Solution-liquid-solid

Raoult s Law (a solid-liquid solution) says that the vapor pressure of an ideal solution iptotai) is directly proportional to the partial vapor pressure (p ) of the pure solvent times the mole fraction Xa = moles of solute per moles of solute and solvent) of the solute. 

Explain why we need to know the relative mobilities (flux rates) of the substances involved in a reaction (e.g., solids, liquids, solutes, gases) to decide on the applicability of equilibrium versus kinetic models. This relates to the concepts of open and closed systems and residence time. 

IR spectroscopy does not directly measure geometrical quantities. In Ch. 4 it is shown that measurements of the wavenumber of the centre of the most intense stretching band (X H - Y) of a H-bond X-H Y can be relatively precisely correlated to the X Y equilibrium distance of this H-bond. IR measmements are most easy, in any conditions gas, solid, liquid, solution, etc., and IR spectrometers are routine instruments in many laboratories. IR spectroscopy is consequently a basic general method to rapidly obtain geometrical parameters of H-bonds. Let us note that theoretical methods may also occasionally be used to estimate geometrical quantities of H-bonds made of small molecules. 

IR and Raman spectra were recorded and assigned for 1,3-dioxolane (24) and a range of mono-, di- and trimethylated derivatives at an early date <59JCS807>. IR data for l,3-dioxolan-2-one (25) in solid, liquid, solution and vapor phases and its Raman spectrum have also been reported <56TFS1 178, 68JSP(27)285>, as have both IR and Raman spectra for l,3-dioxol-2-one (8) <70JST(5)67>. Other simple... 

Fertilizers are packaged in a variety of different forms including solids, liquids (solutions and suspensions), and gas (anhydrous ammonia). The important physical properties of solid fertilizers are particle size, particle strength, caking tendency, chemical stability, and hygroscopicity. 

Considering, for the present, those systems in which only solid and liquid phases are present, it is clear that the system solid—liquid (solution) will be bivariant. If the pressure is maintained constant, the composition of the solution will vary with the temperature or, on the other hand, if the temperature is maintained constant, the composition of the solution will vary with the pressure. The influence of temperature on the solubility of a solid in water is sujSiciently appreciated the effect of pressure, although not so well known, is no less certain. 

Since in systems of two components the two phases, solution and vapour, constitute a bivariant system, the vapour pressure is undefined, and may have different values at the same temperature, depending on the concentration. In order that there may be for each temperature a definite corresponding pressure of the vapour, a third phase must be present. This condition is satisfied by the system solid—liquid (solution)— vapour that is, by the saturated solution (p. 165). In the case of a saturated solution, therefore, the pressure of the vapour at any given temperature is constant. 

Our focus in this chapter will be on solutions involving at least one liquid component—that is, gas-liquid, liquid-liquid, and solid-liquid solutions. And, perhaps not too surprisingly, the liquid solvent in most of the solutions we will study is water. 

Liquid-Liquid and Solid-Liquid Solutions Many salts dissolve in water because the strong ion-dipole attractions that water molecules form with the ions are very similar to the strong attractions between the ions themselves and, therefore, can substitute for them. The same salts are insoluble in hexane (CgH ) because the weak ion-induced dipole forces their ions could form with the nonpolar molecules of this solvent cannot substitute for attractions between the ions. Similarly, oil does not dissolve in water because the weak dipole-induced dipole forces between oil and water molecules cannot substitute for the strong H bonds between water molecules. Oil does dissolve in hexane, however, because the dispersion forces in one substitute readily for the dispersion forces in the other. Thus, for a solution to form, like dissolves like means that the forces created between solute and solvent must be comparable in strength to the forces destroyed within both the solute and the solvent. 

G.G. Warr, Surfactant adsorbed layer structure at solid/liquid solution interfaces impact and implications of AFM imaging studies, Curr. Opin. CoUoid Inteif. Sci., 2000, 5, 88-94. 

Two calorimetric techniques were used (drop calorimetry and differential scanning calorimetry DSC) to measure the temperatures and enthalpies of phase transitions (solid->solid and solid->liquid). Solution calorimetric determinations were also initiated. 

The term miscibility is used to describe the ability of one liquid to dissolve in another. The three kinds of attractive interactions (solute-solute, solvent-solvent, and solvent-solute) must be considered for liquid-liquid solutions just as they were for solid-liquid solutions. Because solute-solute attractions are usually much weaker for liquid solutes than for solids, this factor is less important and so the mixing process is often exothermic for miscible liquids. Polar liquids tend to interact strongly with and dissolve readily in other polar liquids. Methanol, CH3OH ethanol, CH3CH2OH acetonitrile, CH3CN and... 

There are several attractive features of the Extended X-ray Absorption Fine Structure (EXAFS) technique which make it a powerful structural tool notably (i) it is extremely fast, (ii) both sample preparation and data collection are relatively easy, without the requirement of single crystals, (iii) being sensitive to short-range order in atomic arrangements, it can focus on the local environment of specific absorbing atoms, and (iv) the technique is useful for a wide variety of materials such as amorphous solids, liquids, solutions, gases, polymers, and surfaces. 

In a solid/liquid solution, the liquid is usually considered the solvent, regardless of the relative proportions of the components. 

Your Morning Solution Even the simple act of adding sugar to a cup of tea or coffee involves several aspects of solid-liquid solution formation, including the effect of temperature on solubility. 

The formation of a solution is accompanied by an energy change. If you dissolve some potassium iodide, KI, in water, you will find that the outside of the container feels cold to the touch. But if you dissolve some sodium hydroxide, NaOH, in the same way, the outside of the container feels hot. The formation of a solid-liquid solution can apparently either absorb energy (KI in water) or release energy as heat (NaOH in water). 

When charges preferentially adsorb onto an interface adjacent to an aqueous solution they are balanced by counterions creating an electric double layer. For an aqueous NaCl solution I/kq = 30.4 nm at 10 M, 0.96 nm at 0. IM, and in pure water of pH 7, 1/kd is about one micron (e.g., Israelachvili 1992). With this in mind, the interfacial dynamics at an ice/solution interface can become quite complicated, and our studies of premelting dynamics might require consideration of a continuous variation in the interaction potential depending on the redistribution of ions. Preferential ion incorporation is best demonstrated in this context of solid/liquid solute distribution introducing ionic coefficients . A simple example for a monovalent electrolyte solution is... 

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