Description

Solution Notes

Prepare for class 11 and neet

Include all laws with pictures to understand

Definition and formulas of mass %, molarity, Molality,  mole fraction, solubility,  le chatteliers principle, Raoult’s law, Henry’s law, Dalton’s law, colligative properties, osmosis,  reverse osmosis

Formulas: Volume of solution = mass / density

2.: 𝑝=𝑘H𝑥

3.𝑝𝐴=𝑥𝐴𝑝∘A

Where:

pA = partial vapour pressure of A in solution

𝑥𝐴 = mole fraction of A

𝑝∘A = vapour pressure of pure A

By Relative Lowering of Vapour Pressure

Δ𝑝/𝑝∘=𝑛2/𝑛1. Or p°-p/p=xsolute congruent to ns/solvent

Where:

𝑛2​ = moles of solute

𝑛1 = moles of solvent

📌 Used mainly for non-volatile solutes

2. By Elevation of Boiling Point

Δ𝑇𝑏=𝐾𝑏𝑚

𝑚=𝑤2×1000/𝑀2×𝑤1

Where:

𝐾b = molal elevation constant

M2 = molar mass of solute

Substitute m in ΔTb​ = Kb×𝑤2×1000/𝑀2×𝑤1 Molar mass of solute M2 =Kb×𝑤2×1000/ΔTb​×𝑤1

📌 Suitable for non-volatile solutes

3. By Depression of Freezing Point

Δ𝑇𝑓=𝐾𝑓𝑚

𝑚=𝑤2×1000/𝑀2×𝑤1

📌 Most commonly used method in labs

4. By Osmotic Pressure

𝜋=𝐶𝑅𝑇

𝑀=𝑤𝑅𝑇/𝜋𝑉

Heptane and octane form an ideal solution. At 373 K, the vapour pressures of

the two liquid components are 105.2 kPa and 46.8 kPa respectively. What will

be the vapour pressure of a mixture of 26.0 g of heptane and 35 g of octane?

Problems