Solution in solid

De Fontaine, D. (1979) Configurational thermodynamics of solid solutions, in Solid State Physics, eds. Ehrenreieh, H., Seitz, F. and Turnbull, D. (Aeademie Press, New York) p. 74. 

When two metals A and B are melted together and the liquid mixture is then slowly cooled, different equilibrium phases appear as a function of composition and temperature. These equilibrium phases are summarized in a condensed phase diagram. The solid region of a binary phase diagram usually contains one or more intermediate phases, in addition to terminal solid solutions. In solid solutions, the solute atoms may occupy random substitution positions in the host lattice, preserving the crystal structure of the host. Interstitial soHd solutions also exist wherein the significantly smaller atoms occupy interstitial sites... 

Q A saturated solution of a slightly soluble ionic compound does not contain any of the solute in solid form. Is this system at equilibrium Explain your answer briefly. 

The universal interaction is due to the collective influence of the solvent l a dielectric medium and depends on the dielectric constant D and the (Tractive index n of the solvent. Reasonably large environmental pertur-fions may be caused by van der Waals dipolar or ionic fields in solution, in solids or in gases at high pressures. In gases, liquids and perturbation must be averaged over the molecular... 

Ionic current — The propagation of charge by ions. Ionic currents can flow between electrodes in an - electrolyte solution, in - solid electrolytes, in molten salts (including - ionic liquids) and also in plasmas. In solid electrolytes ionic currents can be accompanied by electronic currents, whereas they will be always accompanied by electronic currents in plasmas. 

Equations (15) and (16) suggest that for ideal solutions, i.e., for the solutions involving molecules of similar sizes and intermolecular forces, Yj = 1 and the solubility can be estimated based on enthalpy of fusion, heat capacities of solute in solid and liquid states, and triple point temperature. Moreover, Eqs. (15) and (16) imply that solubility increases with temperature. 

H-donor strength of the solute or its chemical class Volumetric coefficient of expansion of the solute in liquid state volumetric coefficient of expansion of the solute in solid state H-acceptor strength of the solute or its chemical class liquid - solid energy/mol temperature... 

Solid Solutions in solid solutions, the solvent is a solid. The solute can be a solid, liquid, or gas. The most common solid solutions are solid-solid solutions—ones in which the solvent and the solute are solids. A solid-solid solution made from two or more metals is called an alloy. It s also possible to include elements that are not metals in alloys. For example, steel is an alloy that has carbon dissolved in iron. The carbon makes steel much stronger and yet more flexible than iron. Two alloys are shown in Figure 6. 

Urea is used as a feed supplement for cattle, up to 8 lb/yr per head of cattle. In liquid fertilizers, urea raises the upper limit for stable nitrogen solutions. In solids it prevents caking due to the formation of ammonium chloride in mixtures of ammonium and potassium fertilizers. Ureaforms which are condensates of urea and formaldehyde, can be used as time-release fertilizers when it is desired to release fertilizing urea at a controlled rate, such as on a golf course [8]. The main use of solid, prilled urea is as side-dressing. 

Diffusive transfer of solutes in solids is governed by Fick s First and Second Laws, Even though biological solids are not stiucturally homogeneous and diffusion occurs mainly in the fluid occlnded within the solid, Fick s Laws will he expressed in terms of X, that is,... 

This is shown schematically in Figure 6.3 for a sodium chloride solution. In solid sodium chloride, there is a regular array of sodium and chloride ions. As shown in Figure 6.3a, each sodium ion has six chloride ions as its nearest neighbors, and each... 

The rate equations discussed above were derived for solutions. In solid-state, molarity is generally replaced by weight percent. This does not change the fundamental equations, based on the assumption that volumes do not change with low API conversions. 

D12. A countercurrent leaching system is recovering oil from soybeans. The system has five stages. On a volumetric basis, liquid flow rate/solids flow rate = 1.36. 97.5% of the oil entering with the nonsoluble solids is recovered with the solvent. Solvent used is pure. Determine the effective equlibrium constant, m, where m is (kg/m of solute in solvent)/(kg m of solute in solid) and is given by the equation y = m x. 

Coacervation n. The separation of a polymer solution into two or more liquid phases, one of which is a polymer-rich liquid. The term was introduced to distinguish this phenomenon from the precipitation of a polymer solute in solid form. The process is used in microencapsulation by emulsifying or dispersing the material to be encapsulated with a solution of the polymer. By changing the temperature or concentration of the mixture, or by adding another polymer or solvent, a phase separation may be induced and the polymeric portion forms a thin coating on the external surfaces of the particles. After further treatment to solidify the polymeric wall, the capsules can be isolated in powder form by filtration. It is an intermediate stage between sol and gel formation. 

Precipitate pri- si-p9- t9t NL praecipitatum, ff. L, neuter of praecipitatus (1594) n. Substances separated from a solution in solid form by apphcation of cold or heat or by a chemical reaction. 

When it is obvi that foe solubility of a solid depends on intermolecular forces between solute and solvent, it is perhaps not as obvious that fob solubility also depends on bow far the system temperature b removed from foe solid s mehtt point and on the solute s enthalpy of fusion. These dependencies become clear when we relate the starrdard-state fogacity of the solute in solid phase to that in the liquid phase, as indicated bdow. 

In most solutions, a larger amount of one substance is present compared to the other components. This most abundant substance in a solution is called the solvent, and any other components are called solutes. Most people normally think of solutions as liquids, but solutions in solid and gaseous forms are known as well. The state of a solution is often the same as the state of the solvent. This is iUnstrated by I Table 7.1, which lists examples of solutions in various states. The original states of the solvents and solntes are given in parentheses. Solution formation takes place when one or more solutes dissolve in a solvent. 

Dove, M.T. (2001) Gomputer simulation of solid solutions, in Solid Solutions in Silicate and Oxide Systems, vol. 3 (ed. C.A. Geiger), EMU Notes in Mineralogy,... 

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