# AP Inter 2nd Year Chemistry Notes Chapter 2 Solutions

Students can go through AP Inter 2nd Year Chemistry Notes 2nd Lesson Solutions will help students in revising the entire concepts quickly.

## AP Inter 2nd Year Chemistry Notes 2nd Lesson Solutions

→ A homogeneous mixture of two (or) more components is called as solution.

→ Mole fraction : The ratiof of number of moles of the one component of the solution to the total number of moles of all the components of the solution is called mole fraction.

→ Molarity: The number of moles of solute dissolved in one litre of solution is called molarity.

→ Molality : The number of moles of solute present in one kilogram of solvent is called molality.

→ Solubility : The maximum amount Of substance that can be dissolved in a specified amount of solvent at a specified temperature is known as solubility.

→ Henry’s law : The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.

→ Raoult’s law (Volatile solute): For a solution of volatile liquids the partial vapour pressure of each component of the solution is directly proportional to its mole fraction present in solution.

→ Raoult’s law (Non-volatile solute) : The relative lowering of vapour pressure of dilute solution containing non-volatile solute is equal to the mole fraction of the solute.

→ Ideal solutions : The solutions which obey Raoult’s law over the entire range of concentration are known as ideal solutions.

→ Colligative properties : The properties of dilute solutions which depends upon the no. of solute particles of solution are called colligative properties.

→ Ebullioscopic constant : The elevation of boiling point observed in one molal solution containing non-volatile solute.

→ Cryoscopic constant : The depression in freezing point observed in one molal solution containing non-volatile solute.

→ Osmosis : The process of flowing the solvent molecules into the solution when these are separated by semi-permeable membrane.

→ Osmotic pressure : The pressure required to stop the inflow of the solvent molecules into the solution is called osmotic pressure.

→ Isotonic solutions : The solutions having same osmotic pressure at a given temperature are called isotonic solutions.

Formulae

→ Mass % $$\left(\frac{\mathrm{W}}{\mathrm{w}}\right)=\frac{\text { Mass of the component in the solution }}{\text { Total mass of the solution }}$$ × 100

→ Volume % $$\left(\frac{\mathrm{v}}{\mathrm{V}}\right)=\frac{\text { Volume of the component }}{\text { Total volume of solution }}$$ × 100

→ Parts per million $$=\frac{\text { No. of parts of the component }}{\text { Total no. of parts of all components }}$$ × 106

→ Mole fraction of a component $$=\frac{\text { No. of moles of component }}{\text { Total no. of moles of all components }}$$

→ Molarity $$(\mathrm{M})=\frac{\text { No. of moles of solute }}{\text { Volume of solution in litres }}$$

→ Molality $$(\mathrm{m})=\frac{\text { No. of moles of solute }}{\text { Mass of solvent in } \mathrm{kg}}$$

→ Dalton’s law of partial pressures Ptotal = P1 + P2

→ Raoult’s law for a dilute solution $$\frac{\mathrm{P}_0-\mathrm{P}_{\mathrm{S}}}{\mathrm{P}_0}=\frac{\mathrm{n}_{\mathrm{s}}}{\mathrm{n}_0}=\frac{\mathrm{w}}{\mathrm{m}} \times \frac{\mathrm{M}}{\mathrm{w}}$$

→ Elevation of boiling point (∆Tb) = $$\frac{\mathrm{K}_{\mathrm{b}} \times 1000 \times \mathrm{W}}{\mathrm{m} \times \mathrm{W}}$$

→ Depression in freezing point (∆Tf) = $$\frac{\mathrm{K}_{\mathrm{b}} \times 1000 \times \mathrm{W}}{\mathrm{m} \times \mathrm{W}}$$

→ Osmotic pressure (π) = CRT

→ Van’t Hoff factor $$\text { (i) }=\frac{\text { Observed colligative property }}{\text { Calculated colligative property }}$$