IUPAC-NIST Solubility Database
NIST Standard Reference Database 106

Glass Ball as Bullet Solubility System: 1,1,2,3,3,3-Hexachloro-1-propene with Water

   (1) Water; H2O; [7732-18-5]  NIST Chemistry WebBook for detail
   (2) 1,1,2,3,3,3-Hexachloro-1-propene; C3Cl6; [1888-71-7]  NIST Chemistry WebBook for detail

   A. L. Horvath, Imperial Chemical Industries Limited, Runcorn, U.K., July 1993.

Critical Evaluation:

         The 1,1,2,3,3,3-hexachloropropene (1) and water (2) binary system is treated in two parts; part 1 is 1,1,2,3,3,3-hexachloropropylene (1) in water (2) and part 2 is water (2) in 1,1,2,3,3,3-hexachloropropene (1).

       Part 1. The solubility of 1,1,2,3,3,3-hexachloropropene (1) in water (2) has been studied by three work groups in the temperature range from 288 to 313 K. The data of Dreisbach 1 and of Simonov et al. 2 were reported at only a single temperature, that is, at 298.15 and 313.15 K, respectively. The temperature dependence of solubility was measured by Antropov et al.3 in the narrow temperature interval between 288.15 and 299.15 K.

      The data are in very poor agreement and in the absence of other independent studies, it is not possible to determine which values are more reliable. Further studies will be necessary before even tentative values can be prescribed. All reported experimental solubility values in weight percent and mole fraction are summarized in Table 4.

      Part 2. The solubility of water (2) in 1,1,2,3,3,3-hexachloropropene (1) between 288 and 323 K has been measured by five groups of researchers. The measured solubility of Dreisbach1 is markedly higher than all other studies and is therefore rejected. The remaining solubility data originated from workers of the same organization over a number of years.2-5 The solubility data were reported at different temperatures, except for the value at 299.15 K. The data are in good agreement and they were used for the smoothing equation of mole fraction solubility of water in 1,1,2,3,3,3-hexachloropropene between 288 and 323 K:

log10x2 = 2.2310 - 1604.19/(T/K).

This equation, representing the combined data, yielded a standard deviation of 2.38x10-2. The linear relation between the solubility expressed as log10x2 versus the reciprocal of absolute temperature is illustrated in Fig. 2.. The straight line behavior of such plots is characteristic of the solubility of water in halogenated hydrocarbons, as discussed in the Preface.

      The tentative solubility values at 5 K intervals for water (2) in 1,1,2,3,3,3-hexachloropropene (1) in weight percent and mole fraction are presented in Table 5.

Experimental Data:   (Notes on the Nomenclature)

Table 4. Reported solubility of 1,1,2,3,3-hexachloropropene (1) in water (2)
T/KReferenceSol. PowerSolubilitySolx10(**)Sol. Notex1 Powerx1
Table 5. Tentative solubility of water (2) in 1,1,2,3,3,3-hexachloropropene
t/°CT/K102 * Mass Fraction w2104 * Mole Fraction x2
View Figure 1 for this Evaluation

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

   1  Dreisbach, R.R., "Physical Properties of Chemical Compounds," Advances in Chemistry Series No. 22; American Chemical Society: Washington, D.C., 1959; pp. 208-214.
   2  Simonov, V.D.; Pogulyai, V.E.; Shamsutdinov, T.M., Russ. J. Phys. Chem. 1970, 44, 1755-7.
   3  Antropov, L.I.; Populyai, V.E.; Simonov, V.D.; Shamsutdinov, T.M., Russ. J. Phys. Chem. 1972, 46, 311-2 (VINITI No. 3739-71).
   4  Simonov, V.D., et al., Dokl. Neftekim. Sekt. Bashkir. Respub. Pravl. Vses. Khim. Obshchest. 1971, 346-51.
   5  Simonov, V.D.; Shamsutdinov, T.M.; Pogulyai, V.E.; Popova, L.N., Russ. J. Phys. Chem. 1974, 48, 1573-5.