Lecture 2: Solutions And Their Behavior

A homogeneous mixture that consists of one or more solutes uniformly dispersed throughout a medium known as the solvent

Present in the larger amount

Present in the smaller amount than the solvent

Moles solute/kg solvent

Moles solute/L solution (more applicable to us)

Equal to molarity

Solubility is the amount of solute that will dissolve in a given amount of solvent

A saturated solution contains the maximum amount of a solute, as defined by its solubility

• this is NOT a stable system - A solution contains more solute than allowed by the solubility

Two liquids are miscible if they are soluble in each other in all proportions (I.e.: alcohol is miscible in water; oil is not miscible in water)

Energy flows into the system

Energy flows out of the system

Transfer of energy into or out of a system caused by a difference in temperature

As pressure increases for gaseous solutes, solubility increases

A negligible effect

Decreases Example: think about opening a warm can of soda pop—the carbon dioxide is less soluble and comes bubbling out

Increases

Inverse relationship—the colder the liquid (i.e.: blood), the more gas that will dissolve in the liquid

Depends only on the number of solute particles, not the identity of the solute particles

• The vapor pressure of a solution decreases with increasing solute concentration • The boiling point of a solution increases with increasing solute concentration • The freezing point of a solution decreases with increasing solute concentration • The osmotic pressure of a solution increases with increasing solute concentration

Decreases

Increases

Decreases

Increases