A solution is a homogeneous mixture where components cannot be distinguished.
Solutions involve uniform dispersion of a substance (e.g., sugar in water).
The term “solution” includes uniform mixing of solids, liquids, and gases.
A solution consists of a solvent and one or more solutes.
The solvent is the medium in which the solute is dissolved.
Generally, the component present in the larger amount is called the solvent.
A solution may have more than two components.
A solution with only two components is called a binary solution.
Solutions are prepared for various reasons, such as for a specific reaction or analytical purposes.
Colloids are heterogeneous mixtures of tiny particles (1-1000 nm) dispersed in a medium.
Colloidal particles are larger than solute molecules but smaller than suspension particles.
Milk is a colloid containing casein and other ingredients dispersed in an aqueous phase.
Colloids do not settle and cannot be seen with the naked eye.
Types of colloids include foam, aerosol, emulsion, gel, smoke, sol, and solid sol.
Colloids have a heterogeneous two-phase system that appears homogeneous.
Colloids exhibit Brownian motion and the Tyndall effect.
Colloidal particles can pass through filter paper but not semipermeable membranes.
Coagulation is the process of precipitation of colloidal particles.
Hydrophilic colloids have a strong attraction to water, while hydrophobic colloids do not.
Raoult’s Law states that vapor pressure of a solution is proportional to the mole fraction of the solvent.
Ideal solutionsobey Raoult’s Law and have $\Delta H = 0$ and $\Delta V = 0$.
Non-ideal solutionsdo not follow Raoult’s Law and have $\Delta H \neq 0$ and/or $\Delta V \neq 0$.
Colligative properties depend on the number of solute particles, not their chemical nature.
Examples of colligative properties include lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Osmotic pressure is the pressure applied to stop solvent flow from a dilute to a concentrated solution through a semipermeable membrane.
Osmosis is the spontaneous movement of solvent from a dilute to a concentrated solution.
Concentration units include percentage composition, molarity, molality, mole fraction, parts per million (ppm), parts per billion (ppb), and parts per trillion (ppt).
Solubility is affected by temperature and pressure, with gases being more soluble at higher pressures and solids often more soluble at higher temperatures.
