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CHM2CH13
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solubility
the amount of a substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution
solvation
the clustering of solvent molecules around a solute particle
saturated solution
a solution in which undissolved solute and dissolved solute are in equilbrium
unsaturated solution
a solution containing less solute than a saturated solution
supersaturated solution
a solution containing more solute than an equivalent saturated solution
concentration
the quantity of solute present in a given quantity of solvent or solution
polar covalent bond
a covalent bond in which the electrons are not shared equally
non-polar covalent bond
a covalent bond in which the electrons are shared equally
Henry's Law
a law stating that the concentration of the gas in a solution is proportional to the pressure of the gas over the solution
S
g
= k P
g
"like dissolves like"
polar substances dissolve in polar solvents
non-polar substances dissolve in non-polar substances
Factors that affect solubility
solute-solvent interactions
: stronger the attractions are, the greater the solubilty
pressure effects
: solubility increases with increase in pressure
temperature effects
: solubilty of most solids increases with increase in temp, solubilty of most gases decreases with increase in temp
molarity (M)
the concentration of a solution expressed in moles of solute per liter of solution
molality (m)
the concentration of a solution expressed as moles of solute per kilogram of solvent
mole fraction (X
comp
)
the ration of the number of moles of one compound of a mixture to the total number of moles of all components
mass percent
the number of grams of solute in each 100 g of solution
parts per billion (ppb)
the concentration of a solution in grams of solute per 10
9
(billion) grams of solution
parts per million (ppm)
the concentration of as solution in grams of solute per 10
6
(million) grams of solution
colligative property
a property of a solvent that depends on the total concentration of solute particles present
vapor pressure lowering
freezing point depression
boiling point elevation
osmotic pressure
vapor pressure lowering
vapor pressure of a volatile solvent above a solution containing a non volatile solute is proportional to the solvent's concentration in the solution
freezing point depression
K
f
the change in the freezing point of a solution is directly proportional to the solute molality
molal freezing point depression constant
change
T
f
=
K
f
m
boiling point elevation
K
b
the change in boiling point of a solution is directly proprotional to the solute molality
molal boiling point depression constant
change
T
f
=
K
f
m
osmotic pressure
the pressure required to stop osmosis from a pure solvent to a solution
Raoult's Law
P
solution
= X
solvent
P
0
solvent
Partial pressure exerted by the solvent vapor above the solution equals the mole fraction of the solvent times the vapor pressure of the pure solvent.
Author
pamichael5350
ID
122606
Card Set
CHM2CH13
Description
Chapter 13 Properties of Solutions
Updated
2011-12-11T04:45:24Z
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