chem112.12

Strongly polar and ionic solutes tend to dissolve in polar solvents and nonpolar solutes tend to dissolve in nonpolar solvents.

The joining together of molecules by hydrogen bonds.

A colligative property of a solution by which the solution's boiling point is higher than that of the pure solvent.

A property such as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure whose physical value depends only on the ratio of the numbers of moles of solute and solvent particles and not on their chemical identities.

The passage of small molecules and ions, but not species of a colloidal size, through a semipermeable membrane

Two monomer units joined by chemical bonds or intramolecular forces.

A colligative property of a liquid solution by which the freezing point of the solution is lower than that of the pure solvent

The energy exchanged between the system and its surroundings when one mole of a solute dissolves in a solvent to make a dilute solution.

Pressure–Solubility Law

The development in an aqueous solution of a cage of water molecules about ions or polar molecules of the solute.

The enthalpy change associated with the hydration of gaseous ions or molecules as they dissolve in water.

A solution that has a higher osmotic pressure than cellular fluids.

A solution that has a lower osmotic pressure than cellular fluids.

A hypothetical solution that would obey the vapor pressure–concentration law (Raoult's law) exactly.

Mutually insoluble. Usually used to describe liquids that are insoluble in each other.

A more or less loosely associated pair of ions in a solution.

A solution that has the same osmotic pressure as cellular fluids.

Energy released by the imaginary process in which isolated ions come together to form a crystal of an ionic compound.

Mutually soluble

The number of degrees (°C) per unit of molal concentration that a boiling point of a solution is higher than that of the pure solvent.

The number of moles of solute in 1000 g of solvent.

The number of degrees (°C) per unit of molal concentration that a freezing point of a solution is lower than that of the pure solvent.

The molal concentration.

Heat of Solution

Descriptive of a substance with a high boiling point, a low vapor pressure. and that does not evaporate.

The passage of solvent molecules, but not those of solutes, through a semipermeable membrane; the limiting case of dialysis.

A membrane that allows passage of solvent, but not solute particles.

The back pressure that would have to be applied to prevent osmosis; one of the colligative properties.

• (a) The number of grams of an element combined in 100 g of a compound.
• (b) The number of grams of a substance in 100 g of a mixture or solution.

The concentration of a gas dissolved in a liquid at any given temperature is directly proportional to the partial pressure of the gas above the solution.

Vapor Pressure–Concentration Law

The development of a cage-like network of a solution's solvent molecules about a molecule or ion of the solute.

The enthalpy of the interaction of gaseous molecules or ions of solute with solvent molecules during the formation of a solution.

The ratio of the observed freezing point depression to the value calculated on the assumption that the solute dissolves as un-ionized molecules.

The vapor pressure of one component above a mixture of molecular compounds equals the product of its vapor pressure when pure and its mole fraction.

• mol of solute
• L of solution

Changes with temperature.

• mol of solute
• kg of solvent

Does not change with temperature

(w/w) in grams

• mass of solute
• mass of solution X 100%

• moles of solute
• moles of solute + moles of solvent

unitless