Water solubility Henry’s law

Density Dynamic Viscosity Kinematic Viscosity Water Solubility Henry s Law Constant Vapor Pressu... 

Zielinska et al. (1996) and Kelly and Holdren (1995) have summarized the stability in canisters of organics, some of which are U.S. EPA designated HAPs (hazardous air pollutants). Kelly and Holdren propose that for compounds whose stability in canisters is not known, estimates can be made based on species of similar physical and chemical characteristics. These characteristics include their vapor pressure, polarizability, water solubility, Henry s law coefficient in water, and estimated lifetimes with respect to reactions in air and in the aqueous phase. 

The ability to predict the behavior of a chemical substance in a biological or environmental system largely depends on knowledge of the physical-chemical properties and reactivity of that compound or closely related compounds. Chemical properties frequently used in environmental assessment include melting/boiling temperature, vapor pressure, various partition coefficients, water solubility, Henry s Law constant, sorption coefficient, bioconcentration factor, and diffusion properties. Reactivities by processes such as biodegradation, hydrolysis, photolysis, and oxidation/reduction are also critical determinants of environmental fate and such information may be needed for modeling. Unfortunately, measured values often are not available and, even if they are, the reported values may be inconsistent or of doubtful validity. In this situation it may be appropriate or even essential to use estimation methods. 

Wang, Y.H., Wong, P.K. (2002) Mathematical relationships between vapor pressure, water solubility, Henry s law constant, n-octanol/water partition coefficient and gas chromatographic retention index of polychlorinated-dibenzo-dioxins. Water Res. 36, 350-355. 

Physicochemical Lipophilicity (as logP) Water solubility Henry s law constant Rates of reaction... 

Sarraute, S., Delepine, H., Costa Gomes, M.F., Majer, V.(2004) Aqueous solubility, Henry s law constants and air/water partition coefficients of ra-octane and two halogenated octanes. Chemosphere 57, 1543-1551. 

Physical and Chemical Properties. The physical and chemical properties of bromomethane are sufficiently well known to allow estimation of environmental fate. Although there is some disparity in reported values for the solubility in water and Henry s law constant for bromomethane (see Table 3-1), further studies to define these parameters more precisely do not appear essential, since volatilization from water is so rapid. 

The exchange of chemical compounds from the gas phase to a surface, e.g. atmospheric particles, soil, water, vegetation or other surfaces, is controlled by the affinity of the compound to this surface. The ratio of vapour pressure to water solubility can be used as indicator between levels in the atmosphere and water surface (Henry s law H constant). In many model calculations, the ratio between POP levels in octanol and water, the octanol-water partitioning coefficient (Kow), is used as reference for the distribution of POP in organic material [14]. Consequently, the expression ///RT (Cair/Cwalcr) and Kow (Coctanoi/Cwater) provide the octanol-air partitioning coefficient (Koa) ... 

Solution. For TCE in water, the Henry s law coefficient may be taken as 417 atm/mf at 20°C. In this low-concentration region, the coefficient is constant and equal to the slope of the equilibrium line m. The solubility of TCE in water, based on H = 417 atm, is 2390 ppm. Because of this low solubility, the entire resistance to mass transfer resides in the liquid phase. Thus, Eq. (14-25) may be used to obtain N0l, the number of overall liquid phase transfer units. 

The solubility of gases in water is dependant upon temperature and atmospheric pressure and, providing the gas does not react with the water, follows Henry s law, which states that its solubility in the liquid is directly proportional to the partial pressure of the gas. 

Stewart and Munjal (20) determined the solubility of CO2 in distilled water, a S3mthetic sea water, and in three and five-fold concentrations of the synthetic sea water. The Henry s Law constants for CO2 computed for these systems at different temperatures were found to be linearly related to temperature and solution molality. The concentration of CO2 (aq) in moles per total moles of solution (mole fraction) may be written... 

Kurz, J., Ballschmitter, K. (1999) Vapour pressures, aqueous solubilities, Henry s law constants, partition coefficients between gas/water (Kg ) -octanol/water (Kqw) and gas/octanol (Kg ) of 106 polychlorinated diphenyl ethers (PCDE). Chemosphere 38, 573-586. 

Releases of carbon disulfide to the environment as a result of industrial activity are expected to be primarily to the atmosphere. Any carbon disulfide released to surface waters in effluent streams is expected to partition rapidly to the atmosphere as a result of the high ratio of vapor pressure to the solubility (Henry s law constant = 1.01 x 10"2 atm m3/mol) of the compound. Hydrolysis is not a significant removal mechanism since the evaporation half-life from a saturated solution is estimated to be 11 minutes (EPA 1978a). 

Table VII gives the Henry s law coefficients of some atmospheric gases in liquid water at 298 K. The values given reflect only the physical solubility of the gas regardless of the subsequent fate of the dissolved species A. Some of the species included in Table VII dissociate after dissolution or react with water. The Henry s law constants of Table VII do not account for these processes, and the modifications necessary will be discussed in the next paragraph. Henry s law coefficients generally decrease for increasing temperatures, resulting in lower solubilities at higher temperatures (Seinfeld, 1986).

As mentioned before, POP transport in the environment depends on their physicochemical properties [40-54], and these include saturated vapor pressure, solubility, Henry s law constant, octanol-water, octanol-air, and organic carbon-water partition coefficients. The saturated vapor pressure characterizes the capability of a substance to be transferred to the gaseous state. Eollowing the study of Wania and Mackay [40], the efficiency of POP condensation with subcooled liquid pressure (p°L) at 25°C above 1 Pa is very low. POPs with a vapor pressure between 1 and 10" Pa are condensed at a temperature of about -30°C and their deposition may be expected mostly in the polar latitudes. POPs with a vapor pressure of subcooled liquid from 10" to 10" Pa are condensed at a temperature above 0°C and they may reach to the middle latitudes. EinaUy, POPs of low volatility with a vapor pressure of subcooled liquid below 10" Pa are practically not vaporized and these substances may be transported and deposited as fine aerosols or coarse particles [39]. Using the vapor pressure of the subcooled liquid it is possible to characterize the partitioning of a POP between the gas phase and the solid phase of the atmospheric aerosol. The POPs having a lower vapor pressure are better bound with... 

Divers get the bends. Divers can get the bends from nitrogen gas bubbles in their blood. Assume that blood is largely water. The Henry s law constant for N > in water at 23 C is 8(),0()0 atm. The hydrostatic pressure is 1 atm at the surface oi a body of water and increases by approximately 1 atm for every 33 feet in depth. Calculate the N i solubility in the blood as a function of depth in the water, and explain why the bends occur. 

The rise in atmospheric carbon dioxide results in higher concentrations of dissolved carbon dioxide in natural waters. Use Henry s law and the data in Table 3.2 to calculate the solubility of CO2 in water at 25°C when its partial pressure is (a) 4.0 kPa and (b) 100 kPa. 

For example. Clever et al. [4] show for the solubility of mercury in water at 298 K that if the measure of concentration is the mol fraction of mercury in the water, the Henry s law value sH=4.7 x 10" kPa. The same source also shows the values for the concentration being expressed in mol/kg. Another common way is to choose the concentration variable as moFm. ... 

The hydrogencarbonate ion, produced in nature by this reaction, is one of the main causes of temporary hardness in water. Carbon dioxide is fairly soluble in water, 1 cm dissolving 1.7 cm of the gas at stp. The variation of solubility with pressure does not obey Henry s law, since the reaction... 

Hydrogen Chloride—Water System. Hydrogen chloride is highly soluble in water and this aqueous solution does not obey Henry s law at ah concentrations. Solubhity data are summarized in Table 5. The relationship between the pressure and vapor composition of unsaturated aqueous hydrochloric acid solutions is given in Reference 12. The vapor—Hquid equiHbria for the water—hydrogen chloride system at pressures up to 1632 kPa and at temperatures ranging from —10 to +70° C are documented in Reference 13. 

Hydrogen Chloride-Organic Compound Systems. The solubihty of hydrogen chloride in many solvents follows Henry s law. Notable exceptions are HCl in polyhydroxy compounds such as ethylene glycol (see Glycols), which have characteristics similar to those of water. Solubility data of hydrogen chloride in various organic solvents are Hsted in Table 10. 

The solubilities of the various gases in [BMIM][PFg] suggests that this IL should be an excellent candidate for a wide variety of industrially important gas separations. There is also the possibility of performing higher-temperature gas separations, thanks to the high thermal stability of the ILs. For supported liquid membranes this would require the use of ceramic or metallic membranes rather than polymeric ones. Both water vapor and CO2 should be removed easily from natural gas since the ratios of Henry s law constants at 25 °C are -9950 and 32, respectively. It should be possible to scrub CO2 from stack gases composed of N2 and O2. Since we know of no measurements of H2S, SO, or NO solubility in [BMIM][PFg], we do not loiow if it would be possible to remove these contaminants as well. Nonetheless, there appears to be ample opportunity for use of ILs for gas separations on the basis of the widely varying gas solubilities measured thus far. 

An existing lO-in. I.D. packed tower using 1-inch Berl saddles is to absorb a vent gas in water at 85°F. Laboratory data show the Henry s Law expression for solubility to be y = 1.5x, where y is the equilibrium mol fraction of the gas over water at compositions of x mol fraction of gas dissolved in the liquid phase. Past experience indicates that the Hog for air-water system will be acceptable. The conditions are (refer to Figure 9-68). 

The Henry s law constant for the solubility of radon in water at 30°C is 9.57 X 10-6 Mlmm Hg. Radon is present with other gases in a sample taken from an aquifer at 30°C. Radon has a mole fraction of 2.7 X 10-6 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. 

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