Chem Ch 12

homogeneous mixture

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

contains less solute than it has the capacity to dissolve

contains more solute than is present in a saturated solution, can be formed by careful cooling, solute will separate if solution is disturbed (crystalization)

• the measure of how much solute will dissolve in a solvent at a specific temperature
• "like dissolves like" - 2 substances with intermolecular forces of similar type and magnitude are likely to be soluble in each other
• (non-polar will be soluble with non-polar) hydrocarbons are always non-polar
• (polar w polar)

if substances are completely soluble in each other in all proportions

the amount of solute present in a given amount of solution

M = mol solute/ L solution

mass of solute/mass of solution * 100%

• mol of single component/moles of all components
• Xa has no units

m = moles of solute/mass of solvent (kg)

the process in which an ion or molecule is surrounded by solvent molecules arranged in a specific manner

the separation of a mixture of substances into pure components on the basis of their differing solubilities

usually solubility increases but there are exceptions, it is best determined experimentally

• solubility usually decreases with increasing temperature
• warm water is bad for fishes because the solubility of oxygen decreases

• the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution
• c =kP
• if more than 1 gas present P = partial pressure
• c = molar concentration

• doesn't change with liquids or solids
• external pressure GREATLY INCREASES the solubility of gas

• (or collective properties) - properties that depend only on the # of solute particles in solution and not on the nature of the solute particles
• 1. vapor-pressure lowering
• 2. boiling-point elevation
• 3. freezing-point depression
• 4. osmotic pressure (raising)

• electrolytes break apart into ions when they dissolve
• nonelectrolytes do not break apart (molecular compounds or covalent compounds that aren't acids and bases)

• i - actual # of particles in soln after dissociation/# of formula units initially dissolved in solution
• used to convert from concentration of solute to particles
• nonelectrolytes i = 1

one or more cations and one or more anions held together by electrostatic forces

• does not have a measurable vapor pressure
• the vapor pressure of a nonvolatile solution is always less then that of the pure solvent

• P1 = X1 P1*
• X is mole fraction of the solvent not solute
• P1 is vapor pressure of solution
• P1* is vapor pressure of pure solvent
• DONT USE i

• has measurable vapor pressure
• do Raoult's law to each substance with measureable vapor pressure
• total pressure is sum of partial pressures

• the temperature at which the vapor pressure equals the external atmospheric pressure
• ^ Tb = Kb im
• im = concentration of particles in molality
• ^ Tb = Tb - Tb*

• adding solute lowers it
• freezing point depression
• ^Tf = Tf* - Tf
• ^Tf = Kf im

• the pressure required to stop osmosis (the selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one)
• (cap pie) = iMRT
• M is molarity of particles

any solution that obey's Raoult's law

a procedure for separating liquid components of a solution based on their different boiling points

two solutions of equal concentration, therefore equal osmotic pressure

unequal concentrations - this is the more dilute solution

unequal concentrations - this is the more concentrated solution

• a dispersion of particles of one substance throughout a dispersing medium made of another substance (not really a solution) does not break apart over time
• hydrophilic - water loving - proteins
• hydrophobic - water fearing - oil droplets