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 P_total = 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 (∆T_b) = \(\frac{\mathrm{K}_{\mathrm{b}} \times 1000 \times \mathrm{W}}{\mathrm{m} \times \mathrm{W}}\)

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

→ Osmotic pressure (π) = CRT

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