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saturated solution
This is a solution that contains the maximum amount of solute that can dissolve at a given temperature and pressure.
If you try to add more solute, it won’t dissolve and will instead settle at the bottom.
Example: If you keep adding sugar to iced tea and stirring, eventually, some sugar will remain undissolved at the bottom—meaning the tea is saturated with sugar.
supersaturated solution
This solution contains more solute than what would normally dissolve at a certain temperature and pressure.
It’s usually made by heating a saturated solution, adding more solute, and then cooling it slowly. The excess solute remains dissolved temporarily.
This type of solution are unstable, and any disturbance (like stirring or adding a small crystal of solute) can cause the extra solute to crystallize out.
Example: Making rock candy by boiling sugar water and letting it cool slowly—eventually, sugar crystals form because the solution was supersaturated.
Unsaturated Solution:
This is a solution that contains less solute than the maximum amount that can dissolve at a given temperature and pressure.
More solute can still be added and dissolved in the solution.
Example: Adding a spoonful of sugar to hot coffee and stirring until it all dissolves—it's still unsaturated because more sugar can be added and dissolved.
solubility
The maximum amount of a substance (solute) that can dissolve in a given amount of solvent at a specific temperature and pressure.
It’s usually expressed in grams of solute per 100 grams of solvent (g/100g) or in molarity (M).
can be affected by Temperature, pressure (for gases), and the nature of the solute and solvent (like “like dissolves like”—polar solvents dissolve polar solutes, etc.).
Example: The solubility of salt (NaCl) in water at 25°C is about 36g per 100g of water.
strong electrolytes
completely dissociate into ions when dissolved in water.
They produce a lot of ions, making them excellent conductors of electricity.
Examples:
Strong Acids: Hydrochloric acid (HCl), Sulfuric acid (H₂SO₄).
Strong Bases: Sodium hydroxide (NaOH), Potassium hydroxide (KOH).
Salts: Sodium chloride (NaCl), Potassium nitrate (KNO₃).
electrolytes
are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity.
Common examples include salts, acids, and bases.
weak electrolytes
only partially dissociate into ions when dissolved in water.
They produce fewer ions, so they’re poor conductors of electricity.
Examples:
Weak Acids: Acetic acid (CH₃COOH, found in vinegar).
Weak Bases: Ammonia (NH₃)
nonelectrolytes
are substances that do not dissociate into ions at all when dissolved in water.
Their solutions cannot conduct electricity.
Examples:
Sugars: Glucose (C₆H₁₂O₆).
Alcohols: Ethanol (C₂H₅OH).
dissociation (for ionic compounds)
This term is used when ionic compounds (like salts) dissolve in water.
The solid ionic compound breaks apart into its positive and negative ions.
Example: NaCl (s) → Na⁺ (aq) + Cl⁻ (aq).
Ionization (Acids & Bases)
This term is used when acids or bases dissolve in water.
Molecules (covalent compounds) react with water and form ions.
Example (Acid): HCl (aq) → H⁺ (aq) + Cl⁻ (aq).
Example (Base): NH₃ (aq) + H₂O (l) ⇌ NH₄⁺ (aq) + OH⁻ (aq) (Note: This one is a weak base, so it only partially ionizes).
