Compilation - Benzene with Water (IUPAC SDS Volume 37)
SDS Volume (614)
Volume 37. Hydrocarbons in Water and Seawater, Part I, p 111
Original Measurements
Bohon, R. L.; Claussen, W. F.; J. Am. Chem. Soc. 1951, 73, 1571-8.
Variables:
Room Temp: 0.4 - 42.8 °C
Prepared by:
Method/Apparatus/Procedure:
A round-bottmed flask containing about 4 mL of (1) and 400 mL of (2) was evacuated, suspended in a thermostat, shaken for 24h and then allowed to settle for at least another 24h. Next, desired quantities of the water layer were syphoned into 6 glass-stoppered Erlenmeyer flasks. These 6 flasks had previously been tared, partially filled with a suitable amount of diluent water, and reweighed. Weighed portions of the samples were inserted into a quartz cuvette and measured in a Beckman DU spectrophotometer. Absorbances were corrected for absorption of (1) onto the walls of the cuvette.
Source and Purity of Materials:
- Baker and Adamson, purified by recrystallization from ethanol, washing, filtering through silica gel then distilling. Purity was determined by refractometry (no values given).
- Air-free conductivity water, no other details given.
Estimated Errors:
Ambient temperature: ±0.02°C
Mass concentration (m/v) (1): ±0.5% relative
Components:
- Benzene, $\ce{ C6H6 }$; [71-43-2] NIST WebBook
- Water, $\ce{ H2O }$; [7732-18-5] NIST WebBook
Experimental Data
Solubility of benzene in water
| $T$ (°C) | $x_{1}$ | MR1 (g1/100 g sln) |
|---|---|---|
| 0.4 | 4.01 x 10-4 | 0.174 |
| 5.2 | 4.17 x 10-4 | 0.181 |
| 10.0 | 4.15 x 10-4 | 0.180 |
| 14.9 | 4.10 x 10-4 | 0.178 |
| 21.0 | 4.13 x 10-4 | 0.179 |
| 25.0 | 4.13 x 10-4 | 0.179 |
| 25.6 | 4.13 x 10-4 | 0.179 |
| 30.2 | 4.24 x 10-4 | 0.184 |
| 34.9 | 4.36 x 10-4 | 0.189 |
| 42.8 | 4.61 x 10-4 | 0.200 |
(a) Solubilities of (1) in (2) were reported as "optical density" (absorbance) measurements. Solubilities were calculated by the compiler using the Beer-Lambert law, the stated cell path-length (1 cm) and the authors' "extinction coefficients" (absorptivities) and corrected optical densities. This gave a solubility of g(1)/L sln which was then converted to g(1)/100 g sln by assuming a solution density of 1.00 kg/L.
(b) Data refer to the solubility of solid (1) in (2).
(c) Given in the original paper as 1.79 g(1)/L sln.
