# Diffusion through colloidal shells under stress

Entry by Emily Redston, AP 225, Fall 2011

Work in Progress

## Reference

Diffusion through colloidal shells under stress by J. Guery, J. Baudry, D. A. Weitz, P. M. Chaikin, and J. Bibette. Phys. Rev. E 79, 060402(R) (2009).

## Introduction

One area of great interest in soft matter is encapsulation. With applications in almost all types of industrial domains, from the oil industry to food packaging, efficient storage of gases and liquid in solid containers is of tremendous technological and economical importance. Furthermore, encapsulation of active ingredients such as drugs, proteins, nutrients, or vitamins is essential for a myriad of applications, such as drug delivery and agrichemicals.

The goal of encapsulation is to protect the delicate substances inside from a harsh environment, and to retain their activity until some required time. Long-term storage of liquids or gases often involve internal pressures, which increase the tensile stress of the container wall. At a colloidal scale, it is the osmotic pressure difference between the internal and external medium that is relevant, rather than the hydrostatic pressure. Eyring proposed that the permeability of solids is associated with a diffusive process involving an activation mechanism. Unfortunately, many of his ideas have not been tested quantitatively and thus many fundamental concepts are not fully understood.

In this paper, the authors propose a very cute little experiment that tests some of Eyring's ideas. By using core-shell (liquid core - solid shell) colloidal particles that are sensitive to osmotic pressure, they are able to follow the permeation of encapsulated probes at various stresses.

## The Core-Shell Colloids

The authors create these colloidal shells using a double emulsion, which consists of droplets of water in larger drops of crystallizable oil. The oil is a mixture of crystallizable triglycerids, which allows the authors to make the emulsion at high temperature, around 70°C, where the oil is fluid, and then cool the sample to solidify the oil, creating a robust shell. The robust solid shell is only achieved at temperatures below the melting temperature of the oil (around 45°C). NaCl is added to the water to prevent ripening of the droplets, and glucose is also added to match the chemical potential of the inner water to the continuous phase water. The osmotic pressure difference is then deduced from the concentration of salt and glucose.

## Experiments and Results

Figure 1. (a) Temporal evolution of the fractional release (X) for a shell composed of pure oil DM, at different temperatures: ($\circ$) 15 °C; ($\vartriangle$) 45 ° C; ($\diamond$) 60 ° C; and ($\Box$) 65 ° C. The solid lines correspond to the best adjustment of the data with the equation: X(t)=1−[(1−$X_{0}$)exp(−$\Beta_{0}$t)]. (b) Evolution of the characteristic relaxation rate $\Beta_{0}$ in logarithmic scale with 1/$k_{B}$$T_{r}$. The solid line corresponds to an exponential adjustment.
Figure 2. (a) Temporal evolution of the fractional release (X), for different dilution factors (T = 15°C); ($\circ$) d=0, $\Delta$$\Pi$=0 atm; ($\times$)d=1.4, $\Delta$$\Pi$=5 atm; ($\triangledown$) d=1.8, $\Delta$$\Pi$=8 atm; ($\vartriangle$) d=4, $\Delta$$\Pi$=13 atm; ($\diamond$) d=10, $\Delta$$\Pi$=15 atm; ($\Box$) d=100, $\Delta$$\Pi$=17 atm. The solid lines correspond to the best numerical adjustment of the data with Eq. (2). (b) Evolution of dX/dt (t=0) in logarithmic scale with 1−(1/d). The solid line corresponds to an exponential adjustment.

Potentiometric titration is used to measure the concentration of chloride ions as they are released into the continuous water phase. The relative ionic concentraion in the water ouside of the colloids, X, can then be found by normalizing the concentration at each time by the value obtained when all ions are released. Fig. 1(a) shows this fractional release X as a function of time at different temperatures (from 15 to 65°C for the oil). At 15°C the oil is essentially solid, while at 65°C it is entirely melted. The authors believe that the measured release results entirely from the diffusion of sodium and chloride ions from the inner droplets toward the external phase because there is no observed coalescence of the inner droplets with the globule interface.

This passive permeation must obey Fick’s law given by J = −d$N_{i}$ / dt = PS($C_{i}$ - $C_{e}$), where J is the flux of salt from inside toward the external phase, $N_{i}$ is the total number of salt ions inside the globule, P is the permeation coefficient of the shell, S is the total shell surface, and C is the concentration of salt inside (i) and in the external phase (e). The authors then assume that the limiting step is the permeation through the outer shell. The oil film between inner water droplets is much thinner than the shell thickness. Hence the salt concentration Ci is essentially homogeneous within the inner water droplets during the leakage process. If the globule volume fraction $\phi$ is small, we have

dX/dt = $\Beta_{0}$(1 − X), (1)

where the ion concentration X = $C_{e}$(t) / $C_{e}$ (t = infinity), and where $\Beta_{0}$ = 3P/a is the characteristic relaxation rate, with a being the globule radius. Therefore X(t)=1−[(1−$X_{0}$)exp(−$\Beta_{0}$t)], where $X_{0}$ is the initial burst fractional release which arises during the double emulsification process. For all temperatures studied the release mechanism is well described by a single exponential relaxation of time scale 1/$\Beta_{0}$, in agreement with the original Eyring assumption that the permeation coefficient P is proportional to exp($E_{a}$ / $k_{B}$T), where $E_{a}$ is the activation energy and $k_{B}$T is the thermal energy. Fig. 1(b) shows ln$\Beta_{0}$ as a function of 1 / $k_{B}$TT, from which the authors deduce that the activation energy $E_{A}$ is ~ (5 – 7)$k_{B}$$T_{r}$, $T_{r}$ = 25° C. In the absence of osmotic mismatch the leakage of the colloidal system is strictly diffusion driven, with no discontinuity at the liquid-solid transition again in agreement with the Eyring picture.

Dilution of the double emulsion by a factor of 100 using pure water leads to an osmotic pressure difference of $\Delta$$\Pi$ = 17 atm. Because there is a slight but sufficient permeability of water through the shell the chemical potential of the water equilibrates rapidly resulting in an immediate increase in the internal pressure. At 15°C where the DM oil shell is solid, there is a rapid increase in the release of Cl− ions followed by slower approach to the asymptotic limit, as shown by the open squares in Fig. 2(a). We vary the driving osmotic pressure, $\Delta$$\Pi$, by using water with increasing concentrations of glucose, diluting the double emulsion by the same factor each time; this reduces the rate of release. For $\Delta$$\Pi$ = 0, there is a residual very slow release of Cl− shown by the open circles in Fig. 2(a). For $\Delta$$\Pi$ $\ne$ 0, the osmotic pressure mismatch causes a tensile stress on the shell, which should modify the activation energy. To check this hypothesis we must consider the relation between the osmotic pressure difference and the resulting tensile stress that acts on the colloidal shell. In the limit of a thin shell of thickness $\delta$ , this relation can be simply derived from a force balance argument. The force exerted by the osmotic pressure mismatch on each half shell, $\pi$ $a^2$$\Delta$$\Pi$ , and the force due to the tensile stress,$\tau$, acting on the perimeter that holds the two half shells together, 2$\pi$a$\delta$$\tau$, must be equal, $\tau$ = $\Delta$$\Pi$(a/2$\delta$). Part of the local activation energy $E_{A}$ for an ion permeating a solid comes from the deformation energy of adding its additional volume to the solid matrix. The worklike energy for adding this volume increases under compressive stress and

decreases under tensile stress in a complex manner, which nonetheless must be linear in applied stress and ionic vol- ume, 􏰐3. The activation energy is expected to be linearly modified by the tensile stress as E􏰀􏰏􏰁=Ea−􏰏􏰐3. The osmotic pressure difference 􏰋􏰌 can be approximated as 􏰋􏰌 = RT􏰀2Ci − 2Ce − Csugar􏰁 􏰄 RT􏰀2Ci − Csugar􏰁 since Ce can be neglected as long as the globule volume fraction remains small, Csugar is the final sugar concentration imposed by the dilution, and R is the ideal gas constant. 􏰋􏰌 can now be expressed as 􏰋􏰌 = 2RTCi0􏰀1 − X − 1 / d􏰁, where Ci0 is the ini- tial internal salt concentration and d is the dilution factor of the external phase that sets the initial osmotic pressure dif- ference 􏰋􏰌0. Thus, Eq. 􏰀1􏰁 becomes dX / dt = 􏰊􏰀X􏰁􏰀1 − X􏰁 and the characteristic relaxation rate 􏰊􏰀X􏰁 can be expressed as 200 Time (min) 􏰊􏰀X􏰁 = 􏰊0 exp􏰂􏰑􏰀1 − 1/d􏰁􏰃exp􏰀− 􏰑X􏰁, 􏰀2􏰁 with 􏰑=􏰀a/􏰍􏰁􏰀􏰐3/k T􏰁􏰀RTC 􏰁. In kT units, 􏰑􏰀1−1/d􏰁 is the B i0 initial drop of the activation energy induced by the initial tensile stress. Thus, at short time when few ions have dif- fused through the shells and the osmotic shock is still at its maximum, the permeation rate 􏰊 increases by the large factor exp􏰂􏰑􏰀1 − 1 / d􏰁􏰃. At longer time the second term exp􏰀−􏰑X􏰁, which reflects the equilibration of the osmotic stress, slows down the relaxation rate. A plot of log􏰂dX/dt􏰀t=0􏰁􏰃, as a function of 1−1/d is linear with slope 􏰑, as seen in Fig. 3􏰀b􏰁. From the slope we find 􏰑=2.5􏰒0.3. Equation 􏰀2􏰁 can be numerically solved and compared to our data as shown in Fig. 3􏰀a􏰁. In this fit we also take into

account the nonideal dependence of the osmotic pressure with the sugar and salt concentrations 􏰂15􏰃. The fit is remark- able and allows for the determination of the two unknown parameters 􏰑 and 􏰊0. The time evolution reflects the expo- nential decrease in diffusion as the osmotic pressure tends toward equilibration causing the stress to decrease and acti- vation energy to increase. It provides another measure of the enhancement of the permeation rate by stress to be compared with the values obtained by varying the initial osmotic shock, Fig. 3􏰀b􏰁 􏰀􏰑=4.1􏰒1.4 and 􏰊0=8􏰒6 10−4 min−1􏰁. With 􏰍=100 nm we get 􏰐=0.6 nm comparable to the size of a hydrated ion, as expected from the Eyring picture.