1
SOLUTIONS
QUICK REVISION NOTES (JEE Main/Advanced )
【CONCENTRATION TERMS】
● Mass % → (mass solute/mass solution) x 100
● ppm → (mass solute/mass solution) x 10^6
● Mole fraction (x) → n(A)/(n(A)+n(B)) → temperature independent
● Molarity (M) → mol solute / L solution → temperature dependent
● Molality (m) → mol solute / kg solvent → temperature independent
● Normality (N) → N = M x n-factor
Colligative property problems: ALWAYS use molality or mole
fraction, NOT molarity.
【SOLUBILITY — HENRY'S LAW】
→ p = K(H) x x (p = partial pressure, x = mole fraction of gas dissolved)
● - Higher K(H) → LOWER solubility
● - K(H) increases with temperature → gas solubility falls as temp rises
Applications:
1. Soda bottles - sealed under high CO2 pressure
2. Scuba diving - He used instead of N2 to avoid "bends"
3. High altitude - low pO2 → low O2 in blood → altitude sickness
- Fails for gases that REACT with solvent (NH3, HCl)
【RAOULT'S LAW & VAPOUR PRESSURE】
SOLUTIONS
QUICK REVISION NOTES (JEE Main/Advanced )
【CONCENTRATION TERMS】
● Mass % → (mass solute/mass solution) x 100
● ppm → (mass solute/mass solution) x 10^6
● Mole fraction (x) → n(A)/(n(A)+n(B)) → temperature independent
● Molarity (M) → mol solute / L solution → temperature dependent
● Molality (m) → mol solute / kg solvent → temperature independent
● Normality (N) → N = M x n-factor
Colligative property problems: ALWAYS use molality or mole
fraction, NOT molarity.
【SOLUBILITY — HENRY'S LAW】
→ p = K(H) x x (p = partial pressure, x = mole fraction of gas dissolved)
● - Higher K(H) → LOWER solubility
● - K(H) increases with temperature → gas solubility falls as temp rises
Applications:
1. Soda bottles - sealed under high CO2 pressure
2. Scuba diving - He used instead of N2 to avoid "bends"
3. High altitude - low pO2 → low O2 in blood → altitude sickness
- Fails for gases that REACT with solvent (NH3, HCl)
【RAOULT'S LAW & VAPOUR PRESSURE】
