Chemistry Chapter: Liquid Solutions

A homogeneous mixture of two or more components with uniform composition and properties throughout. The component present in the largest quantity is usually the solvent, determining the physical state of the solution. Other components are called solutes.

Solutions containing two components, such as a solute dissolved in a solvent.

The quantitative expression of the amount of solute present in a given amount of solvent or solution.

The mass of a component in a solution, divided by the total mass of the solution, multiplied by 100%.

The volume of a component in a solution, divided by the total volume of the solution, multiplied by 100%.

The mass of solute dissolved in 100 mL of solution. Often used in medicine and pharmacy.

A unit used for expressing concentrations of trace amounts of solutes, defined as the number of parts of a component per million parts of the total solution.

The ratio of the number of moles of a component to the total number of moles of all components in a solution.

The number of moles of solute dissolved in one litre of solution.

The number of moles of solute dissolved per kilogram of solvent.

The maximum amount of a substance that can dissolve in a specified amount of solvent at a given temperature.

The tendency of polar solutes to dissolve in polar solvents, and non-polar solutes to dissolve in non-polar solvents.

The process where solute dissolves in a solvent, increasing the concentration of the solute in the solution.

The process where some solute particles in a solution collide with solid solute particles and separate out of the solution.

A solution in which no more solute can dissolve at the same temperature and pressure.

A solution in which more solute can dissolve at the same temperature and pressure.

A solution in dynamic equilibrium with undissolved solute, containing the maximum amount of solute dissolved in a given amount of solvent. The concentration of solute in this solution is its solubility.

The solubility of solids in liquids generally increases with temperature if the dissolution process is endothermic (absorbs heat) and decreases if it is exothermic (releases heat).

Pressure has a negligible effect on the solubility of solids in liquids, as solids and liquids are highly incompressible.

The solubility of gases in liquids increases with increasing pressure.

At a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the surface of the liquid or solution.

The ratio of the partial pressure of a gas in the vapour phase to its mole fraction in the solution, describing the solubility of a gas in a liquid.

The partial vapour pressure of each component of a solution of volatile liquids is directly proportional to its mole fraction present in the solution.

The vapour pressure of the pure component at the same temperature. It is used in the Raoult's Law equation.

A solution that obeys Raoult's Law over the entire range of concentration.

A solution that does not obey Raoult's Law over the entire range of concentration.

A non-ideal solution where the vapour pressure of the solution is higher than that predicted by Raoult's Law. The A-B interactions are weaker than A-A or B-B interactions.

A non-ideal solution where the vapour pressure of the solution is lower than that predicted by Raoult's Law. The A-B interactions are stronger than A-A or B-B interactions.

A binary mixture of liquids that has the same composition in the liquid and vapour phases at a constant boiling point. They cannot be separated by fractional distillation.

Azeotropes that boil at a temperature lower than that of either pure component. They show large positive deviations from Raoult's Law.

Azeotropes that boil at a temperature higher than that of either pure component. They show large negative deviations from Raoult's Law.

Properties of solutions that depend only on the number of solute particles present and not on their nature or identity.

The decrease in the vapour pressure of a solvent when a non-volatile solute is added to it.

The increase in the boiling point of a solvent when a non-volatile solute is added to it.

The decrease in the freezing point of a solvent when a non-volatile solute is added to it.

The pressure that needs to be applied to a solution to stop the flow of solvent across a semipermeable membrane from a pure solvent to the solution.