Drill: Draw LDDs for: BF
3
NH
3
Solids:
•
Definite size & shape
• Particles vibrate about fixed points
Liquids:
•
Definite size but no shape
•
Particles vibrate about moving points
C
3
H
7
NO
Gases:
• No definite size or shape
•
Particles move at random
Melting Point
•
Temperature at which the solid phase & liquid phase are at equilibrium
•
MP & FP occur at the same temperature
•
Temperature at which the vapor pressure of a solid = the vapor pressure of its liquid phase
Boiling Point:
• Temperature at which the liquid phase & gaseous phase are at equilibrium
•
Temperature at which the vapor pressure of a liquid = the vapor pressure of its gaseous phase or atmospheric P
•
BP & CP occur at the same temperature
Solutions: Homogeneous mixture made up of at least one solute dissolved in the solvent
Solute: The substance being dissolved or the portion in a lesser molar amount
Solvent: The substance doing the dissolving or the portion in the greater molar amount
Colloid: Mixtures with slightly larger particles in which light passes & particles stay suspended
Suspension: Mixtures with slightly larger particles which block or reflect light
Tyndall Effect: Because light reflects off suspended particles, the light ray can be seen from the side
Size Comparison: Solution < Colloid < Suspension
Soluble: When one substance (solute) dissolves in another (solvent)
Solubility: The max amount of one substance (solute) dissolved in another (solvent)
Concentration: The amount of solute dissolved into solution
Concentrated Solution: A solution with a relatively large amount of solute dissolved
Dilute Solution: A solution with a relatively small amount of solute dissolved
Saturated Solution: A solution with the maximum amount of solute dissolved in the solution
Unsaturated Solution: A solution with less than the maximum amount of solute dissolved in solution
Supersaturated Solution: A solution with more than the maximum amount of solute dissolved in solution

Drill: Draw the LDDs for C
4
H
8
& HNO
3
Solution Chemistry:
Solution Measures:
•
Concentration: % soln
–
Mass of one portion per the total mass, all times 100 %
– % soln
= m a
/m total x 100 %
•
Molarity (M)
– Moles of solute per liter of solution (mole/L)
•
Molality (mo)
–
Moles of solute per kilogram of solvent (mole/kg)
•
Mole Fraction (X)
–
Moles of one portion per total number of moles in the solution (mole a
/mole total
)
Problems:
•
Calculate the molarity of a 250 mL solution containing 5.0 g NaOH dissolved in water:
•
Calculate the molality of 69 g of C
2
H
5
OH dissolved in 500.0 mL of water:
•
Calculate the mole fraction of each portion when 92 g of C
2
H
5
OH dissolved in 144 mL of water
•
Calculate the molality & mole fraction of a solution containing 46 g of C
2
H
5
OH dissolved in 1782 mL of water
Drill: Calculate the mass of KI required to make 250 mL of 0.500 M KI.
Colligative Properties: Properties dependent only on the concentration of particles in solution
•
Vapor pressure (VP): VP solution
= (VP solvent
)(X solvent
)
•
X = mole fraction
•
VP = vapor pressure
•
Boiling & Freezing points (BP) & (FP)
• 
T = change in BP or FP
• i = ionic activity
• K = BP or FP constant
•
Osmotic pressure (

)
• 
= i MRT
• p = osmotic pressure
• i = ionic activity
• M = Molarity
Problems:
• Calculate the vapor pressure of a solution containing 150 g C
5
H
10
O
5
in 162 mL of water at 30 o C
• Calculate the osmotic pressure of a solution containing 24 g of NaOH dissolved in 250 mL
solution at 27 o C
• Calculate the BP of a solution containing 24 g of NaOH dissolved in 250 mL of HOH. o (K
BP
= 0.512
o
C/mo)

Drill: Calculate the vapor pressure of a solution containing 75 g C
5
H
10
O
5
in 171 mL of water at 30 o
C
•
VP = 31.8 mm Hg
Molarity (M): M = Moles of solute
Liter soln
Molality (mo): mo = Moles of solute
kg solvent
Mole Fraction (X): X = Moles anything
total moles
Vapor Pressure soln
(VP): VP soln
= (X solvent
)(VP solvent
)

BP or FP:

T
BP
= i moK
BP

T
FP
= i moK
FP
Osmotic Pressure

):

= i MRT
Problems:
•
Calculate BP & FP of 20.0 g of NaOH in 200.0 mL water (K
BP
= 0.512
o
C/mo) (K
FP
= -1.86
o
C/m)
•
Calculate the osmotic pressure of a solution containing 14.8 g of Ca(OH)
2
dissolved in
250 mL solution at 27 o
C
•
Calculate the VP of a solution containing 36 % glucose (C
6
H
12
O
6
) in water at 29 o
C: o (VP water
= 30.0 mm Hg)
Drill: Calculate the BP of a solution containing 45 % formaldehyde (CH
2
O) in water: (K
BP
= 0.512
o
C/mo)
Test Review
Classify the type of Bonding found in each pair of elements:
Fe-Cl Fe-Cr C-Cl H-Br S-O
Classify the type of Intermolecular Force found in each pair of substances:
K-I
H
2
& Cl
2
Draw LDDs for:
HF & HF H
2
& HBr
BH
3
NCl
3
CF
4
HBr & HI CH
4
& C
2
H
6
C
4
H
6
O BrO
4
-1
Problems:
•
Calculate the BP of a solution containing 120 g C
3
H
7
OH in 250 mL of water.
(K
BP
= 0.512
o
C/mo) (K
FP
= -1.86
o
C/mo)
•
Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 50.0 mL solution at 27 o
C
•
Calculate the vapor pressure of a solution containing 12.0 g C
3
H
8
O in 14.4 mL HOH. o VP solvent
= 120 kPa
• Calculate the molarity of 33.1 g of Pb(NO
3
)
2
dissolved in 250 mL of solution.
•
Calculate the mass of lead(II)nitrate required to make 250 mL of 0.40 M Pb(NO
3
)
2
• Calculate the BP of a solution containing 29.9 g of CoBr
3
dissolved in 75 mL of water. o K
BP
= +0.512
o C/mo
• Calculate the molality of a solution that is 33.1 % by mass Pb(NO
3
)
2 in water