Chemistry 11

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9.1.0 CONCENTRATION UNITS OF SOLUTIONS 9.1.1 Percentage composition 9.1.1.1 (a ) Percentage weight / weight 9.1.1.2 (b ) Percentage Weight/Volume 9.1.1.3 (c) Percentage Volume /Weight 9.1.1.4 (d) Percentage Volume / Volume 9.1.2 Molarity ( M )9.1.3 Molality( m )9.1.4 Mole Fraction (x)9.1.5 Parts Per Million ( ppm)9.1.6 Interconversion of Various Concentration Units of Solutions

9.2 TYPES OF SOLUTIONS 9.2.1 Solutions of Solids in Liquids 9.2.2 Solutions of Liquids in Liquids 9.2.2.1 (i) completely Miscible Liquids 9.2.2.2 (ii) Partially Miscible Liquids 9.2.2.2.1Phenol-Water System (H₂O + C₆H₅OH )9.2.2.3 (iii) Liquids Practically Immscible

9.3.1 RAOULTS LAW 9.3.2 Raoults Law (when both components are volatile)

9.4 VAPOUR PRESSURES OF LIQUID-LIQUID SOLUTIONS 9.4.1 i. Ideal Solutions 9.4.1.1 Fractional Distillation of Ideal Mixture of Two Liquids 9.4.2 ii. Non-Ideal Solutions (azeotropic mixtures)9.4.2.1 (a) Positive Deviations 9.4.2.2 (b) Negative Deviations

9.5 SOLUBILITY AND SOLUBILITY CURVES 9.5.1 Solubility Curves 9.5.2 Fractional Crystallisation

9.6 COLLIGATIVE PROPERTIES OF SOLUTIONS 9.6.1 Why Some of the Properties are Called Colligative 9.6.2 Lowering of Vapour Pressure 9.6.3 Elevation of Boiling Point 9.6.4 Measurement of Boiling Point Elevation: Landsbergers Method 9.6.5 Depression of the Freezing Point of a Solvent by a Solute 9.6.6 Measurement of Freezing Point Depression Beckmann s Freezing Point Apparatus 9.6.7 Applications of Boiling Point Elevation and Freezing Point Depression Phenomena

9.7.0 ENERGETICS OF SOLUTION 9.7.1 Hydration Energy of Ions

9.8 HYDRATION AND HYDROLYSIS 9.8.1 Hydration 9.8.2 Hydrates 9.8.3 Hydrolysis