Key Concepts in Solutions and Dispersions

A comprehensive set of vocabulary flashcards covering key terms and concepts related to solutions, dispersions, and chemical interactions.

Dispersion

A mixture where one substance (the dispersed phase) is distributed within another (the continuous phase).

Solution

A homogeneous mixture in which the solute is completely dissolved in the solvent, appearing clear and transparent.

Dispersion

A mixture where one substance (the dispersed phase) is distributed within another (the continuous phase).

Solution

A homogeneous mixture in which the solute is completely dissolved in the solvent, appearing clear and transparent.

Colloid

A heterogeneous mixture composed of small particles dispersed in a medium, which can scatter light but do not settle out.

Suspension

A heterogeneous mixture where the dispersed particles are large enough to settle under gravity over time.

Dispersed Phase

The substance being distributed in the medium (e.g., solid particles in a suspension).

Continuous Phase

The medium that surrounds the dispersed phase (e.g., water in a suspension or solution).

Tyndall Effect

The scattering of light by particles in a colloid or suspension, distinguishing colloids and solutions.

Electrolytes

Substances that dissolve in water to form ions, affecting conductivity.

Strong Electrolyte

A substance that completely dissociates into ions when dissolved in water.

Weak Electrolyte

A substance that partially dissociates into ions in solution.

Nonelectrolyte

A substance that does not dissociate into ions at all when dissolved in water.

Vapor Pressure

The pressure exerted by the vapor of a liquid in a closed system, indicating the tendency of molecules to escape from liquid to vapor.

Boiling Point

The temperature at which the vapor pressure of a liquid equals atmospheric pressure.

Colligative Properties

Properties that depend only on the number of solute particles in a solution, not their identity.

Hypertonic Solution

A solution with a higher concentration of solutes than another solution, causing cell shrinkage.

Hypotonic Solution

A solution with a lower concentration of solutes than another solution, causing cell swelling.

Isotonic Solution

A solution having the same solute concentration as another solution, causing no net water movement.

Micelles

Spherical aggregates of surfactant molecules formed in aqueous environments where hydrophobic tails face inward and hydrophilic heads face outward.

Hydrophilic

Substances that dissolve well in water and interact favorably with polar solvents.

Hydrophobic

Substances that do not dissolve well in water but are soluble in nonpolar solvents.

Solubility

The maximum amount of solute that can dissolve in a specific amount of solvent at equilibrium.

Supersaturated Solution

A solution that contains more solute than it can normally dissolve at a given temperature.

Dynamic Equilibrium

A state reached when the rate of evaporation equals the rate of condensation of a liquid.

Clausius-Clapeyron Equation

A formula describing the relationship between vapor pressure and temperature.

Gibbs Free Energy (ΔG)

A thermodynamic quantity that helps predict the spontaneity of a process, with negative values indicating spontaneity.

Enthalpy (ΔH)

The heat content of a system, which can be absorbed or released during a reaction or change.

Entropy (ΔS)

A measure of disorder or randomness in a system, which generally favors mixing.

Henry's Law

The principle that states that the solubility of a gas in a liquid is directly proportional to its partial pressure.

Osmotic Pressure

The pressure required to stop the net movement of water across a semipermeable membrane.

Density (ρ)

The mass of a substance per unit volume, affecting concentration in solutions.

Dilution

The process of reducing the concentration of a solute in a solution by adding more solvent.

Freezing Point Depression

The decrease in the freezing point of a solvent when a solute is added.

Boiling Point Elevation

The increase in the boiling point of a solvent when a solute is added.

Vapor Pressure Lowering

The reduction in vapor pressure of a solvent when a nonvolatile solute is added.

Unique Phase Behavior

The distinct physical and chemical behavior observed in different types of dispersions (solution, colloid, suspension).

Hydrophilic Head

The polar part of a surfactant molecule that interacts favorably with water.

Hydrophobic Tail

The nonpolar part of a surfactant molecule that avoids water and interacts with oils.

Emulsion

A colloidal system of two immiscible liquids where one is dispersed in the other, stabilized by emulsifiers.

Levelling Effects in Equilibria

The phenomenon where the addition of acids or bases affects the pH of solutions, impacting reactions.

Particle Size

Refers to the dimension of particles in a dispersion, which influences its properties.

Filtration

A separation technique to remove solid particles from liquids.

Centrifugation

A method to separate particles based on density through rapid spinning.

Dialysis

A separation technique that uses a semipermeable membrane to separate solutes based on size.

Hydrophobic Interactions

Forces that cause nonpolar substances to clump together in aqueous solutions, affecting solubility.

Hydrogen Bonding

Strong attractive forces between a hydrogen atom bonded to a highly electronegative atom and another electronegative atom.

Solution Concentration

A measure of the quantity of solute in a given volume of solution.

Saponification

The process of making soap by reacting fats with a strong base.

Long-Chain Hydrocarbons

Hydrophobic organic compounds that contribute to the solubility characteristics of fats and oils.

Solvation

The process of surrounding solute particles with solvent molecules to facilitate dissolution.

Complexation

Formation of complexes between solute molecules and solvent molecules that increases solubility.

Amphipathic Compounds

Molecules that possess both hydrophilic and hydrophobic regions.

Electrostatic Repulsion

The repulsion between similarly charged particles that helps maintain dispersion stability.

Suspension Stability

The property of a suspension that describes how long the dispersed particles remain evenly distributed before settling.

Critical Micelle Concentration

The concentration of surfactants in solution above which micelles form.

Brownian Motion

The random movement of particles suspended in a fluid resulting from their collision with fast-moving molecules in the fluid.

Cohesive Forces

Forces that hold molecules of the same substance together, essential for phenomena like surface tension.

Diurnal Variation

The consecutive alteration of solute concentrations and swelling behavior contingent on changes in day-night cycles.

Osmoregulation

The process by which cells and organisms regulate water and solute concentrations.

Chemical Reaction Mechanisms

Step-by-step sequences of elementary reactions by which overall chemical changes occur.

Protein Binding Capacity

The ability of solutes to bind with proteins within a solvent, impacting solubility.

Vapor-Liquid Equilibrium

The condition in which the rates of vaporization and condensation are equal at a given temperature.

Concentration Gradient

The difference in concentration of a substance between two regions, driving diffusion.

Solution Dynamics

The study of the behavior and movement of solute particles in solutions.

Viscosity Changes

Changes in resistance to flow resulting from the addition of solutes into a solvent.

Phase Separation

The division of a homogeneous mixture into two or more distinct phases.

Ionic Dissociation

The separation of ionic compounds into individual ions in solution.

Non-volatile Solute

A solute that does not readily evaporate and impacts the physical properties of a solution.