McMillan-Mayer solution theory

The crowding approach, which has been based upon McMillan-Mayer solution theory, has anployed Equation 11.7 as a starting point (Davis-Searles et al. 2001 Shimizu and Boon 2004). This is based upon a second virial approximation. FST can even provide the condition upon which this approximation is accurate. Since Equation 11.7 holds under the condition that AN21 is negligibly small, and that this quantity is related to the partial molar volume via Equation 11.5, the proposed condition is... 

The primitive model of electrolytes constitutes a Arm basis for statistical-mechanical description of solutions of charged colloids. This model will be adopted throughout, and it originates from the more general McMillan-Mayer solution theory [62,63]. 

This is essentially the result of the McMillan-Mayer solution theory from statistical mechanics. 

The formal theoretical framework for studying deviations from dilute ideal solutions is embodied in the so-called virial expansion of the osmotic pressure n), through the McMillan-Mayer (1945) theory of solutions ... 

In contrast to Pitzer s work, which is given in molalities (Lewis-Randall theory (LR)), the MSA naturally expresses thermodynamic quantities in terms of concentrations, in the framework of the McMillan-Mayer (MM) theory of solutions [33]. Thus, the data have to be converted from Lewis-Randall to McMillan-Mayer scale for adjusting the model to experiment. The basic ingredients of the LR-to-MM conversion have been given [34] and recently an approximate simple conversion has been tested [35]. The great advantage of this transformation is that it keeps the... 

McMillan-Mayer theory of solutions [1,2], which essentially seeks to partition the interaction potential into tln-ee parts that due to the interaction between the solvent molecules themselves, that due to die interaction between the solvent and the solute and that due to the interaction between the solute molecules dispersed within the solvent. The main difference from the dilute fluid results presented above is that the potential energy u(r.p is replaced by the potential of mean force W(rp for two particles and, for particles of solute in the solvent, by the expression... 

The McMillan-Mayer theory allows us to develop a fomialism similar to that of a dilute interacting fluid for solute dispersed in the solvent provided that a sensible description of W can be given. At the Ihnit of dilution, when intersolute interactions can be neglected, we know that the chemical potential of a can be written as = W (a s) + IcT In where W(a s) is the potential of mean force for the interaction of a solute... 

The McMillan-Mayer theory offers the most usefiil starting point for an elementary theory of ionic interactions, since at high dilution we can incorporate all ion-solvent interactions into a limitmg chemical potential, and deviations from solution ideality can then be explicitly coimected with ion-ion interactions only. Furthemiore, we may assume that, at high dilution, the interaction energy between two ions (assuming only two are present in the solution) will be of the fomi... 

When the adsorbent molecides are not independent, we can no longer use the relation (D.2) for the GPF of the system. In this case, we must start from the GPF of the macroscopic system from which we can derive the general form of the BI for any concentration of the adsorbent molecule. The derivation is possible through the McMillan-Mayer theory of solution, but it is long and tedious, even for first-order deviations from an ideal solution. The reason is that, in the general case, the first-order deviations would depend on many second-virial coefficients [the analogue of the quantity B2(T) in Eq. (D.9)]. For each pair of occupancy states, say i and j, there will be a pair potential [/pp(R, i,j), and the corresponding second-virial coefficient... 

Explain in about 250 words the essential approach of the Mayer theory of ionic solutions and how it differs from the ionic-atmosphere view. The parent of Mayer s theory was the McMillan-Mayer theory of 1950. With what classical equation for imperfect gases might it be likened ... 

It has been seen that reliable conductivity values are known only at low electrolyte concentrations. Under these conditions, even conductance equations for models such as the McMillan-Mayer theory (Sections 3.12 and 3.16) are known. However, the empirical extension of these equations to high concentration ranges has not been successful. One of the reasons is that conductivity measurements in nonaqueous solutions are still quite crude and literature values for a given system may vary by as much as 50% (doubtless due to purification problems). 

In the next section we shall present a simplified expansion theorem of osmotic pressure which was first obtained by McMillan and Mayer. This cluster expansion theory will be further extended in Section 3 to distribution functions, and medn results of Kirkwood and Buff will be recovered. A new and simple derivation of the cluster expansion of the pair distribution function is also given. Section 4 presents a new expression for the chemical potential of solvents in dilute solutions. Section 5 shows how the general solution theory may be applied to compact macromolecules. Finally, Section 6 deals with the second osmotic virial coefficient of flexible macromolecules and is followaJ in Sa tion 7 by concluding remarks. 

The application of McMillan-Mayer theory to high polymer solutions was first made by B. H. ZiMM. J. Chem. Phys. 14, 104 (1946). 

Many models are available for describing the thermodynamic behavior of solutions. " However, so far no one could satisfactorily simulate the solution behavior over the whole concentration range and provide the correct pressure and temperature dependencies. This generated interest in the thermodynamically rigorous theories of Kirkwood—Buff and McMillan—Mayer. In the present paper, the emphasis is on the application of the Kirkwood—Buff theory to the aqueous solutions of alcohols, because it is the only one which can describe the thermodynamic properties of a solution over the entire concentration range. The key quantities in the Kirkwood-Buff theory of solution are the so-called Kirkwood-Buff integrals (KBIs) defined as... 

The present calculations are in agreement with the conclusion of ref 59 (which employed both a lattice and the McMillan— Mayer theories of solution" ) that the solute—solute interactions in the systems investigated increase in the sequence MeOH < EtOH < 2-PrOH < 1-PrOH t-BuOH. There are, however, essential differences between the lower alcohols (MeOH and EtOH) and the higher ones. 

This generated interest in the rigorous statistical thermodynamic theories of Kirkwood-Buff and McMillan-Mayer. In Chapter 5, the emphasis is on the application of the Kirkwood-Buff theory to aqueous solutions of proteins. 

In this chapter some aspects of the present state of the concept of ion association in the theory of electrolyte solutions will be reviewed. For simplification our consideration will be restricted to a symmetrical electrolyte. It will be demonstrated that the concept of ion association is useful not only to describe such properties as osmotic and activity coefficients, electroconductivity and dielectric constant of nonaqueous electrolyte solutions, which traditionally are explained using the ion association ideas, but also for the treatment of electrolyte contributions to the intramolecular electron transfer in weakly polar solvents [21, 22] and for the interpretation of specific anomalous properties of electrical double layer in low temperature region [23, 24], The majority of these properties can be described within the McMillan-Mayer or ion approach when the solvent is considered as a dielectric continuum and only ions are treated explicitly. However, the description of dielectric properties also requires the solvent molecules being explicitly taken into account which can be done at the Born-Oppenheimer or ion-molecular approach. This approach also leads to the correct description of different solvation effects. We should also note that effects of ion association require a different treatment of the thermodynamic and electrical properties. For the thermodynamic properties such as the osmotic and activity coefficients or the adsorption coefficient of electrical double layer, the ion pairs give a direct contribution and these properties are described correctly in the framework of AMSA theory. Since the ion pairs have no free electric charges, they give polarization effects only for such electrical properties as electroconductivity, dielectric constant or capacitance of electrical double layer. Hence, to describe the electrical properties, it is more convenient to modify MSA-MAL approach by including the ion pairs as new polar entities. 

Special emphasis is placed upon the McMillan-Mayer theory (Sections 4 and 5) and on cluster expansions (Section 6), as these represent aspects that are both difficult and strongly established, but that are seldom given detailed exposition. Other developments that are easily accessible in the literature are treated more lightly, as are the many aspects of theory of fluids that are not yet completely developed for application to ionic solution problems. 

The McMillan-Mayer theory shows that the osmotic pressure of a solution, the thermodynamic functions that may be derived from the osmotic pressure as a function of composition, and the solute-solute correlation functions can all be expressed as functionals of the solvent-averaged potentials... 

There are essentially two theories of solutions that can be considered exact the McMIllan-Mayer theory and Fluctuation Solution Theory (FST). The first Is mostly limited to solutes at low concentrations, while FST has no such issue. It is an exact theory that can be applied to any stable solution regardless of the number of components and their concentrations, and the types of molecules and their sizes. Fluctuation Theory of Solutions Applications in Chemistry, Chemical Engineering, and Biophysics outlines the general concepts and theoretical basis of FST and provides a range of applications described by experts in chemistry, chemical engineering, and biophysics. 

Many, if not most, processes of interest occnr in solutions. It is therefore somewhat unfortunate that our understanding of solutions and their properties remains rather limited. There are essentially two theories of solutions that can be considered exact. These are the McMillan-Mayer theory of solutions and Fluctuation Solution Theory (FST), or the Kirkwood-Buff (KB) theory of solutions. The former has practical issues, which limit most applications to solutes at low concentrations. The latter has no such issues. Nevertheless, the general acceptance and appreciation of FST remains limited. It is the intention of this book to outline and promote the considerable advantages of using FST/KB theory to study a wide range of solution properties. 

Now we want to leave our discussion of what might be called the ancient and early modem periods of solution theory history and concentrate on the modem period, characterized by the theories of Mayer and McMillan (McMillan and Mayer 1945) and of Kirkwood and Buff (Kirkwood and Buff 1951). The McMillan-Mayer theory was the earlier of the two, by some 6 years, and had already captured the attention of the experimental community by the time the Kirkwood-Buff theory appeared. 

The starting point of McMillan-Mayer theory is a relationship between distribution functions at different activity sets. The derivation of this relationship is the difficult part of the theory. But once obtained, the relation leads to an expression for the osmotic pressure of a solution, since the components permeable to the osmotic membrane have the same chemical potential on both sides of the membrane while those impermeable have differing chemical potentials. A lengthy computation then leads to an expansion for the osmotic pressure, completely analogous to the activity expansion of the pressure in the theory of imperfect gases. Indeed, for the purpose of comparing gas theory with solution theory, it helps to regard the gas as a solute in a very special and very simple solvent— vacuum. The X expansion is. 

The results of McMillan-Mayer theory have been used primarily in the area of solutions of macromolecules in low molecular weight solvents. The osmotic second virial coefficient, which can be measured either by osmometry or light scattering, gives information on the size of the solute molecules. We shall see why in more detail later when we discuss fluctuation theory. 

The theory of McMillan and Mayer is exact, but only useful in dilute solutions. It delivers thermodynamic functions as a power series in the solute concentrations and it is quite difficult to compute, or even to interpret the coefficients higher than the second virial coefficient, Bj. About 6 years after the McMillan-Mayer theory was developed a new solution theory appeared, not subject to this difficulty, that of Kirkwood and Buff (Kirkwood and Buff 1951), of course this new theory had computational problems of its own. KB (Kirkwood-Buff) theory is also known as fiuctuation theory for reasons that will become obvious below. It is the basis for the rest of this volume and therefore will occupy the remainder of this chapter. 

Second, one might ask, since McMillan-Mayer and Kirkwood-Buff theories are both exact, what is the relation between them McMillan-Mayer theory is formulated in terms of potentials of mean force at infinite dilution, albeit of increasing numbers of particles. Kirkwood-Buff theory is formulated in terms of the potential of mean force between pairs only, but at the actual concentration of the solution. The answer to this question is given by Equation KB23, written down without derivation. A future publication with a derivation is promised but, as far as I know, now 60 years later, none has appeared. This is an unsatisfactory state of affairs. 

There are a variety of theories for dilute polymer solutions that seek to express the virial coefficients in terms of molecular variables. Some of these theories are rigorous, usually based on the McMillan and Mayer general theory of solutions. Others are approximate and attempt to obtain semi-empirical or phenomenological expressions. Almost all the effort has been directed at the second virial coefficient, A. The third virial coefficient, is frequently taken to be related to A 2 (for a solute with molecular weight M) ... 

A mean field theory of solvent structure has been employed by Marcelja(146) to describe the effect of solvent correlation on solute-solute interactions of both hydrophobic and hydrophilic solutes. The interactions between hydrophilic solutes in water has also been considered in a group of papers(141,147-150) where the heats of dilution and of the mixing at constant molality for various non electrolytes (alcohols, amides, sugars, urea, aminoacids and peptides) are interpreted in the framework of the McMillan-Mayer theory(151) and the enthalpy effects arising from interactions between each functional group on one molecule and every functional group on the other molecule are evaluated. 

What follows will concern electrolyte solutions as well as molten salts. In fact, as we will see later, within the framework of the McMillan-Mayer theory(l), there is no difference in the mathematical treatment of a dilute aqueous solution of a given electrolyte and the corresponding molten salt. Of course, the density, temperature and potential energy will be different, but in both cases, the model to be used will be the same. It should then not be surprising that the next section starts with a discussion of the McMillan-Mayer and Debye-Hiickel theories(2) for dilute systems of charged particles. The Debye-Hiickel theory (DH) has been the most successful theory of electrolyte solutions and some of the modern approximations are simple extensions of DH theory, which are statistically consistent. 

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