SDS Volume (2838)

Volume 62. Carbon Dioxide in Water and Aqueous Electrolyte Solutions, p None

Original Measurements

Rumpf, B.; Maurer, G.; Ber. Bunsenges. Phys. Chem. 1993, 97, 85-97.

Variables:

Room Temp: 313.13 - 433.18 $\pu{K}$
Pressure: 0.0181 - 9.868 $\pu{MPa}$
Molality (2): m₂/mol kg^-1 = near 2.00 and 4.00 mol/kg

Prepared by:

H.L. Clever

Method/Apparatus/Procedure:

The apparatus is a modification of one used in earlier work [1]. It consists of a high pressure optical cell, thermostat, magnetic stirrer, thermocouples and $\ce{Pt}$ resistance thermometer, pressure transducers and tanks for aqueous solutions, rinse water and solute gas. The thermostatted about 30 mL high pressure optical cell is filled with carbon dioxide. Pressure and temperature of the gas are measured after equilibration. A known amount of aqueous solvent is added which is slightly greater than that needed to completely dissolve the gas. The pressure in the cell is reduced step-wise by removing very small amounts of the liquid until the first stable bubble appears. The mass of carbon dioxide is calculated from the Bender equation (2). The volume of the cell is known within 0.06 mL. The solvent density is from the literature.

Source and Purity of Materials:

1. Carbon dioxide. Messer Griesheim, Ludwigshafen, > 99.995 mol%, used as received.
2. Ammonium sulfate. Merck GmbH, Darmstadt, > 99.5 mass%. Degassed and dried under vacuum.
3. Water. Deionized and degassed by vacuum distillation.

Estimated Errors:

Ambient temperature: δT/K = ±0.1
Mass concentration (m/v) (1): δm₂/m₂ = ±0.003
δm₁/m₁ = ±0.1 to 0.03

References

¹ Rumpf, B.; Maurer, G.; Fluid Phase Equilib. 1992, 81, 241-60.
² Bender, E.; 5th Proc. Symp. Thermophys. Prop., ASME, NY, 1970, 227-35.