Covers the classification of dispersions by particle size, placing true solutions, colloidal solutions, coarse dispersions and suspensions in order, followed by the mechanism of dissolution in stages and the factors that govern solubility. It then addresses temperature dependence of solubility with examples, strong versus weak electrolytes, and Ostwald's dilution law. Closing sections introduce Henry's law for gases, the van't Hoff relation, and colligative properties.
Topic 6 of 42 in the MU Sofia syllabus for Chemistry (Dental Medicine, Year 1). The free AceMed note covers it in 12 sections, about 840 words (6 min of reading), with 20 flashcards.
In this note
Types of Dispersion
Mechanism of Dissolution
Solubility and Concentration of Solutions:
Temperature dependence of solubility
Solutions of electrolytes ( weak vs strong electrolyte )
Degree of electrolyte dissociation
Ostwald's dissolution law
High-Yield Additions for Solutions & Dispersions
Solubility of Gases in Liquids (Henry’s Law)
Relation Between Solubility & Temperature (Van’t Hoff Equation)
Degree of Dissociation (α) and Ostwald’s Dilution Law
Colligative Properties
Types of Dispersion
A Solution:
Homogeneous dispersion where solute particles are uniformly distributed in a solvent.
Particle size < 1 nm.
Suspension:
Heterogeneous dispersion where solid particles are dispersed in a liquid medium.
Particle size: 100 nm.
Some common examples of suspensions are as follow:
Oil and water
Muddy water
Dust in air
Colloid:
Microheterogeneous dispersion.
Particle size: 1 nm - 100 nm.
Coarse Dispersions:
Particle size > 100 nm.
Includes suspensions, emulsions, and foams.
Prone to precipitation or floating due to significant particle size.
Colloidal Solutions:
Particle size: 1 nm - 100 nm.
Susceptible to precipitation or surface emergence upon prolonged residence or under external factors.
True Solutions:
Particle size < 1 nm.
Stable systems where the dispersed phase is broken down into ions or molecules.
Also known as molecular or ionic solutions.
Molecular and ionic solutions
Disperse medium in liquid solutions is the solvent, while the disperse phase is the solute.
Molecular solutions: Solute particles are individual molecules; no bonds are broken.
Ionic solutions: Solute particles are ions; bonds are broken upon dissolution.(Dissolution) is a spontaneous process favoured by energetics.
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