Chem II Ch. 13: Physical Properties of Solutions

Physical Properties of Solutions

Colloid

a uniform dispersion of one substance in another substance

Solvent

a substance in a solution that is present in the largest amount

Solute

the dissolved substance in a solution

Foam

a colloid that consists of a gas dispersed in either a liquid or a solid

Law

A concise verbal or mathematical statement of reliable relationship between phenomena.

Saturated solution

A solution that contains the maximum amount of a solute that will dissolve in a solvent at a specific temperature

Unsaturated solution

a solution that contains less solute than it has the capacity to dissolve

Supersaturated solution

a solution that contains more dissolve solute than is present in a saturated solution

Solvation

process by which solute particles become surrounded by solvent molecules

Entropy

a thermodynamic state function that describes how dispersed a system’s energy is

Intermolecular Forces

• Dispersion forces

• Dipole-dipole forces

• Hydrogen bonding

• Ion-ion forces

• Ion-dipole

• Dipole-induced dipole

• Ion-induced dipole

Dispersion forces

present in all substances

Dipole-dipole forces

present in polar substances

Hydrogen bonding forces

especially strong dipole-dipole forces exhibited by molecules with O—H, N—H, F—H bonds

Ion-ion forces

present in ionic substances

Ion-dipole forces

the charge of an ion is attracted to the partial charge on a polar molecule

Dipole-induced dipole forces

the partial charge on a polar molecule induces a temporary partial charge on a neighboring nonpolar molecule or atom

Ion-induced dipole forces

the charge of an ion induces a temporary partial charge on a neighboring nonpolar molecule or atom

Intermolecular forces (strongest to weakest)

Ion-ion forces > Ion-dipole forces > Hydrogen bonding > Dipole-dipole interactions > London dispersion forces

Miscible

mutually soluble in any proportions

Molarity (M)

the number of moles of solute divided by the number of liters of solution

Mole fraction (X)

defined as the number of moles of solute divided by the total number of moles

Molality (m)

the number of moles of solute dissolved in 1 kg (1000 g) of solvent

Henry’s law

the solubility of a gas in a liquid is proportional the pressure of the gas over the solution