20. Low molecular weight molecules
20
Molecular Weight
Single Value
Synthetic Polymers
Broad Range of Values
Biological Polymers
# of Molecules
# of Molecules
Molecular Weight
Molecular Weight
Single Value
21. Number Average Molecular Weight
• End-group analysis
determine the number of end-groups in a sample of
known mass
• Colligative Properties
most commonly osmotic pressure, but includes
boiling point elevation and freezing point depression
Weight Average Molecular Weight
• Light scattering
translate the distribution of scattered light intensity
created by a dissolved polymer sample into an
absolute measure of weight-average MW
22. Viscosity Average Molecular Weight
• Viscometry
The viscosity of an infinitely dilute polymer
solution relative to the solvent relates to
molecular dimension and weight.
Molecular Weight Distribution
• Gel permeation chromatography
fractionation on the basis of chain
aggregate dimension in solution.
23. Measurement of Number Average Molecular Weight
2.3.1 End-group Analysis
A. Molecular weight limitation up to 50,000
B. End-group must have detectable species
a. vinyl polymer : -CH=CH2
b. ester polymer : -COOH, -OH
c. amide and urethane polymer : -NH2, -NCO
d. radioactive isotopes or UV, IR, NMR detectable functional group
24. Mn =
2 x 1000 x sample wt
meq COOH + meq OH
C.
D. Requirement for end group analysis
1. The method cannot be applied to branched polymers.
2. In a linear polymer there are twice as many end of the chain
and groups as polymer molecules.
3. If having different end group, the number of detected end group
is average molecular weight.
4. End group analysis could be applied for
polymerization mechanism identified
E. High solution viscosity and low solubility : Mn = 5,000 ~ 10,000
Measurement of Number Average Molecular Weight
25. ? 1: Find a procedure for End group
Analysis for one kind of Polymer
26. Colligative properties
Properties determined by the number of
particles in solution rather than the type
of particles.
Vapour pressure lowering
Freezing point depression
Boiling point elevation
Osmotic pressure
27. How Vapor Pressure Lowering Occurs
• Solute particles take up space in a
solution.
• Solute particles on surface decrease
number of solvent particles on the
surface.
• Less solvent particles can evaporate
which lowers the vapor pressure of a
liquid.
28. Vapor Pressures of Pure Water and a Water Solution
The vapor pressure of water over pure water is greater than the
vapor pressure of water over an aqueous solution containing a
nonvolatile solute.
Solute particles take up
surface area and lower
the vapor pressure
29. *
A
A
A P
X
P
A
X
Let component A be the solvent and B the solute.
solute B is nonvolatile
Applying Raoult’s Law:
where: PA= vapor pressure of the solvent in solution
= vapor pressure of the solution
PA
*= vapor pressure of the pure
solvent
XA= mole fraction of the solvent
30. The lowering in vapor pressure,
A
A P
P
P
*
P
A
A
A X
P
P *
*
*
)
1
( A
A P
X
*
A
B P
X
P
where: B
X = mole fraction of solute
31. When a non volatile solute is added to
solvent:
• Vapor pressure of solvent is lowered
• solution formed must be heated to higher
temperature than boiling point of pure
solvent to reach a vapor pressure of 1 atm.
• This means that non volatile solute elevates
the boiling point of the solvent which we call
boiling point elevation
38. Boiling-point elevation (Ebulliometry)
Tb : boiling point elevation
H v : the latent heats of vaporization
We use thermistor to major temperature. (1×10-4℃)
limitation of Mn : below 20,000
(
C HvMn
Tb
)C=0 =
RT2
+ A2C
42. Freezing-point depression (Cryoscopy)
Tf : freezing-point depression,
C : the concentration in grams per cubic
centimeter
R : gas constant
T : freezing point
Hf: the latent heats of fusion
A2 : second virial coefficient
(
C
Tf
)C=0 =
Hf Mn
RT2
+ A2C