bile salts form lyotropic liquid crystals
TRANSCRIPT
Bile salts form lyotropic liquid crystals
H. Amenitsch a,1, H. Edlund b,2, A. Khan c, E.F. Marques c,d, C. La Mesa e,*a Institute of Biophysics, Austrian Acad. Sci., University of Graz, Austria
b Department Chemistry Proc. Technol., Mid Sweden University, Sundsvall, Swedenc Department Phys. Chemistry I, University of Lund, Lund, Sweden
d Centro de Investigacao en Quimica, Dept. Chemistry, Faculty of Science, University of Porto, Porto, Portugale Department Chemistry, Universita Degli Studi di Roma La Sapienza, P. le Aldo Moro 5, Rome 00185, Italy
Received 28 January 2002; accepted 15 July 2002
Abstract
A reinvestigation of the phase diagrams relative to some conjugated and non-conjugated bile salts in water has
demonstrated the formation of lyotropic liquid crystalline phases, in contradiction with generally accepted statements.
The phase behaviour is complex and the phase diagrams are unusual, compared to most surfactants and lipids. In
particular, coexistence of liquid crystalline phases with crystals has been observed. The formation of liquid crystalline
phases requires very long equilibration times and the thermal stability of the lyotropic phases is moderate. The observed
structure is tentatively assumed to be of the reverse hexagonal type. Structural relations with currently accepted models
for the organisation of bile salts into micelles and solid form have been found.
# 2002 Elsevier Science B.V. All rights reserved.
Keywords: Bile salts; Micelles; Liquid crystals; Phase diagrams; NMR; SAXS
1. Introduction
Bio-compatible surfactants are the subject of
widespread interest, because of their possible use
in the formulation of pharmaceuticals and other
topics. Among many such agents, interest is
devoted to surfactants that are metabolic by-
products. Bile salts (BS) are extremely interesting
in this regard, being the main metabolites of the
cholesterol pool in vivo. Interest toward such
compounds is reflected from studies on their
solution properties [1�/6] and on the solvent
capacity with respect to sterols, glycerides and
lipids [7,8].
The peculiarity of BS as surface-active agents is
due to their molecular structure. Surfactants and
lipids show a clear separation between the polar
region (containing the head-group) and the non-
polar one (consisting of flexible long alkyl chains)
[9]. The hydrophobic part of BS, conversely,
consists of a non-planar, rigid, steroid ring con-
taining up to three hydroxyl groups [10]. The OH
* Corresponding author. Tel.: �/39-6-4991-3707; fax: �/39-6-
490-631
E-mail address: [email protected] (C. La Mesa).1 Provisional address: Department Chem. Eng., University
of Delaware, USA.2 Provisional address: SAXS Beam-line at Elettra, Basoviza,
Trieste, Italy.
Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92
www.elsevier.com/locate/colsurfa
0927-7757/02/$ - see front matter # 2002 Elsevier Science B.V. All rights reserved.
PII: S 0 9 2 7 - 7 7 5 7 ( 0 2 ) 0 0 3 6 0 - 6
groups lie in the same plane and the steroid ring,
thus, bears polar and non-polar sides, as indicated
in Fig. 1. In addition, naturally occurring bile
acids are conjugated with amino-acids such as
taurine and glycine, through a peptide bond; hence
the name tauro, or glyco, derivatives.
The rigidity and two-faced character of BS
imply that their packing into supra-molecular
structures does not follow the conventional fea-
tures peculiar to surfactant aggregation. Several
supra-molecular association models were pro-
posed [11�/13] and even the definition of BS
micelles was questioned for a long time [14,15].
BS aggregate and form micelles of small aggrega-
tion numbers, typically Nagg:/2�/10, which may
noticeably increase as a function of concentration
and/or added electrolyte [5,6,11,16]. In some caseslarge BS micelles are formed by a helical arrange-
ment of steroid units [17,18]. In the NaDC�/water
system, for instance, fibre-like structures can be
drawn from concentrated micellar solutions
[19,20].
BS are incorporated into liquid crystalline
phases [21�/23], but no liquid crystalline phases
in water have been observed up to now. This facthas been rationalised as an example of their
peculiar associative behaviour. According to an
authoritative scientist ‘‘. . .conjugated and free BS
form micelles, but not liquid crystals. . .’’ [24].
Indeed, BS form liquid crystalline phases in water
[25,26].
The occurrence, width and thermal stability of
such phases depend on: (i) the nature of the polarhead group; (ii) the number and position of OH
groups in the steroid skeleton; (iii) temperature;
(iv) concentration, and (v) ionic strength.
The formation of lyotropic mesophases in BS�/
water systems is peculiar. The structure of the
phases, the macroscopic phase appearance, the
observed phase sequence and the equilibrium
conditions between coexisting phases are signifi-cantly different from those observed in systems
containing surfactants and/or lipids [9,27].
The present investigation is focused on the
phase behaviour of binary mixtures containing
water and sodium tauro-cholate (NaTC), sodium
tauro-deoxycholate (NaTDC), sodium tauro-che-
nodeoxycholate (NaTCDC), sodium glyco-deox-
ycholate (NaGDC), and sodium deoxycholate(NaDC). The majority of such compounds have
two OH groups facing outwards from the steroid
nucleus. The cheno-deoxy derivative differs from
the deoxy ones in the position of OH groups: aC-3
and aC-7, compared to aC-3 and aC-12. Tauro-
cholate has three hydroxyl groups, in aC-3, aC-7
and aC-12 positions, respectively.
The packing of BS into organised lyotropicmesophases is the subject of this study. Some
results on the above systems, the ones relative to
optical polarising microscopy and preliminary
small angle X-ray scattering data (SAXS), have
been reported elsewhere. Here we report on more
recent findings and discuss some aspects which
have not yet been considered in detail. We focus
Fig. 1. Chemical structure of cholanic acids, indicating the
position of OH groups in 3a, 7a and 12a, in the top. The front
view and cross-section of BS anions are schematically reported
in the lower part of figure.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9280
on the thermal stability of the phases and on linksbetween current models proposed for the forma-
tion of BS micelles and structure of the lyotropic
phases.
Apart from interest on a biologically relevant
subject, there are practical consequences of BS
organisation in mesomorphous phases, which
imply the use of such liquid crystalline matrices
in the topical administration of pharmaceuticals.
2. Experimental section
2.1. Materials
Basel, Switzerland, supplied D2O, 99.95% iso-
topic purity. Conductivity water (k close to 1 mS,at 25 8C) was used.
Mono-hydrate NaDC, nominal purity �/99%;
NaTC �/97%; emi-hydrate NaTDC �/97%;
NaTCDC, high purity; and NaGDC, containing
1.5 mol H2O/mol �/98%, were from Aldrich.
According to conductivity and surface tension
experiments, the samples are appreciably pure and
have critical micellar concentration values (cmc),very close to those reported in the literature [11].
The pH of BS solutions does change much with
composition. In particular, the pK of tauro (and
glyco) derivatives of bile acid salts is close to 2 [28].
In the case of NaDC, some evidence of hydrolysis
was observed at very low concentrations [29].
Perhaps, use of Tris, phosphate or other buffers
in studies on BS in solution has been questioned,because of the hydrophobic character of hydro-
xymethyl aminomethane ion and, more generally,
of the ionic strength effect on cmc values, micelle
aggregation numbers and counter-ion binding
[30�/33]. In other words, buffers stabilise the
hydrolysis, but have a non-negligible effect on
micelle size and shape, and, presumably, on the
phase diagram.
2.2. Sample preparation and phase diagram
determination
The samples were prepared by weight into glass
tubes, which were flame-sealed and mixed by
centrifugation. They were allowed to stay at
50 8C for, at least, 2 days. Thereafter they wereequilibrated at 20 8C for several weeks. Prelimin-
ary studies of the phase behaviour involved the
inspection between crossed Polaroids.
2.3. Polarised light microscopy
An Axioplan Universal polarising light micro-
scope (Zeiss) equipped with a SITC video-cameraand image processor Argus-20 (Hamamatsu
Photonics, Japan) was used. The microscope is
equipped with a hot stage, operating from 0 to
100 8C. Additional experiments were performed
with a Ceti optical polarising microscope,
equipped with an ME Super camera (Pentax)
and a Linkam unit, TP93, equipped with an HFS
91 heating stage (Linkam). Samples to be investi-gated as a function of temperature were sealed in
thin glass capillaries or between glass sheets for
optical microscopy.
2.4. Electrical conductance
A Wayne-Kerr bridge, mod.6425, was used. An
immersion-type conductivity cell was merged inthe sample, previously melted, and the system was
equilibrated at 20 8C for the required time. The
samples were located into a Hetofrig CB IIe
thermostatic unit and the thermal scan speed was
set at 0.1 (or 0.03) 8C min�1. Phase transitions
were inferred from significant changes in slope in
the conductivity versus temperature plots [34].
More precisely, the transition temperature is thepoint at which (@k /@T ) is a maximum and (@2k /
@T2)�/0.
From ionic conductivity the width of the two-
phase region can also be evaluated. It can be
demonstrated that such quantity is related to the
projection on the temperature axis of the segment
connecting the two branches of the curve. A
significant thermal hysteresis (over 10 8C, insome instances) was observed on cooling.
2.5. Adiabatic compressibility
Density, r , was measured by an Anton Paar
DMA 60 unit [35]. The uncertainty on such values
is to 5�/10�6 g cm�3 when the temperature is
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 81
constant to 9/0.003 8C. Sound velocity, v (in cms�1), was measured at 5 MHz by a 2 cm3 home
built resonant cell, connected to a Matec 750 unit.
The uncertainty on sound velocity values is in the
range 0.5�/1 m s�1. The accuracy on adiabatic
compressibility values, b�/(rv2)�1, is better than
0.01% of the measured value. Details on the
experimental set-up and measuring procedures
are reported elsewhere [36].
2.6. Small angle X-ray scattering (SAXS)
Measurements were carried out in a Kratky
system, equipped with a position-sensitive detec-
tor, containing 1024 channels of width 53 mm. A
Cu�/Ka radiation of wavelength 0.1542 nm was
used and the sample-to-detector distance was fixedto 277 mm. The samples were located in a paste
holder between thin mica windows. The tempera-
ture in the camera was regulated by a Peltier
element (to 9/0.1 8C) and the chamber was kept
under vacuum, to minimise air scattering. Addi-
tional experiments, including those performed as a
function of temperature, were performed at the
SAXS Beam-line in Elettra, Trieste [37].
2.7. 2H (deuterium) quadrupolar splitting
2H has a spin quantum number I�/1 and
possesses an electric quadrupole moment. In
anisotropic liquid crystalline phases the interaction
of the quadrupole moment with the electric field
gradients is not averaged to zero and gives rise to a
splitting. The magnitude of the 2H quadrupolesplitting depends on the phase anisotropy. In poly-
phasic systems, the spectrum is a superposition of
those of the individual phases.
In lyotropic systems, water binds to the surfac-
tant head-group. In fast exchange regime between
the free state and the binding sites a linear relation
between splitting and solute volume fraction is
obtained, from which hydration and phase struc-ture are inferred [38].
Spectra were recorded at 41.45 MHz in a JEOL
FX 270 pulsed FT NMR spectrometer. A control
unit regulates the temperature to 9/0.2 8C. The
samples were equilibrated for long periods (usually
around 40 min), to avoid the occurrence of
temperature gradients. Spectra were repeated untilno changes were observed. In some instances up to
several weeks were required to get constant quad-
rupole splitting values. In all cases we have
investigated, the deuterium quadrupole splitting
does not give powder pattern spectra.
2.8. Pulsed field gradient (PFG) NMR self-
diffusion
The PFG technique is based on the combination
of a radio-frequency (rf) sequence and applied
magnetic field gradient pulses. The sequence con-
sists of two rf pulses (a 908 and a 1808 one) and
two gradient pulses with time duration d and
separation D between their leading edges. They are
located on either side of the 1808 rf pulse. The self-diffusion coefficient is determined by the decay of
a FT signal (at the centre of the echo attenuation)
as a function of the strength, or duration, of the
gradient pulse [39].
Measurements were performed by a Bruker
DMX200 spectrometer, at 200 MHz, with a probe
providing a maximum field gradient of 9 T m�1.
The accuracy on self-diffusion findings is to 9/2%of the measured value.
3. Results
3.1. Phase diagrams
The phase diagrams were constructed by visual
observation, optical polarising microscopy, NMRmethods, electrical conductance and SAXS. A
univocal assignment of the different phases and
the definition of the width of the two-phase
regions is not straightforward. In that sense, the
polymorphic character of BS is still elusive.
The kinetics of liquid crystal formation is slow.
Days to months are required to observe the
formation of liquid crystalline matter, in properexperimental conditions. The kinetics of meso-
phase nucleation depend on temperature. For
instance, in the water�/NaTDC system, the forma-
tion of anisotropic phases occurs in 3 days when
the samples are kept at 20 8C and about 2 days at
25 8C. The effect is reproducible.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9282
An overview to the phase diagrams, reported in
Fig. 2(a�/e), indicates that the formation of a
solution region, as well as of anisotropic liquid
crystalline phases, is ubiquitous. Regions with
hydrated crystals are also observed in all systems.
Differences concern the region of existence of the
phases, the width of the two-phase regions, the
thermal stability and the kinetics of phase forma-
tion.
The two-phase region on the left-hand side of
the liquid crystalline phase in the water�/NaTDC
system has some remarkable features. Some sam-
ples are lyotropic dispersions, in others a weakly
anisotropic upper phase, forming in some days, is
Fig. 2. Temperature versus weight percent phase diagrams for different bile sodium salt�/water systems. In (a) the NaTCDC�/water,
(b) the NaTDC�/water one, (c) the NaGDC�/water system, (d) the NaDC�/water, and (e) the NaTC�/water system.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 83
observed. From this phase, spherulitic crystals
grow and sediment. With time crystals begin
coming into the upper phase. Finally, the liquid
crystalline phase is formed. The kinetics of phase
transformation is sketched in Fig. 3. Each transi-
tion requires hours to days and the kinetic scheme
is reproducible.NaTC�/H2O and NaTDC�/H2O systems show
well-defined phase boundaries, with occurrence of
single and two-phase regions. NaTDC samples
display a monochromatic weak birefringence be-
tween crossed Polaroids. The NaDC�/H2O,
NaCDC�/H2O and NaGDC�/H2O systems, con-
versely, show a more complex phase behaviour,
with occurrence of a narrow liquid crystalline
region. In the case of the NaDC�/H2O system
some hydrolysis may occur [29]. This effect,
perhaps, is traceless in the phase behaviour. In
terms of the phase rule, in fact, the NaDC�/H2O
system is to be considered a two-component
system even in the presence of a reaction betweenthe components.
A wide two-phase region is present in all cases.
In some weeks, single-phase anisotropic samples
are formed. No such effects have ever been
reported in surfactants, or lipids. The coexistence
of crystals with micellar solution and/or lyotropic
phases and the slow kinetics of phase transforma-
tion are peculiar to all BS investigated here.Some comments need to be made:
(i) The formation of transient spherulitic crys-tals is common to all BS. It can be ascribed to
the occurrence of meta-stable liquid crystallites
or to nucleation processes, required for the
formation of the liquid crystalline phases.
(ii) The thermal stability of the mesophases is
moderate. The most stable liquid crystalline
phase, the one observed in the NaTDC�/water
system, disappears at temperatures close to35 8C (Fig. 4). In all systems, a significant
thermal hysteresis is observed on cooling.
(iii) The isotropic phase observed at concentra-
tions above the liquid crystal one is assumed to
be, in a first approximation, a micellar solution.
Such viscous isotropic phase (flowing under
gravity) is always in equilibrium with crystals.
Samples in this region resemble cubic liquidcrystalline phases in their consistency and
macroscopic phase behaviour. The possibility
of the occurrence of an isotropic liquid crystal-
line phase cannot be ruled out, but efforts to get
single-phase samples were unsuccessful.
(iv) Optical polarising microscopy textures in-
dicate that the size of the lyotropic crystallites
(domains) is small [25,26,40].
3.2. Self-diffusion
NMR self-diffusion measurements were per-
formed in the NaTC�/water and NaTDC�/water
systems, representative of tri-hydroxy and di-hydroxy salts, respectively. Water self-diffusion
in the two systems is nearly the same (Fig. 5) when
the surfactant self-diffusion is markedly different,
as indicated in the lower part of Fig. 5. Self-
diffusion values of NaTDC are systematically
lower than those of NaTC.
Fig. 3. The kinetics of phase transformation in BS�/water
systems, at :/20 8C. The kinetic processes reported in the
scheme can be long days, in NaTC�/H2O and NaTDC�/H2O
mixtures, or months, in the NaDC�/water system.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9284
In the concentration range we have investigated
(well above the cmc) the monomer contribution to
the overall self-diffusion is negligible [41]. In fact,
the observed self-diffusion is a weight average
contribution of molecular and micellar species,according to [42,43]
Dexpt�Dmon(CMC=Ctot)
�Dmic(Ctot�CMC=Ctot) (1)
where Dmon and Dmic indicate the self-diffusion of
molecules and micelles, respectively.
[N.B. At low surfactant content, BS form
dimers, trimers, etc, in considerable amounts,
depending on the number and position of the
OH groups in the steroidal skeleton [18]. In that
case Dexpt�/(1/Ctot) Si�1DiCi , which reduces tothe two-site approximation in Eq. (1) at high
surfactant content.]
In the present experimental conditions, c �/cmc,
we can safely assume that the observed values are
ascribed to micelle diffusion. Self-diffusion values
of NaTDC micelles are systematically lower than
those of NaTC ones. Estimates of the solute
hydrodynamic radius were made through theStokes�/Einstein equation. At about 0.4 molal
BS, (approximately 20 wt% of the steroidal
surfactant), NaTDC micelles have hydrodynamic
radius of 39 nm, when NaTC ones are only 5.4.
Accordingly, di-hydroxy BS micelles grow much
more steeply than tri-hydroxy ones. Sodium cho-
late, for instance, forms smaller micelles than
deoxy- and chenodeoxycholate, and NaTDC
shows a pronounced micellar growth compared
to NaTC [11,16].
3.3. Liquid crystal formation
Optical anisotropic textures were observed bypolarising microscopy, as mentioned above. In
some instances, battonets and striated
non-geometric textures appear. The NaGDC�/
H2O system shows weakly birefringent and ill-
defined textures of the non-geometric, non-striated
type [40].
Attempts to separate the spherulitic crystals
occurring in biphasic samples were made and giantfibrous structures are observed when the bottom
phase is separated from the isotropic solution. In
some instances non-geometric and non-striated
textures are mixed with fibre-like ones. Blow and
Rich described optical textures indicating the
occurrence of helical-based fibres [19,20]. We do
not know, at this stage, whether the structure of
the liquid crystalline phase is directly related tosuch fibres.
A strong similarity has been observed by some
of us between such textures and those of fibres
drawn from concentrated micellar solutions [44].
Due to the small size of the lyotropic textures,
mentioned above [25,26], it is not easy to give a
Fig. 4. Electrical conductance, k (mS), versus temperature, in 8C, for a 46.7 wt. NaTDC�/water mixture (^), and for a 58.4 wt.
NaTC�/water one (k). The coexistence of solution and liquid crystalline phases occurs in the region where a steep decrease of
conductivity is observed. The slope of k of as a function of T is nearly the same in solution and in liquid crystalline phase. A significant
thermal hysteresis, indicated by the dotted line, is observed on cooling.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 85
univocal phase assignment solely from optical
polarising microscopy. That is why many experi-
mental methods are required to characterise such
systems.
In two-phase regions the 2H NMR quadrupole
splitting superimposes isotropic signals. In single
phase regions most samples show broad lines (Fig.
6), but splitting is small, if any. This might be due
to the very small bond order parameter of hydra-
tion water [42,43,45], i.e. to a small anisotropy.
The signal width indicates also that fast exchange
conditions between free and bound water are not
fulfilled, presumably because the lyotropic micro-
domains are small. This hypothesis is in good
agreement with optical polarising microscopy
findings.
We do not consider, in this context, exchange
between OH (or NH) protons and water deuter-
ons. If present, they should give rise to large
quadrupole splitting effects, several kHz wide,
which are not observed in the present experimental
conditions. Please note that the very small quad-
Fig. 5. (a) Water self-diffusion, m2 s�1, as a function of BS weight percent in the NaTC�/water system (^), and in the NaTDC�/water
one (k), at 20 8C. (b) The BS self-diffusion, m2 s�1, in the NaTC�/water (k), and NaTDC�/water system (^), as a function of BS
weight percent, at 20 8C. Data are in logarithmic scale.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9286
rupole splitting reported here (some hundred Hz
wide) rules out such possibility.
Structural length scales in lyotropic liquid
crystals are in the range 1�/50 nm and SAXS, or
SANS, can be used. Phases possessing long-range
order, (lamellar, hexagonal, cubic etc.), show well
defined Bragg peaks. A hexagonal phase, for
instance, is built up of long cylinders packed in a
2-D hexagonal array [46]. The Bragg peaks posi-
tion of the hexagonal phase is 1, �3, �4, �7, �9,
corresponding to the (10), (11), (20), (21) and (30)
(hk) reflections, respectively. The hexagonal cylin-
der radius and the interfacial area per molecule
can be calculated from the main spacing, taking
into account the solute volume fraction [27,47].
Diffraction patterns observed in the NaTDC�/
water system (1:1.73:1.89) are close to those
expected for hexagonal phases. Up to five reflec-
tions were observed, with peaks in the order
1:1.75:2.00:2.77:3.09. A selected example of
small-angle scattering findings is reported in Fig.
7.
A few SAXS results are reported in Table 1. As
can be seen there, the spacing is consistent, in a
first order approximation, with a hexagonal order,
or a tetragonal (distorted hexagonal) one. It has
been recently demonstrated that structures in solid
NaTDC and in the corresponding fibres are not
perfectly monoclinic [48]. The same behaviour
could also be observed in liquid crystalline phase
and could be partly responsible for departures
from the typical hexagonal structure. It is well
known, in this regard, that the structure of liquid
crystalline phases made up by rod-like aggregates
may show differences from the canonical hexago-
nal behaviour, depending on composition, struc-
ture of the surfactant, etc. [9,27].
Fig. 6. 2H NMR spectra of heavy water, at 15 8C, for NaTCDC�/D2O, (58.1, 63.2 and 65.2 wt., from the top), left, NaDC�/D2O,
(30.0, 32,8, 34.6 wt. from the top), centre, and NaGDC�/D2O systems, (39.2, 41,1, 40.8 and 43.2 wt., from the top). A bar 500 Hz wide
indicates the quadrupole splitting.
Fig. 7. SAXS patterns, reporting the signal intensity, I , in
arbitrary units, versus q , in A�1, for a 47.3 wt. NaTDC�/water
sample, at 25 8C. The patterns remain nearly constant up to the
phase transition temperature, about 35 8C.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 87
Attempts to calculate area per molecule from X-
ray findings were made. The most reasonable
values were obtained by assuming the hexagonal
liquid crystalline phase to be of the reverse kind.
Strong support in favour of this tentative assign-
ment comes by the fact that no voids in the rods
are possible in the case of reverse hexagonal
phases. It must be kept in mind, in this regard,
that it is difficult to pack the steroidal skeleton of
BS into conventional micelles, either spheres or
rods.
The tentative hypothesis we suggest can be
considered quite exotic. Perhaps it finds support
in some models proposed by Giglio and co-work-
ers [49�/51]. According to his suggestions, long
rod-like aggregates based on a helical arrangement
of BS may form in solution. It is obvious to
forecast the formation of anisotropic structures
when the concentration of micellar surfactant
exceeds a certain value.
SAXS and NMR data, thus, indicate the
occurrence of non-conventional aggregates. The
observed spacing bears structural connections with
the long rod-like aggregates and fibres, for which a
helical arrangement has been proposed [19,20,49�/
51]. Keeping in mind the location in the phase
diagram, we assume the occurrence of reverse
phases, formed by water cylinders arranged in a
non-polar continuum (Fig. 8). This is in fair good
agreement with what is stated above. In addition,
recent findings by some of us show the occurrence
of some links between the size of micelles, crystals,
fibres and liquid crystalline rods [44].
According to X-ray diffraction, NaTC has the
smallest cylinder radius and the largest interfacial
area per molecule (0.65 nm2), as is to be expected
from the presence of three OH groups (Table 1).
NaTCDC has a large interfacial area compared to
other di-hydroxy salts, because the OH groups in
aC3 and aC7 do not pack as tightly as those
located in aC3 and aC12 positions. The trend
observed from interfacial areas, NaTC�/
NaTCDC�/NaTDC]/NaDC, is in agreement
with the salt solubility sequence.
Table 1
SAXS measurements in liquid crystalline samples of selected BS�/water systems, at 20 8C
Salt Weight percent Spacing (A)a Nearest-neighbour distance (A) Cylinder radius (A) Area per molecule (A2)
NaTC 59.9 37.0 42.7 16.3 65
NaTDC 40.0 51.5 59.5 26.3 40
NaTCDC 43.6 41.9 48.4 20.9 51
NaDC 39.1 46.9 54.2 23.4 45
N.B. Areas were calculated assuming a reverse hexagonal structure. The dependence on composition is moderate.a Obtained from the (100) reflection.
Fig. 8. Arrangement of BS into a reverse hexagonal structure.
In the top is reported the structure of the cylinders, below the
top view of the aggregates. Cylinders can be tilted with respect
to the z -axis or may be arranged in a tetragonal (distorted
hexagonal) structure. The area indicated by a dotted arrow
indicates the preferred orientation of the polar regions in the
aggregates.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9288
Temperature has a puzzling effect on spacings.
According to Luzzati [46], the spacing regularly
decreases with T . In the NaTDC system, con-
versely, the spacing increases, or decreases, with
temperature, depending on composition, i.e. on
the sample location in the phase diagram. In other
words, liquid crystalline phases swell, or shrink,
depending on composition. In the case of the
NaTDC�/water system, for instance, swelling is
observed at relatively low concentration, close to
the micellar solution side.
The ionic conductivity of liquid crystalline
phases increases with temperature (Fig. 4). The
slope of k (T ) is nearly the same in liquid crystal
and in solution phase. This implies that ion
transport mechanisms in liquid crystalline and
solution phases are nearly the same. In the
water�/NaTDC system the transition temperature
from liquid crystalline to solution phase is 35 8C(Fig. 4) or lower. Presumably, such transition is
related to physiological requirements, to circum-
vent dis-metabolic diseases.
Adiabatic compressibility measurements, per-
formed in concentrated BS micellar solutions
(Fig. 9), indicate the occurrence of significant
changes in the solution structure at about 35 8C.
The effect may be ascribed to the collapse of
hydrogen bonding networks or to a significant
reduction of hydrophobic interactions at physio-logical temperatures.
3.4. Molecular packing
The formation of supra-molecular aggregates is
ubiquitous in aqueous BS systems. Very peculiar
packing modes into micelles, fibres, liquid crystalsand solid form have been observed and proposed
[12,14,18,44]. In water BS form micellar aggre-
gates, becoming progressively anisometric on in-
creasing the surfactant concentration and/or the
medium ionic strength. Generally, such aggregates
are formed by a helical arrangement of BS anions
and are stabilised by intermolecular hydrogen
bonding [49]. Significant differences have beenobserved between aggregates formed by di- and
tri-hydroxy BS, respectively. The latter, usually,
form small aggregates. It has been demonstrated
also that BS packing at polar�/apolar interfaces in
mixed micelles is perpendicular for di-hydroxy and
flat for tri-hydroxy salts, respectively [52].
If NaTDC micelles are larger and grow faster
with concentration than NaTC ones, the forma-tion of liquid crystalline phases should obey the
same rules, as, indeed, is observed. As to the
packing in liquid crystalline form, slight differ-
ences have been found between the different
Fig. 9. Dependence of adiabatic compressibility, b , in g�1 cm s2, on temperature, in 8C, for 35.7 wt. NaTC mixtures. The
discontinuity occurs at T values close to the phase transition temperature observed in the adjacent liquid crystalline phase.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 89
systems. Similarities can also be found betweenpacking in solid and in liquid crystalline form.
4. Discussion and conclusions
BS form liquid crystalline phases in water.
Attempts to rationalise the observed behaviour
can be made on the basis of the salt solubility
sequence, in turn dependent on chemical structure.Tri-hydroxy salts are more soluble than di-hy-
droxy ones and taurine (or glycine) conjugates
more soluble than free salts. Cheno-deoxy deriva-
tives are slightly more soluble than deoxy ones. All
these observations are reflected in the cmc and in
the maximum solubility limit in micellar form. The
observed sequence is TC�/TCDC:/GDC�/
TDC�/DC. The width of the mesomorphousphase for the di-hydroxy salts, conversely, is in
the order TDC�/TCDC�/GDC:/DC. On these
grounds, an increasing head-group hydrophilicity
favours the formation of liquid crystalline phases.
The effect played by the number and position of
OH groups in the phase behaviour is considerable.
Changing the OH group position from aC-12 to
aC-7, for instance, implies a lower thermal stabi-lity of the lyotropic phase. In general, the chemical
structure of BS plays an intricate role in the
aggregation processes, since it is related to the
packing peculiarities of the different BS. This is
not surprising, since electrostatic, hydrophobic
and intermolecular hydrogen bond interactions
play a role in the structure of micelles and,
consequently, in the self-assembly of aggregatesforming liquid crystalline phases.
The thermal stability of such liquid crystalline
phases is small and a weak Gibbs energy difference
between the isotropic solution and the liquid
crystal phase is expected. The thermal stability of
the liquid crystalline phases increases with increas-
ing the hydrophilic character of the head-group.
This fact can be put in evidence by relating thebehaviour predicted by the above lyotropic scale
to the width of the liquid crystalline phases for the
different phase diagrams.
The kinetics of phase transformation can vary
significantly from system to system. Birefringent
textures form in 1�/3 days in the NaTDC�/water
system, but months are required to get the sameresults in the NaDC�/water one. The very long
time required to have equilibrium structures is a
qualitative indication that the difference in ther-
modynamic stability between the different states of
organisation is small.
The formation of anisotropic textures from the
dispersed solid and the occurrence of transient
spherulitic crystals is common in all BS�/watersystems. Such unconventional nucleation effects,
the long equilibration times and the puzzling
temporal sequence of phase transformations,
may have led most authors to circumvent the
occurrence of liquid crystalline phases.
The liquid crystalline phases are, presumably,
built up of reverse micellar aggregates. Structural
links between the reverse hexagonal phase and therod-like helical aggregates proposed for the iso-
tropic phase are reasonable. Above the liquid
crystal phase border extremely viscous phases
occur; it is not easy to ascertain whether they are
true solutions or else.
Some remarks need to be made on the coex-
istence of solid with liquid crystalline phases.
Lyotropic liquid crystals formed by soaps, surfac-tants and lipids require a liquid-like state of the
flexible chains [53]. Obviously, this statement does
not hold for BS. It is difficult to reconcile the
proposed organisation of bile acid salts in terms of
structures proposed for surfactants and lipids.
Comparison could be made with zwitterionic
surfactants having a steroidal nucleus as hydro-
phobic group. It is well known, in this regard, thatCHAPS and CHAPSO aggregate in stacks [54],
but no evidence of liquid crystal formation is
available.
Let us compare the behaviour of BS with a class
of planar molecules forming lyotropic phases, the
chromonics (a family of substances including
drugs, dyes and some antibiotics) [55]. They
consist of aromatic ring structures, with polargroups facing from the ring, i.e. polar and non-
polar regions are not clearly separated. In terms of
the lyotropic behaviour, thus, BS occupy an
intermediate position between chromonics and
flexible alkyl chain surfactants.
According to the present findings, liquid crystal
formation does not imply any particular physical
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9290
state for the molecule. It is the occurrence ofpositional order of (and in) the domains which
determines the occurrence of liquid crystalline
order for BS.
Acknowledgements
The Swedish Research Council for Engineering
Sciences (TFR) and PRAXIS XXI, Portugal
(project 2/2.1/QUI/411/94) are acknowledged for
financial support. C.L.M. thanks the Departmentof Physical Chemistry 1, at Lund, for a Visiting
Professorship. The administration of SAXS Beam-
line at Elettra is acknowledged for time machine
facilities. Thanks are due to Professor Edoardo
Giglio, La Sapienza University, for suggestions on
the structural relations between SAXS data of
liquid crystalline phases and X-ray diffraction
observed in solution, in solid form or in fibres.
References
[1] P. Ekwall, L. Sjoblom, Acta Chem. Scand. 3 (1948) 1179.
[2] P. Ekwall, J. Colloid Sci. 8 (1954) 66.
[3] K. Fontell, Kolloid-Z. u. Z. Polym. 244 (1971) 246.
[4] K.J. Mysels, Hepatology 4 (1984) 80S.
[5] J.P. Kratohvil, Adv. Colloid Interface Sci. 26 (1986) 131.
[6] J.P. Kratohvil, W. Hsu, D.I. Kwok, Langmuir 2 (1986)
256.
[7] M.C. Carey, D.M. Small, Am. J. Med. 49 (1970) 590.
[8] B. Borgstrom, Int. Rev. Physiol. 12 (1977) 305.
[9] G.J.T. Tiddy, Phys. Rep. 57 (1980) 1.
[10] D.M. Small, in: P.P. Nair, D. Kritchevsky (Eds.), The Bile
Acids, Plenum Press, New York, 1971.
[11] M.C. Carey, D.M. Small, Arch. Intern. Med. 132 (1972)
506.
[12] D.G. Oakenfull, L.R. Fisher, J. Phys. Chem. 82 (1978)
1838.
[13] Y. Murata, G. Sugihra, K. Fukushima, M. Tanaka, J.
Phys. Chem. 86 (1982) 4690.
[14] A. Roda, A.F. Hofmann, K.J. Mysels, J. Biol. Chem. 258
(1982) 6362.
[15] P. Mukerjee, K.J. Mysels, Critical Micelle Concentration
of Aqueous Surfactant Systems, (NSRDS-NBS 36), US
Govt. Printing Office, Washington, DC, 1971.
[16] N.A. Mazer, M.C. Carey, R.F. Kwasnick, G.B. Benedek,
Biochemistry 18 (1979) 3064.
[17] A.R. Campanelli, S. Candeloro De Sanctis, E. Chiessi, M.
D’Alagni, E. Giglio, L. Scaramuzza, J. Phys. Chem. 93
(1989) 1536.
[18] E. Bottari, M.R. Festa, Langmuir 12 (1996) 1777.
[19] A. Rich, D.M. Blow, Nature 182 (1958) 423.
[20] D.M. Blow, A. Rich, J. Am. Chem. Soc. 82 (1960)
3566.
[21] C. La Mesa, A. Khan, K. Fontell, B. Lindman, J. Colloid
Interface Sci. 103 (1985) 373.
[22] M. Svard, P. Schurtenberger, K. Fontell, B. Jonsson, B.
Lindman, J. Phys. Chem. 92 (1988) 2261.
[23] M. Swanson-Vethamuthu, M. Almgren, B. Bergenstahl, E.
Mukhtar, J. Colloid Interface Sci. 178 (1996) 538.
[24] D.M. Small, J. Colloid Interface Sci. 58 (1977) 581.
[25] H. Edlund, A. Khan, C. La Mesa, Langmuir 14 (1998)
3691.
[26] E. Marques, H. Edlund, C. La Mesa, A. Khan, Langmuir
16 (2000) 5196.
[27] P. Ekwall, in: G.H. Brown (Ed.), Advances in Liquid
Crystals, vol. I, Academic Press, New York, 1975.
[28] N. Kallay, M. Colic, V. Simeon, J.P. Kratohvil, Croatica
Chem. Acta 60 (1987) 555.
[29] B. Sesta, P. Pandolfi, Ber. Bunsen-Ges. Phys. Chem. 91
(1987) 7.
[30] M. Vadnere, R. Natarajan, S. Lindenbaum, J. Phys.
Chem. 84 (1980) 1900.
[31] N. Rajagopalan, M. Vadnere, S. Lindenbaum, J. Solution
Chem. 10 (1981) 786.
[32] G. Sugihara, K. Yamakawa, Y. Murata, M. Tanaka, J.
Phys. Chem. 86 (1982) 2784.
[33] J.P. Kratohvil, Adv. Colloid Interface Sci. 26 (1986)
131.
[34] C. Charbit, F. Dorion, R. Gaboriaud, Fluid Phase Equil.
20 (1985) 233.
[35] C. La Mesa, B. Sesta, J. Phys. Chem. 91 (1987) 1450.
[36] C. La Mesa, L. Persi, A. D’Aprano, Ber. Bunsen-Ges.
Phys. Chem. 102 (1998) 1459.
[37] P. Laggner, H. Amenitsch, M. Kriechbaum, G. Pabst, M.
Rappolt, Faraday Disc. 111 (1998) 31.
[38] B. Lindman, P. Stilbs, in: S. Friberg, P. Bothorel (Eds.),
Microemulsions, CRC Press, Boca Raton, FL, 1986.
[39] P. Stilbs, Prog. Nucl. Magn. Reson. Spectrosc. 19 (1987) 1.
[40] F.B. Rosevear, J. Am. Oil Chem. Soc. 31 (1954)
628.
[41] O. Regev, K. Kang, A. Khan, J. Phys. Chem. 98 (1994)
6619.
[42] B. Lindman, O. Soderman, H. Wennerstrom, in: R. Zana
(Ed.), Surfactant Solutions. New Methods of Investiga-
tion, Marcel Dekker, New York, 1986.
[43] R.L. Thurmond, G. Lindblom, M.F. Brown, Biophys. J.
60 (1991) 728.
[44] L. Galantini, E. Giglio, C. La Mesa, N.V. Pavel, F. Punzo,
Langmuir 18 (2002) 2812.
[45] W.S. Price, Concepts Magn. Res. 9 (1997) 299.
[46] V. Luzzati, H. Mustacchi, A.E. Skoulios, F. Husson, Acta
Crystallogr. 13 (1960) 660.
[47] K. Fontell, Mol. Cryst. Liq. Cryst. 63 (1982) 59.
[48] E. Giglio, private communication.
[49] E. Giglio, S. Loreti, N.V. Pavel, J. Phys. Chem. 92 (1988)
2858.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/92 91
[50] G. Briganti, A.A. D’Archivio, L. Galantini, E. Giglio,
Langmuir 12 (1996) 1180.
[51] A.A. D’Archivio, L. Galantini, E. Gavuzzo, E. Giglio, L.
Scaramuzza, Langmuir 12 (1996) 4660.
[52] J. Ulmius, G. Lindblom, H. Wennerstrom, L.B.-A. Jo-
hansson, K. Fontell, O. Soderman, G. Arvidson, Biochem-
istry 21 (1982) 1553.
[53] R.G. Laughlin, The Aqueous Phase Behavior of Surfac-
tants, Academic Press, San Diego, 1994.
[54] N.S. Sundari, V. Srinivas, K.N. Ganesh, D. Balasubrama-
nian, J. Indian Chem. Soc. 62 (1985) 851.
[55] J. Lydon, Curr. Opin. Colloid Interface Sci. 3 (1998)
455.
H. Amenitsch et al. / Colloids and Surfaces A: Physicochem. Eng. Aspects 213 (2003) 79�/9292