Solution Formation and Solubility Concepts

A process where the enthalpy change is positive (heat is absorbed) but can still occur if the entropy change is large and positive, favoring the formation of a solution.

The force that drives the movement of solvent across a semipermeable membrane from a region of high solvent/low solute concentration to a region of low solvent/high solute concentration.

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

A solution where more solute can be dissolved at a given temperature.

A property that depends solely on the number of solute particles in a solution, not their identity. Examples include freezing point depression, boiling point elevation, vapor pressure lowering, and osmotic pressure.

A solution containing more solute than can normally dissolve at that temperature. It is unstable and prone to crystallization.

The minimum temperature at which a liquid changes into its gaseous state under a constant pressure, specifically the vapor pressure of the liquid.

The tendency of a liquid to evaporate. It is the pressure exerted by the vapor above a liquid at a given temperature.

The temperature at which a liquid transitions into a solid.

The spontaneous movement of solvent molecules across a semipermeable membrane from a region of high solvent concentration to a region of low solvent concentration.

A homogeneous mixture where one substance (the solute) is evenly distributed within another substance (the solvent).

The relative amount of solute present in a solution. It can be expressed in various units like molarity, molality, percent by mass, etc.

Interactions between molecules of the same substance, like water molecules attracting each other.

Interactions between molecules of the solute and solvent. These forces determine the solubility of a substance.

The amount of a solute that can dissolve in a given amount of solvent at a specific temperature.

A force of attraction between molecules due to temporary fluctuations in electron distribution, present in all substances.

A force of attraction between polar molecules caused by the alignment of their permanent dipoles.

A special type of dipole-dipole interaction where a hydrogen atom is bonded to a highly electronegative atom (like oxygen or nitrogen).

A force of attraction between an ion and a polar molecule.

A type of interaction that occurs between ions in an ionic compound.

The breaking of interactions between solute molecules. This process usually requires energy.

The breaking of interactions between solvent molecules. This also usually requires energy.

The formation of interactions between solute and solvent molecules. This process usually releases energy.

A change in the degree of disorder or randomness of a system. An increase in entropy generally favors solution formation.

The change in heat content during a chemical reaction or physical process. A negative enthalpy change indicates an exothermic process (releases heat) which generally favors solution formation.

A principle that states that substances with similar polarities dissolve best in each other. 'Like dissolves like.'

The state of balance in a reversible process where the rate of the forward reaction equals the rate of the reverse reaction. In solution formation, it refers to the balance between dissolution and crystallization.

A measure of the tendency of a solid to dissolve in water. A higher Ksp value indicates greater solubility.

The addition of a common ion to a saturated solution, which reduces the solubility of the original salt due to Le Chatelier's principle.

A particle with a positive or negative charge, formed when an atom gains or loses electrons.

A substance that forms ions when dissolved in water, allowing it to conduct electricity.

A substance that does not produce ions when dissolved in water, and therefore does not conduct electricity.

A substance that forms ions in solution but to a lesser extent than a strong electrolyte.

A substance that completely dissociates into ions when dissolved in water, making it a strong conductor of electricity.

The factor that represents the number of particles a solute dissociates into when dissolved in a solvent. It is used to determine the precise effect of the solute on colligative properties.

A homogeneous mixture with tiny particles that are dispersed but not dissolved. They are larger than solution particles but smaller than suspension particles. They scatter light, giving them a cloudy appearance.

The scattering of light by colloid particles, making them appear cloudy or opaque. This is a distinguishing characteristic of colloids.

A type of colloid where the dispersed particles have an affinity for water and form a hydration shell around them. These colloids are relatively stable in water.

A type of colloid where the dispersed particles repel water and tend to aggregate, requiring stabilization to prevent them from clumping together.

A substance that can stabilize a colloid by reducing surface tension and preventing the aggregation of hydrophobic particles, forming micelles around them.

A type of colloid where liquid droplets are dispersed in another liquid. They are often stabilized by emulsifiers.

The process of breaking down large droplets of oil into smaller droplets, which are then surrounded by emulsifiers to prevent them from coalescing. This helps to stabilize the emulsion.