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irradiation for 10 min, and TEM image of the colloids before light irradiation is also given for comparison. It can be seen that after the irradiation, the spheres are deformed to ellipsoids, which can also be con rmed by AFM observations. The elongation occurs in the polarization direction of the laser beam, which is also the grating vector direction of the interference patterns. In the testing period (15 min), the colloids can be continuously elongated by the light irradiation. The average major-to-minor axis ratio (l/d) of the colloids can be used to indicate the deformation degree of the colloids. Figure 5.11 shows the SEM images of colloidal particles observed before the irradiation and after the irradiation for different time periods. After 5-min irradiation, obvious change in the shape can be observed. As the irradiation time increases, the elongation can be observed to increase continuously. The relationship between the average major-tominor ratio (estimated statistically from SEM images of 100 colloidal particles) and the irradiation time is given in Fig. 5.12. The major-to-minor ratio increases almost linearly with the irradiation time increase in the testing range. The colloidal sphere deformation could be attributed to the optically induced electric eld gradient, which has been used by Kumar et al. (1998) to explain the SRG formation. The polymers used to construct the photodeformable colloids can also show sensitive properties to form SRG. Photoinduced mass migration has been used to account for the SRG formation, where the polymer chains are driven by light to move from bright to dark regions. The colloid deformation could also be caused by the mass migration related to the electric eld gradient force.

thermodynamics of liquid mixtures are conceptually and mathematically rather complicated so that the reader must be referred to special monographs on the subject. On the other hand, it matters little at this stage that statistical thermodynamic procedures are so far lacking in the present textbook. The derived equations have not yet even been worked out to an experimentally verifiable form. In fact, the theory of ionic solutions should yield an equation permitting calculation of the activity coefficients of ions on the basis of knowledge of the structure of the ion considered and of all the other components of the solution. The methods of statistical thermodynamics that would, in principle, be capable of carrying out this calculation are developing rapidly and it seems that the future looks promising in this area.

SMI-S supplies profiles of Resource Information Models specific for storage and is a discipline-specific management standard for the storage industry. This technical specification defines the method for the interoperable management of a heterogeneous SAN and describes the information available to a WBEM (Web-Based Enterprise Management) client from an SMI-S compliant CIM server. This technical specification describes an object-oriented, XML-based, messaging-based interface designed to support the specific requirements of managing devices in and through SANs.

1 m (c)

if the membrane is permeable for anion Az~. The membrane potential expressed by Eqs (6.1.3) and (6.1.4) is termed the Nernst membrane potential as it originates from the analogous ideas as the Nernst equation of the electrode potential (p. 165) and the equation of the Nernst potential at ITIES (Eq. (3.3.50)). Consider a system in which both solutions contain various ions for which the membrane is permeable (diffusible ions) and one type of ion that, for some reason (e.g. a macromolecular ion for a porous membrane), cannot pass through the membrane (non-diffusible ion). The membrane is permeable for the solvent. The equilibrium conditions for the diffusible ions are fc(l,Pi) = /(2,p2) (6.1.5)

413 This condition expresses the fact that the two solutions are under different pressures, px and p2, as a result of their, in general, different osmotic pressures. An analogous equation cannot be written for the non-diffusible ion as it cannot pass through the membrane and the 'equilibrium' concentrations cannot be established. First, let us consider dilute solutions, where it is possible to set px = p2Then the electrochemical potentials in Eq. (6.1.5) are expanded in the usual manner, yielding ^ for the diffusible cation and a (2) ^ O (6.1.7) 0 (6.1.6)

1 m (d)

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for the diffusible anion. Elimination of the terms containing the electric potentials in these equations yields (6.1.8) i.e. for univalent, divalent, etc., cations and anions

1 m

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11/2

1 m

La2_(2)J La 3 _(2). The constant A is termed the Donnan distribution coefficient. In the simple case of a diffusible, univalent cation B + and anion A~ and non-diffusible anion X~ present in phase 2, the condition of electroneutrality gives