IUPAC-NIST Solubility Database
NIST Standard Reference Database 106


Glass Ball as Bullet Solubility System: Iodomethane with Water

Components:
   (1) Water; H2O; [7732-18-5]  NIST Chemistry WebBook for detail
   (2) Iodomethane; CH3I; [74-88-4]  NIST Chemistry WebBook for detail

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

Critical Evaluation:

   
The solubility of iodomethane (1) in water (2) has been studied by 8 groups of workers; whereas, the solubility of water (2) in iodomethane (1) has not been investigated yet. The experimental data of Glew (ref. 1) covering the 273 to 323 K temperature range are significantly higher than the likely solubility. Furthermore, the continuous decrease in solubility with temperature between 273 and 323 is not consistent with the formation of a minimum shown by most similar binary systems. Therefore, these data are classed as doubtful and are rejected. The presence of a minimum in the solubility versus temperature behavior for the halogenated hydrocarbon-water systems is discussed in the Preface.

The solubility data of Balls (ref. 2) between 283 and 298 K show a continuous rise with temperature which is contrary to the trends shown by all other investigators and are therefore rejected. The single data point of Liss and Slater (ref. 3) at 293 K is lower than other results and is likewise rejected.

The remaining data of Rex (ref. 4), Fühner (ref. 5), van Arkel and Vles (ref. 6), Swain and Thornton (ref. 7), and Hunter-Smith et al. (ref. 8) are in reasonable agreement, although further studies are required before any values can be recommended. The tentative mass per cent solubilities of iodomethane (1) in water (2) over the 273 to 313 K temperature range were used to obtain the following equation:

Solubility [100 w1] = 19.0036 – 0.11723 (T/K) + 1.95356 × 10–4 (T/K)2

This regression equation was established using the combined data from (refs. 4 - 8), which yielded a standard deviation of 4.3 × 10–2.

The tentative mass per cent solubility values at 5 K intervals for iodomethane (1) in water (2) are presented in Table 1. The curve obtained from the smoothing equation is shown in Figure 1. It shows a distinct minimum at 300.0 K, as discussed in the Preface.

Experimental Data:   (Notes on the Nomenclature)

Table 1. Tentative Solubility of Iodomethane (1) in Water (2)
t/°CT/K102 * Mass Fraction w1103 * Mole Fraction x1
0273.151.5572.003
5278.151.5101.942
10283.151.4721.893
15288.151.4441.856
20293.151.4251.831
25298.151.4171.821
30303.151.4181.822
35308.151.4301.838
40313.151.4501.864
View Figure 1 for this Evaluation

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

   1  Glew, D.N., Ph. D. Thesis, University of Cambridge, Cambridge, U. K. 1952, 245 pp.
   2  Balls, P.W., Ph. D. Thesis, Univ. of East Anglia, Norwich, U. K., July 1980, 375 pp.
   3  Liss, P.S.; Slater, P.G., Nature 1974, 247, 181-4.
   4  Rex, A., Z. Phys. Chem. 1906, 55, 355-70.
   5  F├╝hner, H., Ber. Dtsch. Chem. Ges. 1924, 57, 510-15.
   6  van Arkel, A.E.; Vles, S.E., Recl. Trav. Chim. Pays-Bas 1936, 55, 407-11.
   7  Swain, C.G.; Thornton, E.R., J. Am. Chem. Soc. 1962, 84, 822-6.
   8  Hunter-Smith, R.J.; Balls, P.W.; Liss, P.S., Tellus 35B, 170 (1983).