Solutions | कक्षा 12 रसायन विज्ञान | RBSE Chapter 2 |

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विलयन (Solutions) की संपूर्ण जानकारी। यह video Class 12 Chemistry के Chapter 2 का complete explanation है।
📚 Topics Covered:
✓ Types of Solutions और Concentration Terms
✓ Solubility और Henry's Law
✓ Raoult's Law और Ideal Solutions
✓ Colligative Properties (वैधुत गुण)
✓ Relative Lowering of Vapour Pressure
✓ Elevation in Boiling Point
✓ Depression in Freezing Point
✓ Osmotic Pressure
✓ Van't Hoff Factor (i)
✓ Abnormal Molar Mass
✓ सभी important formulas और derivations
✓ Numerical problems solving tricks
🎯 Perfect For:

RBSE Board Class 12 Students
CBSE Board Exam Preparation
JEE Main Chemistry
NEET Chemistry
Board Exams 2025-26

📖 Chapter Content:
इस chapter में हम सीखेंगे कि solutions कितने types के होते हैं, colligative properties क्या हैं और molecular mass कैसे calculate करते हैं। सभी concepts को simple Hindi और English में समझाया गया है।
⚡ Key Formulas:

Molarity (M) = moles/volume(L)
Molality (m) = moles/mass of solvent(kg)
Mole fraction: X = n/(n₁ + n₂)
Henry's Law: P = KH × X
Raoult's Law: P = P° × X
ΔTb = Kb × m
ΔTf = Kf × m
π = CRT (Osmotic Pressure)
Van't Hoff: i = (observed property)/(calculated property)

🔥 Why This Video:

Clear explanations in Hindi-English mix
Board exam focused content
All formulas properly explained
Previous year questions discussion
Quick revision notes
Numerical solving techniques
Difficult concepts simplified

📝 Important Topics:

Solution components (solute और solvent)
Types: solid in liquid, liquid in liquid, gas in liquid
Concentration terms comparison
Molarity, molality, normality, mole fraction
Mass percentage, volume percentage, ppm
Henry's law applications
Ideal और non-ideal solutions
Positive और negative deviation
Azeotropes

💡 Special Focus:

Colligative properties की definition
Why called colligative (number of particles पर depend)
Relative lowering of vapour pressure
Boiling point elevation constant (Kb)
Freezing point depression constant (Kf)
Osmosis और osmotic pressure
Isotonic, hypertonic, hypotonic solutions
Reverse osmosis
Van't Hoff factor की calculation
Association और dissociation

🧪 Colligative Properties Detail:
1. Relative Lowering of Vapour Pressure:

Formula: (P° - P)/P° = X₂ = n₂/(n₁ + n₂)
For dilute solutions approximately equal to n₂/n₁

2. Elevation in Boiling Point:

ΔTb = Kb × m
Kb = molal elevation constant
M = (Kb × w₂ × 1000)/(ΔTb × w₁)

3. Depression in Freezing Point:

ΔTf = Kf × m
Kf = molal depression constant
M = (Kf × w₂ × 1000)/(ΔTf × w₁)

4. Osmotic Pressure:

π = CRT = (n/V)RT
M = (w₂RT)/(πV)
Most accurate method

📐 Calculations Covered:

Molarity to molality conversion
Mole fraction calculation
Molecular mass from colligative properties
Van't Hoff factor determination
Degree of dissociation/association
Osmotic pressure problems
Boiling point and freezing point calculations

🔬 Van't Hoff Factor:

For non-electrolytes: i = 1
For dissociation: i greater than 1 (NaCl: i = 2, CaCl₂: i = 3)
For association: i less than 1 (benzoic acid in benzene)
Modified formulas: ΔTb = i × Kb × m
π = i × CRT

💧 Important Concepts:

Ideal solution (ΔHmix = 0, ΔVmix = 0)
Non-ideal solution deviations
Azeotropes (minimum और maximum boiling)
Hypertonic solution (higher concentration)
Hypotonic solution (lower concentration)
Isotonic solution (equal concentration)
Plasmolysis और hemolysis

📊 Concentration Terms Comparison:

Molarity: Temperature dependent
Molality: Temperature independent
Normality: Equivalent concept
Mole fraction: Dimensionless
ppm: Parts per million (very dilute)

🌡️ Real Life Applications:

Antifreeze in radiators
Salt on roads in winter
Preservation of food
Reverse osmosis (water purification)
IV drips (isotonic solutions)
Desalination of sea water

👨‍🏫 By: Science 2.0
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