Solutions — Class 12 Maharashtra HSC Chemistry revision notes
A 8-page visual revision sheet for Solutions, written for Class 12 Maharashtra HSC Chemistry. Formulas, diagrams and the traps that cost marks, laid out to be read the night before rather than the term before. Free, and it opens inside CapCompass.
Page 1 as PDF
Solutions in one look
one phase, many components, and how much of each decides everything
- Solute + Solvent: mixed till the mixture is one phase throughout
- Solution: homogeneous, can be gas, liquid or solid
- Concentration and Solubility: how much solute, expressed several ways, and how much a solvent can hold
Types of Solutions
- solvent is usually the component present in the LARGER amount
- it sets the physical state of the solution
- solute and solvent can each be solid, liquid or gas: nine combinations exist
- this chapter focuses mainly on solid-in-liquid, with some gas-in-liquid; solvent is usually water
The Nine Types of Solutions
- Solid in Liquid: sugar in water
- Solid in Solid: alloys, brass
- Solid in Gas: iodine vapour in air
- Liquid in Liquid: ethanol in water
- Liquid in Solid: mercury amalgam in silver
- Liquid in Gas: chloroform vapour in nitrogen
- Gas in Liquid: soda, CO_2 in water
- Gas in Solid: hydrogen in palladium
- Gas in Gas: air
Page 1 of 8. The full sheet, all 8 pages, opens free in the app.
What this Solutions sheet covers
- Solute + Solvent
- Solution
- Concentration and Solubility
- Types of Solutions
- The Nine Types of Solutions
- Solid in Liquid
- Solid in Solid
- Solid in Gas
- Liquid in Liquid
- Liquid in Solid
- Liquid in Gas
- Gas in Liquid
- Gas in Solid
- Gas in Gas
- Solubility and Factors Affecting It
- Molarity vs Molality
- Molarity M
- Molality m
- pressure on solubility
- Henry's Law
- solubility of a gas is directly proportional to its pressure over the solution
- K_H: Henry's law constant, units mol L^-1 bar^-1
- Exceptions to Henry's Law
- Raoult's Law
- partial vapour pressure of each component
- total vapour pressure, Dalton's law of partial pressures
- composition of the vapour, which differs from the liquid
- Ideal vs Non-ideal Solutions
- Ideal
- Non-ideal
- Positive vs Negative Deviation
- Positive deviation
- Negative deviation
- Vapour Pressure and Volatility
- Colligative Properties
- Vapour Pressure Lowering
- Raoult's law for a nonvolatile solute
- relative lowering equals the solute mole fraction
- molar mass of solute, dilute solution
- Boiling Point Elevation
- elevation: the boiling point ==rises==
- K_b: molal elevation constant, K kg mol^-1, a solvent property
- molar mass of solute from Δ T_b
- Freezing Point Depression
- depression: the freezing point ==falls==
- K_f: molal depression constant, K kg mol^-1, a solvent property
- molar mass of solute from Δ T_f
- Osmotic Pressure and Reverse Osmosis
- dilute solution
- C in moles per litre
- molar mass of solute from π
- Isotonic, Hypertonic and Hypotonic Solutions
- Symbols
- van't Hoff Factor
- observed over calculated (no dissociation or association) value
- equivalently, normal molar mass over the observed (abnormal) one
- degree of dissociation or association from i, rearranging i=1+(n-1)α
- Special Cases: the van't Hoff Factor
- Dissociation vs Association
- Dissociation, i > 1
- Association, i < 1
- i Modifies Every Colligative Formula
- relative lowering of vapour pressure
- osmotic pressure
- Abnormal Molar Mass
- Traps that cost marks
- Tricks that save time
How CapCompass uses this sheet
These notes are not a standalone PDF. CapCompass plans Chemistry chapter by chapter against your real exam dates and free hours, and when the plan reaches Solutions the sheet opens inside the study block itself — at the page covering the sub-topic that block is on, with the timer still running. Revision arrives at the moment the plan says revise, instead of having to be gone looking for.
More Chemistry Class 12 revision notes
- Alcohols, Phenols and Ethers
- Aldehydes, Ketones and Carboxylic Acids
- Amines
- Biomolecules
- Chemical Kinetics
- Chemical Thermodynamics
- Coordination Compounds
- Electrochemistry
- Elements of Groups 16, 17 and 18
- Green Chemistry and Nanochemistry
- Halogen Derivatives
- Introduction to Polymer Chemistry
- Ionic Equilibria
- Transition and Inner Transition Elements