Features of Hydrogen Bonding
Hydrogen Bonding and Colligative
properties Association
"Colligative properties" are
those that depend on the number of particles and not necessarily the nature
of particles. Molecular weights determined by colligative property
measurements may be different from true values.
Thus the molecular weight of NaCl using such measurement will
be half its actual value since NaCl exists in solution as two
particles. Benzoic acid on the other hand will give twice the
actual value since it exists as an association of two particles
(dimer).
- In many hydrogen bonded aliphatic acids it has been observed
that the experimental molecular weights are considerably higher
than their true values.
- These values decrease with increase in
temperature approaching the actual molecular weights at elevated
temperatures.
Temp in K
Experimental
mol. wt.
True mol wt.
CH3COOH
(Acetic acid)
350
92.7
60
375
84.5
395.8
73.9
428
67.7
467.8
67.9
CH3CH2CH2COOH
(Butyric acid)
414.5
110.9
88.1
445.8
107.1
468.6
101.0
CH3(CH2)5COOH
(Heptanoic
acid)
462.5
138.1
130.2
473.7
136.5
500.2
133.5
From the above values the following conclusions may be drawn.
- The experimental values of molecular weights are greater than
the actual values.
- These abnormal molecular weights are due to association between
two or three molecules of the acids.
- This association is possible through inter molecular hydrogen
bonding
- If the compound exists completely as dimers then the molecular
weight should have been double.
- The compound exists as an equilibrium mixture containing the
monomers, the dimers and even trimers wherever possible.
- Increasing temperature increase the average kinetic energy
of the molecules, this disrupts hydrogen bonding inter action
shifting the equilibrium in favour of the monomeric form.
- At higher temperature the value of molecular weight is closer
to the actual value.
* Data on this page is from: Hydrogen bonding, Vinogradov
/ Linnell
Copyrights: 2005 www.chemvista.org All Rights Reserved