Temperature, pressure, nature of solute and solvent, and presence of other solutes can affect the solubility of a solute in a solvent.
Intermolecular forces: The forces of attraction and repulsion between molecules that determine their solubility in different solvents.
Solvent-solute interactions: The interactions between the solvent and solute, which affect solubility.
Temperature: The effect of temperature on solubility, with some substances becoming more soluble as temperature increases while others become less soluble.
Pressure: The effect of pressure on solubility, such as with gases, where increased pressure can increase solubility.
Polarity: The extent to which a molecule is polar or nonpolar and how this affects solubility in different solvents.
pH: The influence of the pH of the solvent on solubility.
Concentration: The relationship between the concentration of solute and the solubility of that solute in a particular solvent.
Surface area: How surface area of a solid solute influences solubility.
Particle size: How the size of a solute particle affects solubility.
Crystallization: The process of crystals forming in a supersaturated solution and how it affects solubility.
Colligative properties: The change in solvent properties due to dissolved solute molecules or ions, such as boiling point and freezing point.
Unequal electronegativity: When bonding occurs between two atoms with different electronegativity values, it can form polar or nonpolar compounds, affecting solubility.
Salting out effect: How by adding a salt to a solution can cause a precipitation of some solutes that were originally soluble.
Gibbs Energy: How Gibbs energy, a measure of energy difference between the reactants vs products, influences solubility.
Dissolution: How the process of dissolving a solute into a solvent affects solubility.
Hydration: How water molecules can surround and solvate ions, affecting their solubility.
Ion size: How the size of an ion affects its solubility in a given solvent.
Electrolyte properties: Whether a solute is an electrolyte or not can influence its solubility in a given solvent.
Nature of the solute: Different solutes behave differently in solvents based on their nature, such as organic solutes in water.
Viscosity: The thickness of the solvent as determined by the interactions between its molecules and how it affects solubility of a solute in that solvent.
Temperature: Solubility of a solute in a solvent increases with increasing temperature.
Pressure: Solubility of gases in liquids increases with increasing pressure.
Solvent polarity: Polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes.
Solute polarity: Polar solutes dissolve in polar solvents and non-polar solutes dissolve in non-polar solvents.
Particle size: The solubility of a solute increases as the particle size decreases since smaller particles have a greater surface area for the solvent to interact with.
Concentration: The extent of solubility of a solute in a solvent increases with increasing concentration of the solute until it reaches saturation.
Chemical nature of solute and solvent: Solubility of a solute in a solvent depends on the attractive forces between the solute and solvent molecules.
Co-solvency: The addition of another solvent can increase or decrease the solubility of a solute in a solvent.
pH: The solubility of some solutes (such as acids or bases) is affected by the pH of the solvent.
Presence of other solutes: The presence of other solutes in a solvent can affect the solubility of a solute in the same solvent.
Ionic strength: The solubility of electrolytes (compounds that dissociate into ions when in solution) decreases with increasing ionic strength.
Temperature dependence of solubility: Some solutes exhibit an increase in solubility with decreasing temperature (such as sodium sulfate), whereas others exhibit a decrease (such as sodium chloride).