The properties of water and their role in colloidal and biological systems:
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| Main Author: | |
|---|---|
| Format: | Book |
| Language: | English |
| Published: |
Amsterdam [u.a.]
Elsevier
2008
|
| Edition: | 1. ed. |
| Series: | Interface science and technology
16 |
| Subjects: | |
| Online Access: | Inhaltsverzeichnis |
| Physical Description: | XIV, 224 S. graph. Darst. 24cm |
| ISBN: | 9780123743039 0123743036 |
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| 020 | |a 9780123743039 |9 978-0-12-374303-9 | ||
| 020 | |a 0123743036 |c (hbk.) : £100.00 |9 0-12-374303-6 | ||
| 035 | |a (OCoLC)229031857 | ||
| 035 | |a (DE-599)GBV57211415X | ||
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| 084 | |a UP 7500 |0 (DE-625)146433: |2 rvk | ||
| 100 | 1 | |a Van Oss, Carel J. |e Verfasser |4 aut | |
| 245 | 1 | 0 | |a The properties of water and their role in colloidal and biological systems |c Carel Jan van Oss |
| 250 | |a 1. ed. | ||
| 264 | 1 | |a Amsterdam [u.a.] |b Elsevier |c 2008 | |
| 300 | |a XIV, 224 S. |b graph. Darst. |c 24cm | ||
| 336 | |b txt |2 rdacontent | ||
| 337 | |b n |2 rdamedia | ||
| 338 | |b nc |2 rdacarrier | ||
| 490 | 1 | |a Interface science and technology |v 16 | |
| 650 | 4 | |a Surface chemistry | |
| 650 | 4 | |a Surfaces (Physics) | |
| 650 | 4 | |a Water |x Analysis | |
| 650 | 4 | |a Water |x Properties | |
| 650 | 0 | 7 | |a Hydrochemie |0 (DE-588)4072678-2 |2 gnd |9 rswk-swf |
| 689 | 0 | 0 | |a Hydrochemie |0 (DE-588)4072678-2 |D s |
| 689 | 0 | |5 DE-604 | |
| 830 | 0 | |a Interface science and technology |v 16 |w (DE-604)BV019653877 |9 16 | |
| 856 | 4 | 2 | |m Digitalisierung UB Bayreuth |q application/pdf |u http://bvbr.bib-bvb.de:8991/F?func=service&doc_library=BVB01&local_base=BVB01&doc_number=016738148&sequence=000002&line_number=0001&func_code=DB_RECORDS&service_type=MEDIA |3 Inhaltsverzeichnis |
| 999 | |a oai:aleph.bib-bvb.de:BVB01-016738148 | ||
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| adam_text | Contents
Prefece
XIII
t.
General
and Historical Introduction
ι
Preamble
ι
ι.
Some Examples of Polar Forces Interacting in the Mammalian Blood Circulation
2
2.
Early Examples of the Treatment of Non-Covalent Interactions in Water
3
2.1.
DLVO and Non-DLVO forces
3
2.2.
Good s introduction of a
Ф
-factor
and Fowkes evaluation of a van
der
Waals/Non-van
der Waals
ratio of the surface tension of water
4
2.3.
The three van
der Waals
forces: Are some of them polar?
4
3.
Macroscopic-Scale Interactions, Chaudhury s Thesis and
Lifshitz-van
der Waals
Forces
5
4.
Rules for Repulsive
Apoiar
(van
der Waals)
Forces between Different Polymers
Dissolved in an
Apoiar
Liquid, Compared with the Rules for Repulsive Polar
(Lewis Acid-Base) Forces between Identical Polymers, Particles or Cells,
Immersed in Water
5
4.1.
Van
der Waals
repulsions between different materials immersed in an
apoiar
liquid
5
4.2.
Lewis acid-base repulsions between identical polar materials, immersed
in water
6
5.
The Fallacy of Designating Only One Single Component to Represent the Polar
Properties of the Surface Tension of a Polar Condensed-Phase Material
7
6.
More Recent Developments
8
6.1.
Properties of water
8
6.2.
Influence of immersion in water on the behavior of non-polar and polar
entities
9
Section A. Non-Covalent Energies of Interaction—Equations and
Combining Rules
11
2.
The
Apoiar
and Polar Properties of Liquid Water and Other
Condensed-Phase Materials
13
1.
The yLW and xAB Equations
13
vi
The Properties of Water and their Role in Colloidal and Biological Systems
1.1.
Apoiar
surface tensions
13
1.2.
Surface tensions of polar materials
Ч
1.3.
Surface and
interfacial
tensions
14
1.4.
The
Dupré
equations
16
1.5.
The Young equation
17
1.6.
The
Young-Dupré
equation and contact angle determination
17
2.
The Values for yLW,y+ and
y
for Water at
20 °С 23
3.
Apoiar
and Polar Surface Properties of Various Other Condensed-Phase
Materials
24
3.1.
Liquids
24
3.2.
Synthetic polymers
25
3.3.
Plasma proteins (see Table
2.3) 25
3.4.
Carbohydrates
27
3.5.
Clays and other minerals
27
3.6.
Large solid surfaces vs ground solids—Direct contact angle
measurements vs thin layer wicking
29
3.
The Extended OLVO Theory
31
1.
Hamaker
Constants and the Minimum Equilibrium Distance between Two
Non-Covalently Interacting Surfaces of Condensed-Phase Materials
32
1.1.
Hamaker
constants and their relation to yLW and the minimum
equilibrium distance, d0, between two surfaces of condensed-phase
materials
32
1.2.
The minimum equilibrium distance, d0, as a constant
33
1.3.
The proportionality constant
Aü/y,LW
34
2.
The DLVO Theory Extended by the Addition of Polar Interaction Energies
Occurring in Water
34
2.1.
DLVO and XDLVO theories
34
2.2.
Need for separate treatments of LW,
AB
and EL energies as a function
of distance
35
3.
Decay with Distance of Lifshitz-van
der Waals
Interactions
36
3.1.
LW decay with distance
36
3.2.
Retardation of the van
der Waals-London
forces
36
3.3.
Attractive and repulsive LW interactions
37
3.4.
Mechanism of LW action at a distance in water
38
4.
Decay with Distance of Lewis Acid-Base Interactions
38
4.1.
Decay with distance of
AB
free energies and forces
38
4.2.
Mechanisms of
AB
attractions and repulsions at a distance in water
39
5.
Decay with Distance of Electrical Double Layer Interactions
40
5.1.
Equations and relation between the
ζ
-potential and the
ψο
-potential
40
5.2.
Electrokinetic determination
ofç
-potentials
41
6.
Influence of the Ionic Strength on Non-Covalent Interactions in Water
42
6.1.
Definition of ionic strength
42
Contents
vii
6.2.
Influence of ionic strength on LW interactions
42
6.3.
Influence of the ionic strength on
AB
interactions
43
6.4.
Influence of the ionic strength on EL interactions
43
7.
An EL-AB Linkage
44
8.
Role of the Radius of Curvature, R, of Round Particles or Processes in
Surmounting
AB
Repulsions in Water
45
9.
Comparison between Direct Measurements via Force Balance or Atomic Force
Microscopy, and Data Obtained via Contact Angle Determinations, in the
Interpretation of Free Energies vs Distance Plots of the Extended DLVO
Approach
46
9.1.
Direct measurements of forces vs distance
46
9.2.
Determination of the separate LW,
AB
and EL contributions
47
9.3.
Advantages and disadvantages of the extended DLVO approach vs
contact angle determinations
48
Section B. Surface Thermodynamic Properties of Water with Respect
to Condensed-Phase Materials Immersed in It
49
4.
Determination of
Interfacial
Tensions between Water and Other
Condensed-Phase Materials
51
1.
The
Interfacial
Tension between a Solid (S) and a Liquid (L)
51
1.1.
Importance of the
interfacial
tension
(γ%Ο
between
S
and
L
51
1.2.
The polar versions of ysl and
y¡w
52
2.
The
Interfacial
Tension between an
Apoiar
Material or Compound (A) and
Water (W)
52
2.1.
The /aw equation
52
2.2.
Measurement of
уд у
between
apoiar
organic liquids and water
53
3.
The
Interfacial
Tension between Polar Compounds or Materials and Water
54
3.1.
Expression of /lw between
monopolar
compounds and water
54
3.2.
Measurement of ylw between polar organic liquids and water
54
3.3.
The zero time dynamic
interfacial
tension between polar organic liquids
and water: ylw°
55
3.4.
Determination of yiw° via the aqueous solubility of
і
56
3.5.
Derivation of
y¡w°
from the polar equations for ym, after having
determined the components and parameters of
y¡
57
3.6.
Determination of ylw via the Young equation, the polar properties of
y¡
and the water contact angle measured on material,
і
57
5.
The
interfacial
tension/free energy of interaction between water and
identical condensed-phase entities, i, immersed in water,
w
59
1.
The
AG;«,,
Equation Pertaining to Identical Entities, i, Immersed in Water,
w
59
1.1.
AG,w,LW, or the
apoiar
component of AG1W1IF
60
1.2.
AG,wiAB. or the polar component of AG1W1IF
60
viii
The Properties of Water and their Role in Colloidal and Biological Systems
1.3.
The use of AGiwiIF in the quantitative definition of hydrophobicity and
hydrophilicity
60
2.
Mechanism of Hydrophobic Attraction in Water
63
2.1.
AGiwi11 and the hydrophobic effect
63
2.2.
Increasing or decreasing the hydrophobizing capacity of water
64
3.
Mechanism of Hydrophilic Repulsion in Water
66
3.1.
AGiwi11 and hydrophilic repulsion, or hydration pressure
66
3.2.
Increasing or decreasing the hydrophilic repulsion occurring in water
66
4.
Osmotic Pressures of
Apoiar
Systems as well as of Polar Solutions, Treating
Aqueous Solutions in Particular
67
4.1.
Osmotic pressure in
apoiar
systems
67
4.2.
Osmotic pressure of aqueous polymer solutions
68
4.3.
Osmotic pressure of linear polar polymers, dissolved in water
68
4.4.
Conclusions regarding osmotic pressure
71
6.
The
Interfacial
Tension/Free Energy of Interaction between Water and Two
Different Condensed-Phase Entities, i, Immersed in Water,
w
73
1.
The AGiw2 Equation Pertaining to Two Different Entities,
1
and
2,
Immersed
in Water,
w
73
1.1.
AGiw2LW, or the
apolar
component of AGiw2
74
1.2.
AGiw2AB, or the polar component of AGiw2
74
1.3.
Possible role of AG]w2EL
75
2.
Examples of AGiW2 Interactions
75
2.1.
Hydrophobic attraction between a hydrophobic and a hydrophilic entity,
immersed in water
75
2.2.
Hydrophilic repulsion between different hydrophilic entities, immersed
in water
76
2.3.
Advancing freezing fronts, causing a repulsion or an attraction,
depending on the hydrophilicity or hydrophobicity of the immersed
particles, cells or macromolecules
78
2.4. Chromatographie
applications of hydrophobic interactions and their
reversal
81
2.5.
Polymer phase separation in water
81
3.
Water Treated as the Continuous Liquid Medium for AG]wi and AGiW2
Interactions
83
7.
Aqueous Solubility and Insolubility
85
1.
The Solubility Equation
85
1.1.
The contactable surface area (Sc)
86
1.2.
Contactable surface areas do not apply to spherical molecules or
particles
87
2.
Aqueous Solubility of Small Molecules
89
2.1.
Aqueous solubility of small non-ionic organic molecules
89
2.2.
Aqueous solubilities of inorganic salts
89
Contents
¡x
2.3.
Aqueous solubility of surfactants manifests itself as their critical micelle
concentration
(cmc)
91
3.
Aqueous Solubility of Polymeric Molecules
93
3.1.
Similarities between the aqueous solubility of polymer molecules and
the stability of particle suspensions in water
93
3.2.
Aqueous solubility of linear polymers
94
3.3.
Aqueous solubility of globular proteins
94
3.4.
Aqueous solubility of non-globular, fibrous proteins
96
3.5.
Aqueous solubility of gel-forming polymers
96
4.
Influence of Temperature on Aqueous Solubility
98
5.
Aqueous Insolubilization (Precipitate Formation) Following the Encounter
between Two Different Solutes that Can Interact with Each Other When
Dissolved in Water
98
5.1.
Classes of pairs of compounds that readily precipitate when
encountering each other in aqueous solution
98
5.2.
Mechanism of insolubilization upon the encounter of two different
compounds with opposing properties
99
5.3.
Mechanism of the formation of specifically impermeable precipitate
barriers
100
5.4.
Examples of specifically impermeable precipitate barriers or
membranes
101
5.5.
Single diffusion precipitation
109
8.
Stability Versus Flocculation of Aqueous Particle Suspensions
113
1.
Stability of Particle Suspensions in Water
113
1.1.
LW,
AB
and EL energies and the extended
DIVO
theory
114
2.
Stability of Charged and Uncharged Particles, Suspended in Water
117
2.1.
Role of attached ionic surfactants or electrically charged polymers
in conferring stability to aqueous particle suspensions
117
2.2.
Non-charged particles or particles of low charge stabilized by non-ionic
surfactants or polymers, via steric stabilization
118
3.
Linkage between the EL Potential and
AB
Interaction Energies in Water-
Importance of
AB
Interaction Energies for the Stability vs Flocculation Behavior
of Aqueous Suspensions of Charged Particles—
The Schulze-Hardy Phenomenon Revisited
123
3.1.
Mechanism of Schulze-Hardy type flocculation
123
3.2.
Linkage between changes in
ç-potential
and especially, changes
in the electron-donicity of polar surfaces, when immersed in water
126
4.
Destabilization of Aqueous Particle Suspensions by Cross-Linking
128
4.1.
Cross-linking of latex particles for diagnostic purposes—
The latex fixation test
128
4.2.
Cross-linking of human red blood cells with antibodies to cause
flocculation (hemagglutination) for blood group determinations
129
X The Properties of Water and their Role in Colloidal and Biological Systems
Section
С
Physical and Physicochemical Properties of Water
131
9.
Cluster Formation in Liquid Water
133
1.
Size of Water Molecule Clusters
133
1.1.
Measurement of the cluster size of water via its solubility in organic
solvents
133
1.2.
Variability as a function of temperature CO of the cluster size as well as
of the viscosity of water
134
1.3.
When water cluster size decreases with an increase in T, its Lewis acidity
increases and its Lewis alkalinity decreases
135
2.
Implications of the Increased Lewis Acidity of Water Following Increases in
Τ
135
2.1.
Consequences for the aqueous solubility of solutes and for the stability
of aqueous suspensions as a function of
Τ ΐ35
2.2.
Consequences for the attachment or detachment among two different
solutes and/or solids, immersed in water, as a function of
Τ
136
3.
Influence of Cluster Formation in Liquid Water on the Action at a Distance
Exerted by Polar Surfaces when Immersed in Water
137
3.1.
Connection between cluster size and the decay length of water
137
3.2.
The influence of cluster formation in liquid water on the XDLVO approach
pertaining to the stability of aqueous suspensions of human blood cells
139
10. Hydration
Energies of Atoms and Small Molecules in Relation to Clathrate
Formation
141
Preamble
141
1.
Free Energy of
Hydration
of Atoms and Small Molecules Immersed in Water
142
1.1.
The
AG™
part
142
1.2.
The AGww part
143
1.3.
AGjw and AGWW combined
143
2. Hydration
of Small
Apoiar
Molecules
144
3. Hydration
of Small Partly Polar Molecules
145
4.
Clathrate Formation as
a
Hydration
Phenomenon Occurring with Atoms or Small
Molecules
146
4.1.
The free energy of cohesion between the water molecules in liquid water
only contributes to the hydration energy of immersed atoms or small
molecules
146
4.2.
Influence of AGjwIF on larger molecules or particles, immersed in water
146
4.3.
Conclusion
147
4.4.
Alternative and simplified explanations
147
11.
The Water-Air Interface
149
1.
Hyperhydrophobicityofthe Water-Air Interface
149
1.1.
Causes of the hyperhydrophobicity of the water-air interface
149
Contents
1.2. Hyperhydrophobicity
of the water-air interface as the sole cause of the
increased value of the water contact angle when measured on rough
solid surfaces
151
1.3.
Hyperhydrophobicity of the water-air interface as the basis of flotation
as a separation method
152
2.
The f-Potentialof Air or Gas Bubbles in Water
152
3.
Repulsion versus Attraction of Various Solutes by the Water-Air Interface
153
3.1.
Determination of repulsion or attraction of solutes by the water-air
interface
153
3.2.
Repulsion of hydrophilic or near-hydrophilic solutes by the water-air
interface
154
3.3.
Solutes which comprise hydrophobic components are strongly attracted
to the water-air interface
158
4.
Inadvisability of Using Aqueous Solutions for the Measurement of Contact
Angles
160
12.
Influence of the
pH
and the Ionic Strength of Water on Contact Angles
Measured with Drops of Aqueous Solutions on Electrically Charged,
Amphoteric and Uncharged Surfaces
161
1.
Influence of the
pH
of Water on Electrically Charged and Amphoteric Surfaces
161
1.1.
Electrically charged surfaces
162
1.2.
Amphoteric surfaces
162
1.3.
Importance of the f-potential of simply electrically charged as well as of
amphoteric surfaces
162
2.
Influence of the
pH
on Water Contact Angles Measured on (Non-Charged)
Hydrophobic as Well as on (Non-Charged) Hydrophilic Surfaces
163
3.
Influence of the Ionic Strength on Water Contact Angles
164
3.1.
Low ionic strengths
164
3.2.
High ionic strengths
164
3.3.
Low concentrations of salts with
plurivalent
counterions
164
4.
Comparison Between the Influence of
pH
and Increases in Ionic Strength
on Water contact Angles on Solid Surfaces as well as on the Surface Properties
of such Solid Surfaces when Completely Immersed in Water
165
4.1.
Uncharged solids or solid particles
165
4.2.
Influence of
pH
or added salt on electrically charged solid surfaces,
particles or macromolecules
165
5.
Conclusions
166
13.
Macroscopic and Microscopic Aspects of Repulsion Versus Attraction
in Adsorption and Adhesion in Water
167
1.
Macroscopic-Scale Repulsion vs Microscopic-Scale Attraction in Water
168
1.1.
The adsorption of human serum albumin
(HSA)
onto metal oxide particles
immersed in water
168
xii
The Properties of Water and their Role in Colloidal and Biological Systems
2.
Methodologies Used in Measuring Protein Adsorption onto and Desorption
from Metal Oxide Particles in Water
171
2.1.
The continuous circulation device
171
2.2.
Determination of AG]w2(mac) and AGiw2(mic)
173
2.3.
Influence of the
pH
of the aqueous medium on protein adsorption and
desorption
173
2.4.
Other desorption approaches
174
3.
Hysteresis of Protein Adsorption onto Metal Oxide Surfaces, in Water
176
3.1.
Hysteresis interference with the determination of Keq and k,j
176
3.2.
Hysteresis following hydrophilic adsorption
176
3.3.
Hysteresis following adsorption onto a hydrophobic surface
177
3.4.
Absence of hysteresis when adsorptive forces are purely electrostatic
177
3.5.
Hysteresis as a function of adsorption time
179
3.6.
Importance of using the value for pre-hysteresis
Кеч ^°
i8o
3.7.
Determination of K^1 *0
180
4.
Kinetics of Protein Adsorption onto Metal Oxide Surfaces Immersed in Water
181
4.1. Von Smoluchowski s
approach applied to the kinetic adsorption rate
constant, ka
182
4.2. Von
Smoluchowski s
f
factor
182
4.3.
Determination of
f
and
ψ
і8г
4.4.
The equilibrium binding constant and the kinetic rate constants
184
14.
Specific Interactions in Water
187
1.
Innate and Adaptive Ligand-Receptor Interactions in Biological Systems
187
1.1.
Specific innate ligand-receptor interactions
187
1.2.
Specific adaptive interactions
192
2.
The Forces Involved in Epitope-Paratope Interactions
196
2.1.
Mechanisms and outcomes of epitope-paratope interactions
196
2.2.
Roles of the three non-covalent forces
201
2.3.
Minor or dubious mechanisms of specific bond formation
204
REFERENCES
207
Subject Index
215
|
| adam_txt |
Contents
Prefece
XIII
t.
General
and Historical Introduction
ι
Preamble
ι
ι.
Some Examples of Polar Forces Interacting in the Mammalian Blood Circulation
2
2.
Early Examples of the Treatment of Non-Covalent Interactions in Water
3
2.1.
DLVO and Non-DLVO forces
3
2.2.
Good's introduction of a
Ф
-factor
and Fowkes' evaluation of a van
der
Waals/Non-van
der Waals
ratio of the surface tension of water
4
2.3.
The three van
der Waals
forces: Are some of them polar?
4
3.
Macroscopic-Scale Interactions, Chaudhury's Thesis and
Lifshitz-van
der Waals
Forces
5
4.
Rules for Repulsive
Apoiar
(van
der Waals)
Forces between Different Polymers
Dissolved in an
Apoiar
Liquid, Compared with the Rules for Repulsive Polar
(Lewis Acid-Base) Forces between Identical Polymers, Particles or Cells,
Immersed in Water
5
4.1.
Van
der Waals
repulsions between different materials immersed in an
apoiar
liquid
5
4.2.
Lewis acid-base repulsions between identical polar materials, immersed
in water
6
5.
The Fallacy of Designating Only One Single Component to Represent the Polar
Properties of the Surface Tension of a Polar Condensed-Phase Material
7
6.
More Recent Developments
8
6.1.
Properties of water
8
6.2.
Influence of immersion in water on the behavior of non-polar and polar
entities
9
Section A. Non-Covalent Energies of Interaction—Equations and
Combining Rules
11
2.
The
Apoiar
and Polar Properties of Liquid Water and Other
Condensed-Phase Materials
13
1.
The yLW and xAB Equations
13
vi
The Properties of Water and their Role in Colloidal and Biological Systems
1.1.
Apoiar
surface tensions
13
1.2.
Surface tensions of polar materials
Ч
1.3.
Surface and
interfacial
tensions
14
1.4.
The
Dupré
equations
16
1.5.
The Young equation
17
1.6.
The
Young-Dupré
equation and contact angle determination
17
2.
The Values for yLW,y+ and
y"
for Water at
20 °С 23
3.
Apoiar
and Polar Surface Properties of Various Other Condensed-Phase
Materials
24
3.1.
Liquids
24
3.2.
Synthetic polymers
25
3.3.
Plasma proteins (see Table
2.3) 25
3.4.
Carbohydrates
27
3.5.
Clays and other minerals
27
3.6.
Large solid surfaces vs ground solids—Direct contact angle
measurements vs thin layer wicking
29
3.
The Extended OLVO Theory
31
1.
Hamaker
Constants and the Minimum Equilibrium Distance between Two
Non-Covalently Interacting Surfaces of Condensed-Phase Materials
32
1.1.
Hamaker
constants and their relation to yLW and the minimum
equilibrium distance, d0, between two surfaces of condensed-phase
materials
32
1.2.
The minimum equilibrium distance, d0, as a constant
33
1.3.
The proportionality constant
Aü/y,LW
34
2.
The DLVO Theory Extended by the Addition of Polar Interaction Energies
Occurring in Water
34
2.1.
DLVO and XDLVO theories
34
2.2.
Need for separate treatments of LW,
AB
and EL energies as a function
of distance
35
3.
Decay with Distance of Lifshitz-van
der Waals
Interactions
36
3.1.
LW decay with distance
36
3.2.
Retardation of the van
der Waals-London
forces
36
3.3.
Attractive and repulsive LW interactions
37
3.4.
Mechanism of LW action at a distance in water
38
4.
Decay with Distance of Lewis Acid-Base Interactions
38
4.1.
Decay with distance of
AB
free energies and forces
38
4.2.
Mechanisms of
AB
attractions and repulsions at a distance in water
39
5.
Decay with Distance of Electrical Double Layer Interactions
40
5.1.
Equations and relation between the
ζ
-potential and the
ψο
-potential
40
5.2.
Electrokinetic determination
ofç
-potentials
41
6.
Influence of the Ionic Strength on Non-Covalent Interactions in Water
42
6.1.
Definition of ionic strength
42
Contents
vii
6.2.
Influence of ionic strength on LW interactions
42
6.3.
Influence of the ionic strength on
AB
interactions
43
6.4.
Influence of the ionic strength on EL interactions
43
7.
An EL-AB Linkage
44
8.
Role of the Radius of Curvature, R, of Round Particles or Processes in
Surmounting
AB
Repulsions in Water
45
9.
Comparison between Direct Measurements via Force Balance or Atomic Force
Microscopy, and Data Obtained via Contact Angle Determinations, in the
Interpretation of Free Energies vs Distance Plots of the Extended DLVO
Approach
46
9.1.
Direct measurements of forces vs distance
46
9.2.
Determination of the separate LW,
AB
and EL contributions
47
9.3.
Advantages and disadvantages of the extended DLVO approach vs
contact angle determinations
48
Section B. Surface Thermodynamic Properties of Water with Respect
to Condensed-Phase Materials Immersed in It
49
4.
Determination of
Interfacial
Tensions between Water and Other
Condensed-Phase Materials
51
1.
The
Interfacial
Tension between a Solid (S) and a Liquid (L)
51
1.1.
Importance of the
interfacial
tension
(γ%Ο
between
S
and
L
51
1.2.
The polar versions of ysl and
y¡w
52
2.
The
Interfacial
Tension between an
Apoiar
Material or Compound (A) and
Water (W)
52
2.1.
The /aw equation
52
2.2.
Measurement of
уд\у
between
apoiar
organic liquids and water
53
3.
The
Interfacial
Tension between Polar Compounds or Materials and Water
54
3.1.
Expression of /lw between
monopolar
compounds and water
54
3.2.
Measurement of ylw between polar organic liquids and water
54
3.3.
The zero time dynamic
interfacial
tension between polar organic liquids
and water: ylw°
55
3.4.
Determination of yiw° via the aqueous solubility of
і
56
3.5.
Derivation of
y¡w°
from the polar equations for ym, after having
determined the components and parameters of
y¡
57
3.6.
Determination of ylw via the Young equation, the polar properties of
y¡
and the water contact angle measured on material,
і
57
5.
The
interfacial
tension/free energy of interaction between water and
identical condensed-phase entities, i, immersed in water,
w
59
1.
The
AG;«,,
Equation Pertaining to Identical Entities, i, Immersed in Water,
w
59
1.1.
AG,w,LW, or the
apoiar
component of AG1W1IF
60
1.2.
AG,wiAB. or the polar component of AG1W1IF
60
viii
The Properties of Water and their Role in Colloidal and Biological Systems
1.3.
The use of AGiwiIF in the quantitative definition of hydrophobicity and
hydrophilicity
60
2.
Mechanism of Hydrophobic Attraction in Water
63
2.1.
AGiwi11" and the hydrophobic effect
63
2.2.
Increasing or decreasing the hydrophobizing capacity of water
64
3.
Mechanism of Hydrophilic Repulsion in Water
66
3.1.
AGiwi11" and hydrophilic repulsion, or "hydration pressure"
66
3.2.
Increasing or decreasing the hydrophilic repulsion occurring in water
66
4.
Osmotic Pressures of
Apoiar
Systems as well as of Polar Solutions, Treating
Aqueous Solutions in Particular
67
4.1.
Osmotic pressure in
apoiar
systems
67
4.2.
Osmotic pressure of aqueous polymer solutions
68
4.3.
Osmotic pressure of linear polar polymers, dissolved in water
68
4.4.
Conclusions regarding osmotic pressure
71
6.
The
Interfacial
Tension/Free Energy of Interaction between Water and Two
Different Condensed-Phase Entities, i, Immersed in Water,
w
73
1.
The AGiw2 Equation Pertaining to Two Different Entities,
1
and
2,
Immersed
in Water,
w
73
1.1.
AGiw2LW, or the
apolar
component of AGiw2
74
1.2.
AGiw2AB, or the polar component of AGiw2
74
1.3.
Possible role of AG]w2EL
75
2.
Examples of AGiW2 Interactions
75
2.1.
Hydrophobic attraction between a hydrophobic and a hydrophilic entity,
immersed in water
75
2.2.
Hydrophilic repulsion between different hydrophilic entities, immersed
in water
76
2.3.
Advancing freezing fronts, causing a repulsion or an attraction,
depending on the hydrophilicity or hydrophobicity of the immersed
particles, cells or macromolecules
78
2.4. Chromatographie
applications of hydrophobic interactions and their
reversal
81
2.5.
Polymer phase separation in water
81
3.
Water Treated as the Continuous Liquid Medium for AG]wi and AGiW2
Interactions
83
7.
Aqueous Solubility and Insolubility
85
1.
The Solubility Equation
85
1.1.
The contactable surface area (Sc)
86
1.2.
Contactable surface areas do not apply to spherical molecules or
particles
87
2.
Aqueous Solubility of Small Molecules
89
2.1.
Aqueous solubility of small non-ionic organic molecules
89
2.2.
Aqueous solubilities of inorganic salts
89
Contents
¡x
2.3.
Aqueous solubility of surfactants manifests itself as their critical micelle
concentration
(cmc)
91
3.
Aqueous Solubility of Polymeric Molecules
93
3.1.
Similarities between the aqueous solubility of polymer molecules and
the stability of particle suspensions in water
93
3.2.
Aqueous solubility of linear polymers
94
3.3.
Aqueous solubility of globular proteins
94
3.4.
Aqueous solubility of non-globular, fibrous proteins
96
3.5.
Aqueous solubility of gel-forming polymers
96
4.
Influence of Temperature on Aqueous Solubility
98
5.
Aqueous Insolubilization (Precipitate Formation) Following the Encounter
between Two Different Solutes that Can Interact with Each Other When
Dissolved in Water
98
5.1.
Classes of pairs of compounds that readily precipitate when
encountering each other in aqueous solution
98
5.2.
Mechanism of insolubilization upon the encounter of two different
compounds with opposing properties
99
5.3.
Mechanism of the formation of specifically impermeable precipitate
barriers
100
5.4.
Examples of specifically impermeable precipitate barriers or
membranes
101
5.5.
Single diffusion precipitation
109
8.
Stability Versus Flocculation of Aqueous Particle Suspensions
113
1.
Stability of Particle Suspensions in Water
113
1.1.
LW,
AB
and EL energies and the extended
DIVO
theory
114
2.
Stability of Charged and Uncharged Particles, Suspended in Water
117
2.1.
Role of attached ionic surfactants or electrically charged polymers
in conferring stability to aqueous particle suspensions
117
2.2.
Non-charged particles or particles of low charge stabilized by non-ionic
surfactants or polymers, via "steric stabilization"
118
3.
Linkage between the EL Potential and
AB
Interaction Energies in Water-
Importance of
AB
Interaction Energies for the Stability vs Flocculation Behavior
of Aqueous Suspensions of Charged Particles—
The Schulze-Hardy Phenomenon Revisited
123
3.1.
Mechanism of Schulze-Hardy type flocculation
123
3.2.
Linkage between changes in
ç-potential
and especially, changes
in the electron-donicity of polar surfaces, when immersed in water
126
4.
Destabilization of Aqueous Particle Suspensions by Cross-Linking
128
4.1.
Cross-linking of latex particles for diagnostic purposes—
The latex fixation test
128
4.2.
Cross-linking of human red blood cells with antibodies to cause
flocculation (hemagglutination) for blood group determinations
129
X The Properties of Water and their Role in Colloidal and Biological Systems
Section
С
Physical and Physicochemical Properties of Water
131
9.
Cluster Formation in Liquid Water
133
1.
Size of Water Molecule Clusters
133
1.1.
Measurement of the cluster size of water via its solubility in organic
solvents
133
1.2.
Variability as a function of temperature CO of the cluster size as well as
of the viscosity of water
134
1.3.
When water cluster size decreases with an increase in T, its Lewis acidity
increases and its Lewis alkalinity decreases
135
2.
Implications of the Increased Lewis Acidity of Water Following Increases in
Τ
135
2.1.
Consequences for the aqueous solubility of solutes and for the stability
of aqueous suspensions as a function of
Τ ΐ35
2.2.
Consequences for the attachment or detachment among two different
solutes and/or solids, immersed in water, as a function of
Τ
136
3.
Influence of Cluster Formation in Liquid Water on the Action at a Distance
Exerted by Polar Surfaces when Immersed in Water
137
3.1.
Connection between cluster size and the decay length of water
137
3.2.
The influence of cluster formation in liquid water on the XDLVO approach
pertaining to the stability of aqueous suspensions of human blood cells
139
10. Hydration
Energies of Atoms and Small Molecules in Relation to Clathrate
Formation
141
Preamble
141
1.
Free Energy of
Hydration
of Atoms and Small Molecules Immersed in Water
142
1.1.
The
AG™
part
142
1.2.
The AGww part
143
1.3.
AGjw and AGWW combined
143
2. Hydration
of Small
Apoiar
Molecules
144
3. Hydration
of Small Partly Polar Molecules
145
4.
Clathrate Formation as
a
Hydration
Phenomenon Occurring with Atoms or Small
Molecules
146
4.1.
The free energy of cohesion between the water molecules in liquid water
only contributes to the hydration energy of immersed atoms or small
molecules
146
4.2.
Influence of AGjwIF on larger molecules or particles, immersed in water
146
4.3.
Conclusion
147
4.4.
Alternative and simplified explanations
147
11.
The Water-Air Interface
149
1.
Hyperhydrophobicityofthe Water-Air Interface
149
1.1.
Causes of the hyperhydrophobicity of the water-air interface
149
Contents
1.2. Hyperhydrophobicity
of the water-air interface as the sole cause of the
increased value of the water contact angle when measured on rough
solid surfaces
151
1.3.
Hyperhydrophobicity of the water-air interface as the basis of flotation
as a separation method
152
2.
The f-Potentialof Air or Gas Bubbles in Water
152
3.
Repulsion versus Attraction of Various Solutes by the Water-Air Interface
153
3.1.
Determination of repulsion or attraction of solutes by the water-air
interface
153
3.2.
Repulsion of hydrophilic or near-hydrophilic solutes by the water-air
interface
154
3.3.
Solutes which comprise hydrophobic components are strongly attracted
to the water-air interface
158
4.
Inadvisability of Using Aqueous Solutions for the Measurement of Contact
Angles
160
12.
Influence of the
pH
and the Ionic Strength of Water on Contact Angles
Measured with Drops of Aqueous Solutions on Electrically Charged,
Amphoteric and Uncharged Surfaces
161
1.
Influence of the
pH
of Water on Electrically Charged and Amphoteric Surfaces
161
1.1.
Electrically charged surfaces
162
1.2.
Amphoteric surfaces
162
1.3.
Importance of the f-potential of simply electrically charged as well as of
amphoteric surfaces
162
2.
Influence of the
pH
on Water Contact Angles Measured on (Non-Charged)
Hydrophobic as Well as on (Non-Charged) Hydrophilic Surfaces
163
3.
Influence of the Ionic Strength on Water Contact Angles
164
3.1.
Low ionic strengths
164
3.2.
High ionic strengths
164
3.3.
Low concentrations of salts with
plurivalent
counterions
164
4.
Comparison Between the Influence of
pH
and Increases in Ionic Strength
on Water contact Angles on Solid Surfaces as well as on the Surface Properties
of such Solid Surfaces when Completely Immersed in Water
165
4.1.
Uncharged solids or solid particles
165
4.2.
Influence of
pH
or added salt on electrically charged solid surfaces,
particles or macromolecules
165
5.
Conclusions
166
13.
Macroscopic and Microscopic Aspects of Repulsion Versus Attraction
in Adsorption and Adhesion in Water
167
1.
Macroscopic-Scale Repulsion vs Microscopic-Scale Attraction in Water
168
1.1.
The adsorption of human serum albumin
(HSA)
onto metal oxide particles
immersed in water
168
xii
The Properties of Water and their Role in Colloidal and Biological Systems
2.
Methodologies Used in Measuring Protein Adsorption onto and Desorption
from Metal Oxide Particles in Water
171
2.1.
The continuous circulation device
171
2.2.
Determination of AG]w2(mac) and AGiw2(mic)
173
2.3.
Influence of the
pH
of the aqueous medium on protein adsorption and
desorption
173
2.4.
Other desorption approaches
174
3.
Hysteresis of Protein Adsorption onto Metal Oxide Surfaces, in Water
176
3.1.
Hysteresis'interference with the determination of Keq and k,j
176
3.2.
Hysteresis following hydrophilic adsorption
176
3.3.
Hysteresis following adsorption onto a hydrophobic surface
177
3.4.
Absence of hysteresis when adsorptive forces are purely electrostatic
177
3.5.
Hysteresis as a function of adsorption time
179
3.6.
Importance of using the value for pre-hysteresis
Кеч'^°
i8o
3.7.
Determination of K^1"*0
180
4.
Kinetics of Protein Adsorption onto Metal Oxide Surfaces Immersed in Water
181
4.1. Von Smoluchowski's
approach applied to the kinetic adsorption rate
constant, ka
182
4.2. Von
Smoluchowski's
f
factor
182
4.3.
Determination of
f
and
ψ
і8г
4.4.
The equilibrium binding constant and the kinetic rate constants
184
14.
Specific Interactions in Water
187
1.
Innate and Adaptive Ligand-Receptor Interactions in Biological Systems
187
1.1.
Specific innate ligand-receptor interactions
187
1.2.
Specific adaptive interactions
192
2.
The Forces Involved in Epitope-Paratope Interactions
196
2.1.
Mechanisms and outcomes of epitope-paratope interactions
196
2.2.
Roles of the three non-covalent forces
201
2.3.
Minor or dubious mechanisms of specific bond formation
204
REFERENCES
207
Subject Index
215 |
| any_adam_object | 1 |
| any_adam_object_boolean | 1 |
| author | Van Oss, Carel J. |
| author_facet | Van Oss, Carel J. |
| author_role | aut |
| author_sort | Van Oss, Carel J. |
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| building | Verbundindex |
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| ctrlnum | (OCoLC)229031857 (DE-599)GBV57211415X |
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| dewey-ones | 546 - Inorganic chemistry |
| dewey-raw | 546.22 |
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| dewey-sort | 3546.22 |
| dewey-tens | 540 - Chemistry and allied sciences |
| discipline | Chemie / Pharmazie Physik |
| discipline_str_mv | Chemie / Pharmazie Physik |
| edition | 1. ed. |
| format | Book |
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| id | DE-604.BV035069753 |
| illustrated | Illustrated |
| index_date | 2024-07-02T22:03:45Z |
| indexdate | 2024-07-09T21:21:30Z |
| institution | BVB |
| isbn | 9780123743039 0123743036 |
| language | English |
| oai_aleph_id | oai:aleph.bib-bvb.de:BVB01-016738148 |
| oclc_num | 229031857 |
| open_access_boolean | |
| owner | DE-703 DE-11 |
| owner_facet | DE-703 DE-11 |
| physical | XIV, 224 S. graph. Darst. 24cm |
| publishDate | 2008 |
| publishDateSearch | 2008 |
| publishDateSort | 2008 |
| publisher | Elsevier |
| record_format | marc |
| series | Interface science and technology |
| series2 | Interface science and technology |
| spelling | Van Oss, Carel J. Verfasser aut The properties of water and their role in colloidal and biological systems Carel Jan van Oss 1. ed. Amsterdam [u.a.] Elsevier 2008 XIV, 224 S. graph. Darst. 24cm txt rdacontent n rdamedia nc rdacarrier Interface science and technology 16 Surface chemistry Surfaces (Physics) Water Analysis Water Properties Hydrochemie (DE-588)4072678-2 gnd rswk-swf Hydrochemie (DE-588)4072678-2 s DE-604 Interface science and technology 16 (DE-604)BV019653877 16 Digitalisierung UB Bayreuth application/pdf http://bvbr.bib-bvb.de:8991/F?func=service&doc_library=BVB01&local_base=BVB01&doc_number=016738148&sequence=000002&line_number=0001&func_code=DB_RECORDS&service_type=MEDIA Inhaltsverzeichnis |
| spellingShingle | Van Oss, Carel J. The properties of water and their role in colloidal and biological systems Interface science and technology Surface chemistry Surfaces (Physics) Water Analysis Water Properties Hydrochemie (DE-588)4072678-2 gnd |
| subject_GND | (DE-588)4072678-2 |
| title | The properties of water and their role in colloidal and biological systems |
| title_auth | The properties of water and their role in colloidal and biological systems |
| title_exact_search | The properties of water and their role in colloidal and biological systems |
| title_exact_search_txtP | The properties of water and their role in colloidal and biological systems |
| title_full | The properties of water and their role in colloidal and biological systems Carel Jan van Oss |
| title_fullStr | The properties of water and their role in colloidal and biological systems Carel Jan van Oss |
| title_full_unstemmed | The properties of water and their role in colloidal and biological systems Carel Jan van Oss |
| title_short | The properties of water and their role in colloidal and biological systems |
| title_sort | the properties of water and their role in colloidal and biological systems |
| topic | Surface chemistry Surfaces (Physics) Water Analysis Water Properties Hydrochemie (DE-588)4072678-2 gnd |
| topic_facet | Surface chemistry Surfaces (Physics) Water Analysis Water Properties Hydrochemie |
| url | http://bvbr.bib-bvb.de:8991/F?func=service&doc_library=BVB01&local_base=BVB01&doc_number=016738148&sequence=000002&line_number=0001&func_code=DB_RECORDS&service_type=MEDIA |
| volume_link | (DE-604)BV019653877 |
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