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.