Henry's constants for phenol over its diluted aqueous solution

Abstract

229for silver sulfate and silver acetate (Table VI) is positive and passes through a maximum at X,,, = 0.45 with LX = 5.8 and 5.1, respectively. Thus an increase of 3.0 and 3.7 moles of AN occurs in the case of dioxane + AN mixtures for silver sulfate and silver acetate and an increase of 5.8 and 5.1 moles of Me,SO occurs in the case of dioxane + Me,SO for silver sulfate and silver acetate, respectively, per faraday, relative to the mean molar velocity of the solvent mixtures as reference (23) in the cathode compartment when the solutions of these salts are electrolyzed at the given composition of the solvent mixtures. The enrichment of AN or Me,SO in the cathode compartment arises largely through their transport by the silver ion while the anion transports dioxane in the opposite directlon, i.e., toward the anode. These two effects add together and thus a heteroselective solvation results in large A values. These results support the conclusions based on the transfer energy variation of the ions observed earlier.Henry's constants for phenol over its aqueous solutlon were measured In the temperature range from -2 to 27 OC. An equation was proposed to correlate these data and those estimated from the lllerature data at 44-90 OC.

Henry's law constant measurements for phenol, o-, m-, and p-cresol as a function of temperature

“…The previous temperature dependence recommended by Janini and Quaddora (1986) is probably suspicious because their determination at 293 K are much lower than all the other reported values for the four studied compounds. For phenol and o-cresol, our temperature dependence d(lnHLC)/d(1/T) agrees reasonably with the previous determinations (Parsons et al, 1971;Abd-El-Bary et al, 1986;Harrison et al, 2002).…”

“…Concerning phenol, our value at 293 K is in quite good agreement with that determined by Tremp et al (Tremp et al, 1993) using a Stripping Column Technique (see table 5) and with that of Sheikheldin et al, 2001. Our experimental data are also quite consistent with the average value of 9206 M atm -1 derived at 278 K from simultaneous measurements of the phenol concentration in gas and aqueous phases . However, our values are between 2 and 5 times lower than the previous ones (Parsons et al, 1971;Abd-El-Bary et al, 1986;Sheikheldin et al, 2001;Harrison et al, 2002) as shown in figure 4. On the contrary, the value reported by Janini and Quaddora (1986) at 296 K is approximately 4 times lower than our own determination.…”

Activity Coefficients of Chlorophenols in Water at Infinite Dilution

“…The comparison with the data obtained for phenol by Moore et al (1995), Dohnal and Fenclova (1995), Hakuta (1975), and Abd-el- Bary et al (1986) is given in Figure 1. The agreement is good.…”

“…A property enabling the prediction of the solubility behavior of chemicals in the environment is the activity coefficient in dilute aqueous solutions. The data for phenol were measured by several authors (Moore et al, 1995;Dohnal and Fenclova, 1995;Hakuta, 1975;Abd-el-Bary et al, 1986). There is a lack of measurements for the activity coefficients of chlorinated phenols in aqueous solutions.…”

Standard partial molal properties of aqueous alkylphenols and alkylanilines over a wide range of temperatures and pressures

“…Bernauer et al (2006) recently reported highly reliable k H values for aniline that are the result of a simultaneous treatment of new vapor-liquid equilibrium and calorimetric data. Other values for phenol were measured by Abd-El- Bary et al (1986) using the inert gas stripping method and by Tabai et al (1997) using ebulliometry. In the latter reference are reported both the Henry's law constants and limiting activity coefficients.…”