Solubility of Carbon Dioxide in Aqueous Solutions Containing Acetic Acid or Sodium Hydroxide in the Temperature Range from 313 to 433 K and at Total Pressures up to 10 MPa

Abstract

The solubility of carbon dioxide in aqueous solutions containing acetic acid and in aqueous solutions containing sodium hydroxide was measured in the temperature range from 313 to 433 K and total pressures up to 10 MPa. The molalities of acetic acid or sodium hydroxide in the liquid phase were about 4 and 1 mol/kg, respectively. Experimental results are reported and compared to correlations and predictions.

Solubility of ammonia in liquid mixtures of (water+methanol)

“…It is a continuation of recent research that dealt with (a) the solubility of carbon dioxide in pure water, in a purely organic solvent (methanol) and in liquid mixtures of water and that organic solvent, without as well as with a single strong electrolyte [1][2][3][4][5][6][7][8][9] and (b) with the solubility of ammonia in pure water and in aqueous solutions of some single strong electrolytes, as well as in pure methanol [10][11][12][13][14][15]. It will be extended in future work to the influence of some single strong electrolytes on the solubility of ammonia in liquid mixtures of (water + methanol) as well as to the simultaneous solubility of the reacting gases carbon dioxide and ammonia in such aqueous organic solutions.…”

The applicability of activities in kinetic expressions: A more fundamental approach to represent the kinetics of the system CO2–OHHaubrock1, Hogendoorn2, Versteeg3 2007Chemical Engineering Science430250View full textAdd to dashboardCite

“…Nevertheless, the VLE model where only sodium hydroxide and CO 2 are present has been validated with data taken from Rumpf et al (1998). The current thermodynamic model predicts the experimentally determined overall pressures within an error of 6% if low pressure values (< 1 bar) are excluded (Fig.…”

“…Nevertheless the shape of the curves is not altered by the unequal ionic strength. Looking at the structure of the equations used in the Pitzer approach (see Rumpf et al, 1998) and keeping in mind that "only" the interaction parameter 0 (see Table A5) is employed to calculate the activity coefficients of CO 2 , it could be expected that the shape of the curve would barely change.…”

“…The semi-empirical Pitzer model has been successfully applied by a number of authors (Engel, 1994;Rumpf et al, 1998;van der Stegen et al, 1999) for the description of different electrolyte systems.…”

“…This avoids the use of triple or quadruple interaction parameters which are very scarcely reported in the open literature whereas for the most common single electrolytes binary interaction parameters are readily available. In the extended Pitzer equation, which is described in more detail by Rumpf et al (1998), the ion-ion binary interaction parameters 0 i,j and 1 i,j as well as the ternary interaction parameter i,j,k are characteristic for each aqueous single electrolyte solution. These parameters are solely determined by the properties of the pure electrolytes.…”