

💡 Solution Chemistry: Complete Guide with Advanced Topics & Memory Game

🔍 What is a Solution?

A solution is a homogeneous mixture composed of two or more substances. The substance present in the larger amount is usually the solvent, and the one in lesser amount is the solute.

• Solvent: The component that dissolves the solute (e.g., water).
• Solute: The component that gets dissolved (e.g., salt).

🧪 Henry’s Law

Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid at constant temperature.

Mathematical Expression: C = kP, where:

• C is the concentration of gas in the liquid.
• P is the partial pressure of the gas.
• k is the Henry’s law constant.

Applications: Carbonated beverages, deep-sea diving, and anesthesia.

🧪 Types of Solutions

Depending on the physical states of solute and solvent, solutions can be:

• Solid in liquid (e.g., sugar in water)
• Gas in liquid (e.g., CO₂ in soda)
• Liquid in gas (e.g., water vapor in air)

🔬 Non-Ideal Solutions

Non-ideal solutions deviate from Raoult’s Law due to differing interactions between solute and solvent molecules.

✅ Positive Deviation

• Weaker solute-solvent interactions
• Increased vapor pressure
• Example: Ethanol and Acetone

✅ Negative Deviation

• Stronger solute-solvent interactions
• Decreased vapor pressure
• Example: Acetone and Chloroform

♻️ Azeotropes

An azeotrope is a mixture of two or more liquids that boils at a constant temperature and composition.

• Minimum Boiling Azeotrope: Ethanol + Water
• Maximum Boiling Azeotrope: Hydrochloric acid + Water

They cannot be separated by simple distillation.

📏 Colligative Properties

• Relative Lowering of Vapor Pressure
• Boiling Point Elevation
• Freezing Point Depression
• Osmotic Pressure

These depend on the number of solute particles, not their identity.

🧮 van’t Hoff Factor (i)

Formula: i =

observed value⁄calculated value

It adjusts for dissociation/association of solutes. For example, NaCl dissociates into Na⁺ and Cl⁻, so i ≈ 2.

Graphical view of Positive and negative Deviation

Positive & Negative Deviations

Graphical view of Depression in Freezing Point

Depression in Freezing Point

Graphical view of Elevation in Boiling Point

Elevation in Boiling Point

🎮 Memory Puzzle Game

Match the concepts and their terms by clicking below:

🎮 Play Colligative Properties Memory Game

✅ Conclusion | निष्कर्ष

This article includes basic to advanced level content from solubility concepts to memory games.

📌 Bookmark this article to revise before exams and Olympiads!

Colligative Properties IIT - JEE level Problems

Question 1

A solution contains 5.85 g of NaCl in 100 g of water. Calculate the depression in freezing point. (K_f = 1.86 K kg/mol)

Answer: ΔT_f = 3.72 K (Using van't Hoff factor i = 2)

Question 2

A 0.1 molal solution of urea (non-electrolyte) causes a depression in freezing point of 0.186 K. What is the molal depression constant of the solvent?

Answer: K_f = ΔT_f/m = 0.186 / 0.1 = 1.86 K kg/mol

Question 3

Which of the following 0.01 molal aqueous solution will have the lowest freezing point?
A. NaCl
B. Glucose
C. BaCl₂
D. Urea

Answer: C. BaCl₂ (i = 3, highest van't Hoff factor)

Question 4

Calculate the osmotic pressure of a 0.1 M solution of glucose at 27°C. (R = 0.0821 L atm/mol K)

Answer: π = nRT/V = 0.1 × 0.0821 × 300 = 2.46 atm

Question 5

A solution containing 1 g of solute in 100 g of water gave a boiling point elevation of 0.52°C. If K_b = 0.52 K kg/mol, find the molar mass of the solute.

Answer: M = (1000 × 1 × 0.52) / (100 × 0.52) = 100 g/mol

Question 6

1.8 g of glucose (C₆H₁₂O₆) is dissolved in 100 g of water. Calculate the depression in freezing point. (K_f = 1.86 K kg/mol)

Answer: ΔT_f = 0.186 K

Question 7

Which of the following shows the highest boiling point elevation?
A. 0.1 M NaCl
B. 0.1 M BaCl₂
C. 0.1 M Glucose
D. 0.1 M AlCl₃

Answer: D. AlCl₃ (i = 4, highest number of particles)

Question 8

A 1 molal solution of a non-volatile solute has a freezing point depression of 1.86°C. What will be the freezing point of this solution?

Answer: 0 - 1.86 = -1.86°C

Question 9

Osmotic pressure of a solution at 300 K is 2.46 atm. Find the concentration of solute (R = 0.0821 L atm/mol K).

Answer: C = π / RT = 2.46 / (0.0821 × 300) = 0.1 M

Question 10

Which property is used to determine molar mass of a solute in dilute solution?
A. Surface tension
B. Colligative property
C. Viscosity
D. Refractive index

Answer: B. Colligative property

Question 11

3 g of a non-volatile solute dissolved in 100 g water produces a boiling point elevation of 0.3°C. Molar mass of solute is 60. What is K_b?

Answer: K_b = ΔT_b × M × 1000 / (W × m) = 0.3 × 60 × 1000 / (3 × 100) = 6 K kg/mol

Question 12

Identify the colligative property which is not affected by ionization:
A. Relative lowering of vapor pressure
B. Boiling point elevation
C. Freezing point depression
D. None of these

Answer: D. None of these (all are affected by van’t Hoff factor)

Question 13

A 0.1 M solution of MgSO₄ behaves as 0.15 M in osmotic pressure calculation. What is the van’t Hoff factor?

Answer: i = 0.15 / 0.1 = 1.5

Question 14

Freezing point of a solution of 10 g urea in 180 g of water is?
(K_f = 1.86 K kg/mol, Molar mass of urea = 60 g/mol)

Answer: ΔT_f = 1.86 × (10/60) / (0.18) ≈ 1.72 K; T_f = -1.72°C

Question 15

Which factor decides magnitude of colligative properties?
A. Nature of solute
B. Number of solute particles
C. Volume of solvent
D. Temperature

Answer: B. Number of solute particles

🔗 Related Links

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