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 × 102 (T/K) + 5.45647 × 105 (T/K)2,
which shows a standard deviation of 3.72 × 102 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 × 102 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.