Solubility of a solid

The solubility of a solid in the liquid phase of a mixture depends on the properties of the two phases for the components that crystallize, the equilibrium is governed by the following equation [ XI... [Pg.171]

The chemical potential of a curved surface is extremely critical in ceramic processing. It detemiines reactivity, tlie solubility of a solid in a liquid, tire rate of liquid evaporation from solid surfaces, and material transport during sintering. [Pg.2761]

For a substance to dissolve in a liquid, it must be capable of disrupting the solvent structure and permit the bonding of solvent molecules to the solute or its component ions. The forces binding the ions, atoms or molecules in the lattice oppose the tendency of a crystalline solid to enter solution. The solubility of a solid is thus determined by the resultant of these opposing effects. The solubility of a solute in a given solvent is defined as the concentration of that solute in its saturated solution. A saturated solution is one that is in equilibrium with excess solute present. The solution is still referred to as saturated, even... [Pg.59]

The solubility of a solid in a liquid at its saturation vapor pressure is usually represented as a (T, x2) graph, where x2 is the mole... [Pg.86]

In Fig. 2, we showed the solubility of a solid component in a compressed gas as calculated from Eq. (11). A similar calculation can be made for the solubility of a liquid component in a compressed gas which is only slightly soluble in the liquid. For the liquid component, when xt 1, the equation of equilibrium is... [Pg.147]

The solubility of a solid can be increased by removing one of its ions from solution acid can be used to dissolve a hydroxide, sulfide, sulfite, or carbonate precipitate and nitric acid can be used to oxidize metal sulfides to sulfur and a soluble salt. [Pg.593]

The effect of complex formation on the solubility of a solid can be observed in the home. Silver dinnerware eventually becomes discolored by an unsightly black tarnish of Ag2 S, formed from the reaction of the silver surface with small amounts of H2 S present in the atmosphere. Silver sulfide is highly insoluble in water. Commercial silver polishes contain ligands that form strong soluble complexes with Ag ions. If a tarnished serving pan is rubbed with a polish, the black tarnish dissolves, returning the silver to its brilliant shine. [Pg.1328]

The solubility of a solid in a relevant solvent medium is a crucial characteristic. Solubility is defined as the concentration of the dissolved solid (the solute) in the solvent medium, which becomes the saturated solution and which is in equilibrium with the solid at a defined temperature and pressure. The solubility depends on the physical form of the solid, the nature and composition of the solvent medium, the temperature, and the pressure [1],... [Pg.322]

Some substances will dissolve in a particular solvent and others will not. There is a general rule in chemistry that states like dissolves like. Polar substances (such as alcohols) will dissolve in polar solvents like water. Nonpolar solutes (such as iodine) will dissolve in nonpolar solvents such as carbon tetrachloride. The mass of solute per 100 mL of solvent (g/100 mL) is a common alternative to expressing the solubility as molarity. It is necessary to specify the temperature because the solubility of a substance will vary with the temperature. The solubility of a solid dissolving in a liquid normally increases with increasing temperature. The reverse is true for a gas dissolving in a liquid. [Pg.172]

Some of these factors were addressed in the Reactions and Periodicity chapter. In general, the solubility of a solid or liquid will increase with temperature and be unaffected by pressure changes. The solubility of a gas will decrease with increasing temperature and will increase with increasing partial pressure of the gas (Henry s law). [Pg.180]

The solubility of a solid, provided that it does not form crystal solvates, or solid solutions, with the solvent but remains as a pure solid, and provided again that only dispersion forces are operative, is given approximately by ... [Pg.79]

The solubility of a solid-solution component varies depending on temperature and pressure. [Pg.146]

Solvent Strength of Pure Fluids. The density of a pure fluid is extremely sensitive to pressure and temperature near the critical point, where the reduced pressure, P equals the reduced temperature, Tr, =1. This is shown for pure carbon dioxide in Figure 2. Consider the simple case of the solubility of a solid in this fluid. At ambient conditions, the density of the fluid is 0.002 g/cm3. Thus the solubility of a solid in the gas is low and is given by the vapor pressure over the total pressure. The solubilities of liquids are similar. At the critical point, the density of C02 is 0.47 g/cm3. This value is nearly comparable to that of organic liquids. The solubility of a solid can be 3—10 orders of magnitude higher in this more liquid-like C02. [Pg.220]

The Kelvin equation may also be applied to the equilibrium solubility of a solid in a liquid. In this case the ratio p/p0 in Equation (40) is replaced by the ratio a/a0, where a0 is the activity of dissolved solute in equilibrium with a flat surface, and a is the analogous quantity for a spherical surface. For an ionic compound having the general formula MmXn, the activity of a dilute solution is related to the molar solubility S as follows ... [Pg.263]

When considering the solubility of a solid organic compound in water, conceptually we can imagine first converting it to the liquid state and then proceeding as above for a liquid compound. The free energy cost involved in the solid-to-liquid conversion is referred to as the free energy of fusion, (Chapter 4). This entity can be derived... [Pg.138]

What effect does temperature have on the solubility of a solid solute in a liquid solvent ... [Pg.245]

In the following discussion, only the basic equations that allow the calculation of the solubility of a solid material (solute, component 2) in a dense gas will be reported. The equilibrium condition for component 2 is ... [Pg.47]

The solubility of a solid in a liquid is the amount of the solid that will dissolve in the liquid to form an equilibrated saturated solution (Faure, 1998), 111. In the literature, the solubility of a particular solid substance in water has been traditionally derived from laboratory measurements of the mass or moles of the solid that dissolves in a given mass or volume of distilled and deionized water. These values are often listed in milligrams per liter, grams per 100 milliliters (Lide, 2007), grams per liter, micrograms per liter Oigl-1), molal, molar, or micromolar ( iM) (Table 2.8). [Pg.31]

Using the carbamazepine-nicotinamide cocrystal system, a mathematical model has been developed to predict the solubility of cocrystals [41], The model predicted that the solubility of a solid cocrystal is determined by the solubility products of the reactant species and solution complexa-tion constants that could be obtained from the performance of solubility studies. In addition, graphical methods were developed to use the dependence of cocrystal solubility on ligand concentration for evaluation of the stoichiometry of the solution-phase complexes that are the precursor to the crystalline cocrystal itself. It was proposed that the dependence of cocrystal solubility on solubility product and complexation constants would aid in the design of screening protocols, and would provide guidance for systems where crystallization of the cocrystal did not take place. [Pg.378]

When we consider the solubility of a solid component in a solvent, the emphasis is placed on obtaining the mole fraction or other composition variable as a function of the temperature. Thus, Equation (10.96) gives the solubility as a function of the temperature in this interpretation. The solubility in an ideal solution is given by... [Pg.257]

In the study of the solubility of a solid component in a solution or the lowering of the freezing point of a solvent by the presence of a solute, the solid phase must be considered as the pure component. We indicate this component, the one that is present in both phases, by the subscript 1. The... [Pg.270]

Solubility constants. The solubility of a solid phase can be represented by a constant known as the solubility constant Kso, which is defined by the product of ion activities in solution, where these ions are the same as those that make up the original solid phase. For example, consider a solid phase consisting of a metal Me and a ligand L the solubility constant for the reaction MeaLb <-> aMeh+ + bV is given by the expression ... [Pg.96]

Dlepen and Scheffer ( 6) were the first to show that near either the lower or upper critical end point the solubility of a solid in a supercritical fluid is enhanced and also very sensitive to changes in temperature and pressure our solubility isotherms show this effect for both end points. First, the isotherms cross at about 140 bar so that the solubility at the lowest temperature (50.0°C) is largest at 120 bar. This is a result of approaching the lower critical end point region (which should be close to the critical point of pure C02 as previously mentioned). At temperatures and pressures near this LCEP the solubility enhancement results in lower temperature isotherms having the greater solubilities. The effect of the upper critical end point is also well shown by our data. The 58.5°C isotherm shows a large increase in solubility at about 235 bar the slope of the isotherm is near zero. As Van Welie and Diepen... [Pg.24]

The effect of temperature on retention has been described experimentally,(4-8) but the functional dependence of k with temperature has only recently been described.W A thermodynamic model was outlined relating retention as a function of temperature at constant pressure to the volume expansivity of the fluid, the enthalpy of solute transfer between the mobile phase and the stationary phase and the change in the heat capacity of the fluid as a function of temperature.(9) The solubility of a solid solute in a supercritical fluid has been discussed by Gitterman and Procaccia (10) over a large range of pressures. The combination of solute solubility in a fluid with the equation for retention as a function of pressure derived by Van Wasen and Schneider allows one to examine the effect of solubility on solute retention. [Pg.173]

The solubility of a solid in a supercritical fluid has been described by Gitterman and Procaccia.(lO) The region of interest chromatographically will be for infinitely dilute solutions whose concentration is far removed from the lower critical end point (LCEP) of the solution. Therefore the solubility of the solute in a supercritical fluid at infinite dilution far from criticality can be approximated as,... [Pg.174]

The fraction of coal which dissolves instantaneously in the supercritical fluid increases with an increase in the density and temperature of the supercritical fluid. This effect is similar to that generally observed for the solubility of a solid in a supercritical fluid. With an increase in density and temperature... [Pg.263]

The influence of surface free energy on solubility can be determined from straightforward thermodynamic considerations. The solubility of a solid can be calculated from the standard Gibbs free energy of reaction according to the relation ... [Pg.49]

It is clear from this equation that the solubility of a solid will increase exponentially with increasing surface area. For most solids, including carbonates, the influence of excess surface free energy is not large for particles unless they are under 0.1 microns in diameter (see Figure 2.6). It is important, however, to remember that... [Pg.50]

How would you expect the solubility of a solid to depend on crystal size What happens as a newly formed precipitate ages in contact with its supernatant liquid ... [Pg.353]

The saturation concentration is equal to the solubility of a solid in a liquid at a given temperature. Therefore, its value can in principle be found from the liquidus curve of the equilibrium phase diagram of the A-B binary system (see Fig. 1.1). [Pg.220]

Equation (3.6) illustrates that the solubility of a solid in a liquid depends on the enthalpy change at Tm and the melting temperature of the solid. Equation (3.6) is a valid one when T > Tm because the liquid solute in an ideal solution is completely miscible in all proportions. Table 3.1 shows the ideal solubilities of compounds and their heat of fusion. Equation (3.6) is the equation for ideal solubility. The relationship of In x2 (ideal or nonideal solubility) vs. 1/T is shown in Figure 3.1. [Pg.125]

In summary, the solubility of a solid in liquids is dependent greatly on the values of AHf and Tm as well as the characteristics of molecular interactions between the solute and solvent. [Pg.133]

We can survey the precipitation in the usual equilibrium diagram, in which the concentration and the temperature of the saturated solutions arc represented. Figure 7 schematically indicates the solubility of a solid as a function of the temperature. It can be seen that at increasing temperatures the solubility increases. Since the rate of crystallization or precipitation in-... [Pg.209]

How does temperature affect the solubility of a solid, a liquid, and a gas ... [Pg.325]

The solubility of a solid solute (component 2), in a supercritical fluid is calculated, if the solid phase is a pure component, by ... [Pg.265]

In the solubility of a solid substance the changes in energy and entropy in the solid-liquid transition must also be consider-... [Pg.364]

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