SOLUBILITY EQUILIBRIA | 4.3

Solution

homogenous mixture of 2 or more substances

Solute

substance(s) present in

the smaller amount(s)

Solvent

substance present in the

larger amount

Solution Process

molecular view of the formation of solution

Stirring (Agitation)

Surface Area

Temperature

Factors Affecting Rate of Dissolution

Solubility

Maximum amount of solute that can be dissolved in a given

amount of solvent at a specified temperature

Molar solubility (s)

- the number of moles of

solute dissolved in 1 L of

a saturated solution.

- moles solute/L of solution

- Unit: M

saturated solution

Dissolved solute = solubility

unsaturated solution

Dissolved solute < solubility

supersaturated solution

Dissolved solute > solubility

Nature of Solute and

Solvent

Pressure

Temperature

Factors Affecting Solubility

↑temperature, ↓ solubility

relationship of temperature and solubility and gas phase

Saturated Solutions

any undissolved solids are in

equilibrium with the saturated

solution (liquid)

undissolved solute and saturated solution

equilibrium exists between an

**** and its *****

Unsaturated solution No precipitate

Q < Ksp

Saturated solution

Q = Ksp

Saturated solution, Supersaturated solution, Precipitate will form

Q > Ksp

rules to remember in dissolution equations

COMPLEX IONS

ions that contains a

central metal cation

bonded to one or more

molecules or ions

- usually participated in

by transition metal

cations (have more

than one oxidation

state)