ABSTRACT
It follows from the general propositions of phase equilibrium thermodynamics that the concentration of a dissolved impurity is defined from the equality of chemical potentials. One way of macroscopic thermodynamic analysis of solubility C s is to find particular values of pi and μs (see Section 1.2). It is simple to do this if both phases are ideal solutions. This assumption was used to obtain the ratios in (1.1.18) and (1.1.19). The principal feature of an ideal solution is the absence of chemical interactions of impurity atoms with one another and with other point defects. In this case, every subsystem consisting of one type of point defects has a partial chemical potential ) https://www.w3.org/1998/Math/MathML"> μ i = g i 0 + k T l n C i . https://s3-euw1-ap-pe-df-pch-content-public-p.s3.eu-west-1.amazonaws.com/9780429219092/f12f6525-7a90-46ab-98b1-4551c8ba4ab6/content/math5_1_1.tif" xmlns:xlink="https://www.w3.org/1999/xlink"/> Here, C i is the concentration of i-defects, T is temperature expressed in energy units, and g i 0 is Gibbs free energy necessary for the incorporation of a single defect into a pure crystal. The total chemical potential of the solid phase represents just an additive value (1.2.16).
