IUPAC-NIST Solubility Database
NIST Standard Reference Database 106

Glass Ball as Bullet Solubility System: 1,2-Dibromoethane with Water.

   (1) 1,2-Dibromoethane; C2H4Br2; [106-93-4]  NIST Chemistry WebBook for detail
   (2) Water; H2O; [7732-18-5]  NIST Chemistry WebBook for detail

   A. L. Horvath, Imperial Chemical Industries Limited, Runcorn, U.K.

Critical Evaluation:

        The 1,2-dibromoethane (1) and water (2) binary system is treated in two parts; part 1 is 1,2-dibromoethane (1) in water (2) and part 2 is water (2) in 1,2-dibromoethane (1).
     Part 1. The solubility of 1,2-dibromoethane (1) in water (2) has been studied by 14 groups of workers in the temperature range from 273.15 to 348.15 K. The datum of Booth and Everson1 is noticeably higher than the likely solubility and is rejected. Similar conclusions were found for the poor reliability of other solubility data (see e. g., CCl4, CHBr3, CHCl3, CH2Cl2, and CH2Br2), which justifies the rejection of these data. The measurements of Wade2 and Dreisbach3 are significantly lower than the solubility values calculated from the smoothing equation and are also rejected. The temperature dependence of the solubility data of Howe et al.4 contradicts that of all other measured data and therefore the datum at 303.15 K is rejected.
     The remaining data from the other ten laboratories were compiled or used for the smoothing equation. The combined data values of Gross and Saylor,5 van Arkel and Vles,6 Shostakovsky and Druzhinin,7 Druzhinin and Shostakovsky,8 Chitwood,9 Call,10 O'Connell,11 Chiou and Freed,12 Mackay et al.,13 and Tokoro et al.14 were used to obtain the following mass percent (1) equation:

Solubility [100 w1] = 3.8651 – 2.7921 × 10–2 (T/K) + 5.45647 × 10–5 (T/K)2,

which shows a standard deviation of 3.72 × 10–2 in the temperature range from 273 to 348 K.
     The measurements and the curve obtained from the smoothing equation are shown in Fig. 17. The curve obtained from the smoothing equation shows no minimum over the temperature interval under examination.  Additional details concerning the appearance of a solubility minimum in most aqueous halogenated hydrocarbon systems within the temperature interval of 270-320 K are provided in the Preface.
     The tentative values of solubility at 5 K intervals for 1,2-dibromoethane (1) in water (2) are presented in Table 1.

     Part 2. The solubility of water (2) in 1,2-dibromoethane (1) has been reported by six groups of workers in the temperature range from 288 to 348 K with partially consistent results. The solubility data of Shostakovsky and Druzlinin7 are significantly higher than all other measurements and are therefore rejected. These data are an order of magnitude too high. The datum of Mackay et al.13 is several per cent lower than other results and is also rejected.
     The remaining data of Bell,15 Staverman,16 Hutchison and Lyon,17 and O'Connell11 were used for data smoothing. The fitting equation used was:

log10 x2 =  0.75213 – 868.78/(T/K),

which gave a standard deviation of 5.19 × 10–2 in the narrow temperature range from 288 to 303 K. The tentative solubility values at 5 K intervals for water (2) in 1,2-dibromoethane (1) are presented in Table 2.
     Measured values and the linear relationship between the solubility expressed as log10 x2 versus 1/(T/K) are plotted in Fig. 18. This linear relationship is a characteristic of water solubility in halogenated hydrocarbons. The phenomenon is discussed in some detail in the Preface.

Experimental Data:   (Notes on the Nomenclature)

Table 1. Tentative solubility of 1,2-dibromoethane (1) in water (2)
t/°CT/K102 * Mass Fraction w1104 * Mole Fraction x1
Table 2. Tentative solubity of water (2) in 1,2-dibromoethane (1)
t/°CT/K102 * Mass Fraction w2103 * Mole Fraction x2
View Figure 1 for this Evaluation

View Figure 2 for this Evaluation

References: (Click a link to see its experimental data associated with the reference)

   1  Booth, H.S.; Everson, H.E., Ind. Eng. Chem. 1948, 40, 1491-3.
   2  Wade, P., J. Sci. Food Agric. 5, 184-92 (1954).
   3  Dreisbach, R.R., "Physical Properties of Chemical Compounds," Advances in Chemistry Series No. 22; American Chemical Society: Washington, D.C., 1959; pp. 208-214.
   4  Howe, G.B.; Mullins, M.E.; Rogers, T.N., AFESC Tyndall Air Force Base, Report ESL-TR-86-66, Vol. 1, Florida, Sept. 1987, 86 pp. (AD-A188 571).
   5  Gross, P.M.; Saylor, J.H., J. Am. Chem. Soc. 1931, 53, 1744-51.
   6  van Arkel, A.E.; Vles, S.E., Recl. Trav. Chim. Pays-Bas 1936, 55, 407-11.
   7  Shostakovskii, M.F.; Druzhinin, I.G., Zh. Obshch. Khim. 12, 42-7 (1942).
   8  Druzhinin, I.G.; Shostakovskii, M.F., J. Gen. Chem. USSR 12, 48-54 (1942).
   9  Chitwood, B.G., Adv. in Chem. Ser., Am. Chem. Soc., 1952, 7, 91-9.
   10  Call, F., J. Sci. Food Agric. 8, 630 (1957).
   11  O'Connell, W.L., Trans. Am. Inst. Mech. Eng. 1963, 226, 126-32.
   12  Chiou, C.T.; Freed, V.H., "Chemodynamic Studies on Bench Mark Industrial Chemicals"; National Technical Information Service: Springfield, Virginia, 1977; PB-274263.
   13  Mackay, D. et al. Volatilization of Organic Pollutants from Water, U. S. EPA Report 600/2-82-019, Athens, Georgia, 1982, (PB 82-230939).
   14  Tokoro, R.; Bilewicz, R.; Osteryoung, J., Anal. Chem. 58, 1964 (1986).
   15  Bell, R.P., J. Chem. Soc. 1932, 2905-11.
   16  Staverman, A.J., Recl. Trav. Chim. Pays-Bas 1941, 60, 836-41.
   17  Hutchinson, C.A.; Lyon, A.M., Columbia University Report A-745, July 1, 1943.