IUPAC-NIST Solubility Database
NIST Standard Reference Database 106

Glass Ball as Bullet Solubility System: Tribromomethane (bromoform) with Water

   (1) Water; H2O; [7732-18-5]  NIST Chemistry WebBook for detail
   (2) Tribromomethane (bromoform); CHBr3; [75-25-2]  NIST Chemistry WebBook for detail

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

Critical Evaluation:

The tribromomethane (1) and water (2) binary system is discussed in two parts; part 1 is tribromomethane (1) in water (2) and part 2 is water (2) in tribromomethane (1).

Part 1. All the available data for the solubility of tribromomethane (1) in water (2) were considered acceptable for use in the smoothing equation except the following reported values. The datum of Squire and Caines (ref. 1) is rejected because of the lack of details on the purity of the sample, method of the experimental work, and significant deviation from other measurements. The approximate value of Booth and Everson (ref. 2) is also rejected because it is significantly lower than later studies. The datum of McNally and Grob (ref. 3) is rejected because the reported solubility is rather higher than other determinations. The data of Wright et al. (ref. 4) are contrary to the general trend of the temperature dependence of the solubilities in water (formation of maximum) and are rejected.

The remaining data, mainly at 298 K, are in reasonable agreement although further studies are required before any values can be recommended without qualification.

The tentative solubility values in mass per cent for tribromomethane (1) in water (2) over the 283 to 303 K temperature range were used to obtain the following equation:

Solubility [100 w1] = 2.371 – 0.01517 (T/K) + 2.7808 × 10-5 (T/K)2

This regression equation was established using the combined data from (refs. 5 - 12), which yielded a standard deviation of 1.6 × 10–2.

The tentative solubility values in mass per cent at 5 K intervals for tribromomethane (1) in water (2) are presented in the Table 1.

The curve obtained from the smoothing equation is shown in Figure 1. It should be noted that the solubility minimum, which is discussed in the Preface, appearing in the 283 to 303 K temperature interval is not pronounced.

Part 2. The only datum available for the solubility of water (2) in tribromomethane (1) is that of Mackay et al. (ref. 9); therefore, no Critical Evaluation is possible. The interested reader is referred to the relevant Compilation Sheet for the experimental solubility.

Experimental Data:   (Notes on the Nomenclature)

t/°CT/K102 * Mass Fraction w1104 * Mole Fraction x1
View Figure 1 for this Evaluation

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

   1  Squire, P.W.; Caines, C.M., Pharm. J. 1905, 74, 784-6.
   2  Booth, H.S.; Everson, H.E., Ind. Eng. Chem. 1948, 40, 1491-3.
   3  McNally, M.E.; Grob, R.L., J. Chromatogr. 1984, 284, 105-16.
   4  Wright, D.A.; Sandler, S.I.; DeVoll, D., Environ. Sci. Technol. 1992, 26, 1828-31.
   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  O'Connell, W.L., Trans. Am. Inst. Mech. Eng. 1963, 226, 126-32.
   8  Symons, J.M., et al. Treatment Techniques for Controlling Trihalomethanes in Drinking Water, U. S. EPA Report 600/2-81-156, Cincinnati, OH., 1981.
   9  Mackay, D. et al. Volatilization of Organic Pollutants from Water, U. S. EPA Report 600/2-82-019, Athens, Georgia, 1982, (PB 82-230939).
   10  Nicholson, B.C.; Maguire, B.P.; Bursill, D.B., Environ. Sci. Technol. 1984, 18, 518-21.
   11  Munz, C.D., Ph. D. Thesis, Stanford University, Stanford, CA., 1985, 306 pp.
   12  Warner, H.P.; Cohen, J.M.; Ireland, J.C., Determination of Henry's Law Constants of Selected Priority Pollutants, U. S. EPA Technical Report, PB87-212684, Cincinnati, OH., July 1987.