IUPAC-NIST Solubilities Database

IUPAC-NIST Solubility Database
NIST Standard Reference Database 106

Solubility System: Carbon dioxide with Ammonium sulfate, Sodium sulfate and Water

Components:
   (1) Sodium sulfate; Na2SO4; [7757-82-6]  NIST Chemistry WebBook for detail
   (2) Ammonium sulfate; (NH4)2SO4; [7783-20-2]  NIST Chemistry WebBook for detail
   (3) Carbon dioxide; CO2; [124-38-9]  NIST Chemistry WebBook for detail
   (4) Water; H2O; [7732-18-5]  NIST Chemistry WebBook for detail

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

Variables:
   Temperature = 313.17 K to 433.16 K
   Pressure = 313.17 K to 433.16 K
   Concentration = m₂/mol kg^-1 = m₃/mol kg^-1 = 1.003

Prepared By:
   H.L. Clever

Experimental Remarks:

   The authors estimated the solubility of carbon dioxide in the multicomponent electrolyte system from the results of the carbon dioxide solubility in the single electrolyte aqueous solutions. The authors approach and approximation used are outlined in the paper.

Experimental Data:   (Subscripts 1,2,3, ..., in column headings refer to components 1,2,3, ...)

System CO₂ (1) + (NH₄₂SO₄(2) + Na₂SO₄(3) + H₂O (4)
T/K	Pressure [MPa]	Molality m₁ [mol/kg]	Molality m₂ [mol/kg]	Molality m₃ [mol/kg]
313.17	0.0084	0.0	1.003	1.003
313.19	0.504	0.0502	1.003	1.003
313.19	1.098	0.1041	1.003	1.003
313.18	2.341	0.2087	1.003	1.003
313.19	3.803	0.3160	1.003	1.003
313.18	5.543	0.4231	1.003	1.003
313.18	8.263	0.5323	1.003	1.003
333.19	0.0177	0.0	1.003	1.003
333.19	0.703	0.0506	1.003	1.003
333.19	1.468	0.1039	1.003	1.003
333.18	3.169	0.2089	1.003	1.003
333.19	5.155	0.3128	1.003	1.003
333.19	7.802	0.4187	1.003	1.003
333.18	8.561	0.4446	1.003	1.003
333.17	9.673	0.4704	1.003	1.003
353.15	0.0415	0.0	1.003	1.003
353.20	0.940	0.0526	1.003	1.003
353.19	1.855	0.1047	1.003	1.003
353.20	4.007	0.2104	1.003	1.003
353.16	6.570	0.3152	1.003	1.003
353.14	8.142	0.3696	1.003	1.003
393.08	0.1833	0.0	1.003	1.003
393.14	1.300	0.0522	1.003	1.003
393.13	2.555	0.1048	1.003	1.003
393.14	5.221	0.2098	1.003	1.003
393.14	8.257	0.3145	1.003	1.003
413.16	0.3388	0.0	1.003	1.003
413.15	1.531	0.0541	1.003	1.003
413.15	1.571	0.0527	1.003	1.003
413.15	2.844	0.153	1.003	1.003
413.15	5.686	0.2109	1.003	1.003
413.15	8.967	0.3174	1.003	1.003
413.16	8.987	0.3172	1.003	1.003
433.16	0.5808	0.0	1.003	1.003
433.16	1.845	0.0523	1.003	1.0035
433.14	1.876	0.0523	1.003	1.003
433.14	3.146	0.1043	1.003	1.003
433.14	4.540	0.1569	1.003	1.003
433.13	6.017	0.2094	1.003	1.003
433.15	7.598	0.2622	1.003	1.003
433.15	9.104	0.3129	1.003	1.003

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 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 stepwise 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 %.
   (3) Sodium sulfate. Riedel de Haen AG, Seelze, > 99 mass %. Degassed and dried under vacuum.
   (4) Water. Deionized and degassed by vaccum distillation.

Estimated Errors:
   Solubility: δm₂/m₂ = δm₃/m₃ = ± 0.003
δm₁/m₁ = ± 0.01 to 0.03
   Temperature: δT/K = ± 0.1

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.