the amount of subsstance that will dissolve ina given amount of solvent
entropy
the measure of the energy randomization or energy dispersal in a system
miscible
if solute-solvent interaction are comparabl or stronger than solute-solute interactions and solvent-solvent interactions
enthalpy of hydration
the enthalpy change that occurs when one mole of gaseous solute ions are dissoved in water
it is always negative for ionic compounds because the ion dipole interacions that occur btw a dissolved ion and the surrounding water olecules are stonger than the h bonds in water
it is the delta h of solvent plus the delta h of mix
delta hof solute is the positive part and delta h of hydration is negative = delta h of solution
dynamic equilibrium
when the rates of dissolution and deposition are equal
Saturated solution
when dynamic equilibrium has been reached(if u add more solue it won't dissolve)
unsaturated
a solution containing less than the equilibrium amount of solute
if u add more solute itwill dissolve
supersaturated
in certain conditions a solutions can contain moe than the equilibrium amount
unstable
recrystalization
technique for purification
put the solid in water at an elevated temp, enough to ba saturated at that elevated temp as it cools it becomes supersaturated and excess solid comes out, if cooled slowly it comes out in crystals which reject impurities
henrys law
Sgas+kHPgas
the equations shows that the solubility of the gas in a liquid is directly proportional to the pressure of a gas above the liquid
concentrated
containing large quantities of the solute compared to the solvent
colliod
a mixture in which a dispersed substance is inely divided in dispersing medium
ex fog smoke milk
molarity
amount of solute(moles)volume of solution(liters)
molality
amount of solute(moles)mass of solvent(kg)
parts by mass
a ratio of the mass of the soute to the mass of the soution multiplied by a multiplication factor
the multiplication factor depends on the particular units used for percent by mss its 100 for ppm its 10 to the 6th for ppb its 10 to the 9th
parts by volume
is a ratio of volume of solute to volume of solution multiplication facts are identical to parts by mass
mole fraction
amount solute(mole)total amount of solute and solvent(moles)
Raoults law
Psolution=XsolventP0solvent
Psolution=vapor pessure of the solution
Xsolvent=the mole fraction of the solvent
Psolvent=vapor presure of the pure solvent
colligative property
properties that depend on the amount of solute and not the type of solute
ex freezing point depression and bioling point elevation
vapor presure of a solution
vapor pressure of a solution is lower than the vapor pressure of the pure solvent picture n page 541
freezing point depression
the freezing point of a solution containing a nonvolitile solute is less han that of a pure solvent
change in temp=m * Kf
change in temp =the change in frezzing point in degrees celcius
m=the molality of the solutionin moles perkilogram solvent
Kf=the freezing point depression constant for that solvent
bioling point elevation
the boiling point of a solution containing a nonvolitile solute is greater than that of the pure solvent
the change in temp=m*Kb
the change in temp=the change in boiling point
m=molality of the solution in moles per kilogram solvent
Kb=elevation of boiling point constant for that solvent
osmosis
the flow of solvent from a solution of lower solute concentration to one of higher solute concentration
osmotic pressure
the pressure required to stop osmotic flow
II=MRT
M=molarity of the soltion
T=temperature inK
R=ideal gas constant(0.08206L*atm/mol*K
precipitate
a solid insoluble compound that forms in and separates from a solution
precipitation reaction
a reaction in which a solid insoluble product forms upon mixing two solutions
net ionic equation
an equation that shows only the species that actually changed during the reaction
complex ion
an ion that contains a central metal ion bound to one or more ligands
intensive property
a property such as density that is independent of the amount of a given substance
intensive property v colligative property
intensiv property is like density it doesnt matter how much of something you have the density is stil the same
colligative property depends on the amount bt not the type
complex ions
an ion that contains a central metal ion bound to one or more ligands
law of mass action
ratio : products on top rectants on bottom
anything disolved(aq) is put in brackets(molarity)
and anythin in gas state is put as a subscript of P (partial pressure)
s and l ae ignored
equilibrium constant
K
equilibrium position
whether it shifts rt or left or no shift when stuff is changed