Chqpter 13 Flashcards
Define solubility
Solute dissolved in saturated solution
Saturated solution
Has max amount of solute
Define unsaturated solution
Less solute than saturated solution
Supersaturated solution
More solute than saturated
Define ion-dipole force
Ion attracted to partial charge on polar molecule
Dipole-Induced Dipole force
Partial charge on polar molecule give temporary partial charge to non polar neighbor
Ion-Induced Dipole
Ion charge give temporary partial charge to non polar neighbor
Molarity Equation
M= (moles of solute) / (Liters of solution) = mol/L
Molality Equation
m=(moles of solute) / (kg of solvent) = mol/kg
Henry’s law
C=kP
C=concentration
K=moles/L
P= atm
Raoults Law
Pa=(Xa)(P°a)
Pa= vapor pressure above solution
Xa= mole fraction in solution
P°a= vapor pressure of pure solvent
Define Colligative Properties
•Physical properties that depend on solute particles NOT IDENTITY
(Ex: boil/freeze point, osmotic pressure)
VANT HOFF FACTOR
• equation for colligative properties
• non-electrolytic: i=1
• electrolytic: i= # of ions solute dissociates into
Freezing point depression equation
Tf= (T°f) - (change in Tf)
Tf= solution freeze point
T°f= pure solvent freeze point
Osmotic pressure equation
OP= (i)(M)(R)(T)
i= vant hoff
M= molarity
R= gas constant
T=Tempature
Isotonic Solution
(Organ Transplant)
• same concentration both side of membrane
• burst if stored in water
Hypertonic Solution
(Food preservation)
•high concentration outside membrane
•salt pulls H2O from microbe & kills
Hypotonic Solution
(Tree Growth)
•low concentration outside membrane
• H2O pulled through sap to top of tree
Reverse Osmosis
(Water Purification)
•reverse solvent flow by pressure bigger than osmotic
•obtain H2O w/ low solute concentration
