Figure 1 - uploaded by Gerd Maurer
Content may be subject to copyright.
Solubility of ammonia in water. Exptl. results: +, Wilson; 27 ×, Wucherer; 28 0, Clifford and Hunter; 29 3, Mü ller; 30 O, this work. Calculation: s.
Source publication
Experimental results for the solubility of ammonia in 2−6 m aqueous solutions of four single electrolytes (NaCl, NaNO3, CH3COONa, and NaOH) at temperatures from 313 to 393 K and pressures up to about 0.7 MPa are reported. The experimental results are compared to correlations/predictions.
Contexts in source publication
Context 1
... The new data agree with reliable literature data within the experimental uncertainty. A comparison with some selected literature data is shown in Figure 1. ) as well as a ternary (τ NH3,NH3,NH3 ) parameter for interactions between dissolved ammonia molecules. ...
Context 2
... comparison with some selected literature data is shown in Figure 1. ) as well as a ternary (τ NH3,NH3,NH3 ) parameter for interactions between dissolved ammonia molecules. These parameters were determined by Weyrich 25 and Rumpf et al. 26 from literature data on the vapor-liquid equilibrium and the heat of dilution of the binary system NH 3 -H 2 O: Figure 1 shows a comparison between the new experimental data, the results from the correlation by Rumpf et al., 26 and selected literature. [27][28][29][30] The new experimental data agree within the experimental uncertainty with the predictions as well as with most literature data. ...
Similar publications
The electrocatalytic nitrogen reduction reaction (N2RR) in aqueous media has garnered substantial interest as it allows direct conversion of N2 to NH3 under benign reaction conditions. However, the competing hydrogen evolution reaction (HER), strong N≡N bond, sluggish kinetics, and low solubility of N2 in pure water seriously limit the overall N2RR...
Citations
... In calcium carbonate precipitation processes with all additives used, more than 97% of the NH 3 initially introduced into the reaction mixture remains in the solution, higher the 92.5% capture efficiency for the precipitation system without additives (Fig. 4). The NH 3 salting-out effect by the electrolytes is quite obvious for the post-distillation liquid compared with the ammonia solution, because the solubility of NH 3 in water is reduced in the presence of dissolved inorganic salts [40]. Usually, the effect of the salt addition on the solubility has been attributed to the greater attraction between the ions and the water molecules than between the gas molecules. ...
This research aims to investigate the effect of selected organic substances containing hydroxyl groups on the reduction of NH3 escape and the improvement of CO2 capture during the precipitation of calcium carbonate by carbonation method using post-distillation liquid from the Solvay process and gas stream containing CO2 in the amount corresponding to the exhausted gases produced by the combustion of fossil fuels. Glycerol, ethylene glycol (EG), methanol, isopropanol, pentaerythritol, and neopentyl glycol (NPG) were used as ammonia escape inhibitors. The addition of NPG has been shown to result in the highest reduction of NH3 escape (83.1%) and the highest CO2 capture efficiency (86.1%). During the proposed CaCO3 precipitation with NPG, 98.7% of the NH3 initially introduced into the reaction mixture remains in the solution. Furthermore, the features that should be taken into account when introducing various alcohols and polyols for capturing NH3 and CO2 in the calcium carbonate precipitation via the carbonation method have been discussed.
... In practical terms, it would be useful to have information on the change in Henry coefficient as a function of EC L . A large amount of literature exists which describes the solubility of ammonia in various electrolytes in terms of the Pitzer thermodynamic model [14][15][16]. However, the ionic composition of the solution must be known in order to predict the Henry coefficient. ...
From theoretical calculations validated by the results of experiments, it was shown that the properties of the washing liquid that flows into biotrickling filters at livestock facilities determine the maximum ammonia removal efficiency (RE) that can be achieved. For a well-designed biotrickling filter not limited by hydrodynamic conditions, the ammonia driving force is mainly controlled by the pH, and also by the electrical conductivity (ECL), although to a lesser extent. With the washing liquid at a given temperature, therefore, the removal efficiency depends on the gaseous ammonia concentrations to be treated (CGin; usually lower than 20 mgNH3 m⁻³) and on the values of the pair (pH, ECL). Theoretical prediction of the maximum removal efficiency that can be achieved by simply measuring the properties of the washing liquid, in line or from samples, could be a useful diagnostic tool to identify possible failure of the apparatus and to manage the electrical conductivity to guarantee removal efficiency at a desired rate.
... The effective increase in the analytical signal could be explained by the "salting out" effect resulting from the addition of NaCl, which reduced the solubility of molecular ammonia in the standard solution and led to its enhanced evaporation into the head-space [59]. The increase of both the blank and the standard signal could be attributed to an increased evaporation of the drop due to the drying effect exerted by the sample on the head-space. ...
A novel approach to the automation technique Lab-In-Syringe, also known as In-Syringe Analysis, is proposed which utilizes a secondary inlet into the syringe void, used as a size-adaptable reaction chamber, via a channel passing through the syringe piston. This innovative approach allows straightforward automation of head-space single-drop microextraction, involving accurately controlled drop formation and handling, and the possibility of on-drop analyte quantification. The syringe was used in upside-down orientation and in-syringe magnetic stirring was carried out, which allowed homogenous mixing of solutions, promotion of head-space analyte enrichment, and efficient syringe cleaning. The superior performance of the newly developed system was illustrated with the development of a sensitive method for total ammonia determination in surface waters. It is based on head-space extraction of ammonia into a single drop of bromothymol blue indicator created inside the syringe at the orifice of the syringe piston channel and on-drop sensing of the color change via fiber optics. The slope of the linear relationship between absorbance and time was used as the analytical signal. Drop formation and performance of on-drop monitoring was further studied with rhodamine B solution to give a better understanding of the system's performance. A repeatability of 6% RSD at 10 mmol L-1 NH3, a linear range of up to 25 mmol L-1 NH3, and a limit of detection of 1.8 mmol L-1 NH3 were achieved. Study of interferences proved the high robustness of the method towards humic acids, high sample salinity, and the presence of detergents, thus demonstrating the method superiority compared to the state-of-the-art gas-diffusion methods. A mean analyte recovery of 101.8% was found in analyzing spiked environmental water samples.
... Experimental data for the two-component system, NH 3 -H 2 O, in the form of mass fractions of ammonia and the total pressure were obtained from Stephen (1963) and Sing et al. (1999). The performed calculations for the two-component system revealed similar, good accuracy in predictions of the total pressure, P, by all the tested thermodynamic models, see Fig. 1. ...
... Values of partial pressure of water and ammonia for varied molality of sodium chloride and ammonia in aqueous phase were obtained from the experiments of Sing et al. (1999) for the three-component system of NaCl -NH 3 -H 2 O. The calculations were carried out for the temperature of 313 K and molality of NaCl at 4 mol/kg H2O and also for 353 K and NaCl molality of 2 mol/kg H2O . ...
A comparative study of thermodynamic electrolyte models applied to the Solvay soda system
Fast development of computation techniques for electrolyte activities contributed recently to introduction of a few substantial programmes for thermodynamic computing of multiphase systems. The presented study comprises useful information for practical computing using selected thermodynamic models of aqueous electrolyte solutions. Those models enable quantitative description of both phase and ionic equilibria and provide values of activity coefficients. The carried out analysis of individual models involved a comparison of their practical effectiveness features along with problems encountered in evaluation of the coefficients. The authors conclude that for the Solvay soda system the exUNIQUAC model for an in-house code or the MSE model for a commercial one can be used.
... The present work is a continuation of experimental research on (a) the solubilities of the single gases ammonia and carbon dioxide in pure water, in a purely organic solvent (methanol), and in liquid mixtures of water and that organic solvent without or with a single salt and (b) on the simultaneous solubility of those gases in water without or with a single salt. [1][2][3][4][5][6][7][8][9][10][11][12][13][14][15][16][17][18][19] It will be extended in an upcoming contribution to the influence of some single salts on the simultaneous solubility of ammonia and carbon dioxide in liquid mixtures of (water þ methanol). ...
A high-pressure-cell technique based on the analytical method was used to investigate the simultaneous solubility of the chemically reacting gases ammonia and carbon dioxide in solvent mixtures of (water + methanol). Seven (gas-free) solvent compositions were considered (methanol mole fractions of about 0, 0.05, 0.25, 0.5, 0.75, 0.95, and 1). The temperatures were approximately (313, 353, and 393) K. In the isothermal experimental series, carbon dioxide was added stepwise to a cell containing a mixture of (water + methanol + ammonia). The stoichiometric molality of ammonia in the solvent mixture of (water + methanol) was approximately (6 and 12) mol·(kg of solvent mixture)−1. The carbon dioxide loading (i.e., the ratio of the stoichiometric molalities of carbon dioxide and ammonia) ranged up to 1.07. The total pressure ranged up to 5.5 MPa. Vapor−liquid equilibrium data, including partial pressures of all components, are reported.
... CCl 4 and CH 3 Br,Table 1). It is worth noting that the largest deviations are associated with (i) the measurement of NH 3 solubility by Sing et al. (1999), and (ii) the data of Elliott and Rowland (1993). The study by Sing et al. (1999) was conducted at high temperature and extremely high salinity (Note e,Table 1), and is included only to highlight the steep decrease in salting out effect with increasing solubility (in the absence of more appropriate data for soluble gases in addition to the data points for methanal (Zhou and Mopper, 1990) and H 2 O 2 (Bandstra, 2000)). ...
... It is worth noting that the largest deviations are associated with (i) the measurement of NH 3 solubility by Sing et al. (1999), and (ii) the data of Elliott and Rowland (1993). The study by Sing et al. (1999) was conducted at high temperature and extremely high salinity (Note e,Table 1), and is included only to highlight the steep decrease in salting out effect with increasing solubility (in the absence of more appropriate data for soluble gases in addition to the data points for methanal (Zhou and Mopper, 1990) and H 2 O 2 (Bandstra, 2000)). The study by Elliott and Rowland (1993) has been identified by Moore (2000) as underestimating the salting-out effect for CH 3 Cl, and this appears to be supported by the considerably lower value of K H /K H,0 for CH 3 Br compared with that measured by De Bruyn and Saltzman (1997). ...
... The study by Elliott and Rowland (1993) has been identified by Moore (2000) as underestimating the salting-out effect for CH 3 Cl, and this appears to be supported by the considerably lower value of K H /K H,0 for CH 3 Br compared with that measured by De Bruyn and Saltzman (1997). For the above reasons the data of Sing et al. (1999) and Elliott and Rowland (1993) are not included in the data used to fit the model. It is recommended that where reliable data for the solubility of a gas of interest at the required salinity is available, this data should be considered before applying this predictive equa- tion. ...
The ocean-atmosphere flux of a gas can be calculated from its measured or estimated concentration gradient across the air-sea interface and the transfer velocity (a term representing the conductivity of the layers either side of the interface with respect to the gas of interest). Traditionally the transfer velocity has been estimated from empirical relationships with wind speed, and then scaled by the Schmidt number of the gas being transferred. Complex, physically based models of transfer velocity (based on more physical forcings than wind speed alone), such as the NOAA COARE algorithm, have more recently been applied to well-studied gases such as carbon dioxide and DMS (although many studies still use the simpler approach for these gases), but there is a lack of validation of such schemes for other, more poorly studied gases. The aim of this paper is to provide a flexible numerical scheme which will allow the estimation of transfer velocity for any gas as a function of wind speed, temperature and salinity, given data on the solubility and liquid molar volume of the particular gas. New and existing parameterizations (including a novel empirical parameterization of the salinity-dependence of Henry's law solubility) are brought together into a scheme implemented as a modular, extensible program in the R computing environment which is available in the supplementary online material accompanying this paper; along with input files containing solubility and structural data for ~90 gases of general interest, enabling the calculation of their total transfer velocities and component parameters. Comparison of the scheme presented here with alternative schemes and methods for calculating air-sea flux parameters shows good agreement in general. It is intended that the various components of this numerical scheme should be applied only in the absence of experimental data providing robust values for parameters for a particular gas of interest.
... Pitzer's parameters ω W for interactions in water were taken from Sing et al. 2 (for NaCl as dissolved salt) and from Weyrich et al. 4 (for Na 2 SO 4 as dissolved salt). Because the solubility of both NaCl and Na 2 SO 4 in pure methanol is very small, the corresponding parameters ω M for interactions in methanol were neglected; that is, they were set to zero. ...
New experimental results are reported for the influence of two single salts (sodium chloride and sodium sulfate) on the solubility of ammonia in liquid mixtures of water and methanol at 353 and 393 K. The mole fractions of methanol in the (gas-free and salt-free) solvent mixture of water and methanol were about 0.25, 0.5, and 0.75 in the experiments with sodium chloride and about 0.05 and 0.25 in the experiments with sodium sulfate. The molality of the salt varied between about 0.25 and 2 (0.15 and 1) mol/kg of the solvent mixture in the systems with sodium chloride (sodium sulfate). The maximum molality of ammonia was about 6.7 mol/kg of (water + methanol) for both temperatures and for both salts. The maximum total pressure above the liquid solutions was about 0.3 MPa (1 MPa) in the system containing sodium chloride at 353 K (393 K) and about 0.2 MPa (0.7 MPa) in the system with sodium sulfate at 353 K (393 K). The experimental results are used to test a thermodynamic framework which allows the influence of both single strong electrolytes on the solubility of ammonia in liquid mixtures of water and methanol to be predicted. The prediction results are in good agreement with the new experimental data.
... This contribution deals with the 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. ...
New experimental results are reported for the solubility of ammonia in liquid mixtures of (water+methanol). Five (gas-free) solvent compositions are considered (mole fraction of methanol of about 0.05, 0.25, 0.5, 0.75, and 0.95). The temperature amounts to about 313K, 353K, and 393K. The solubility pressure ranges up to about 0.1MPa, 0.6MPa, and 1.6MPa, respectively. The molality of ammonia in the solvent mixture of (water+methanol) (the mole fraction of ammonia in the liquid) ranges up to 13molkg−1 (about 0.3). The experimental results are used to determine Henry's constant of ammonia in the liquid mixtures of (water+methanol). An extension of Pitzer's molality scale-based model for the Gibbs excess energy (to solvent mixtures) is applied in a thermodynamic model to describe the phase equilibrium.
... The solubility of ammonia in aqueous salt-free and saltcontaining solutions was investigated in previous work. 1,2 That research shall be extended to salt-free and salt-containing aqueous/organic solvent systems, where methanol is arbitrarily chosen as the organic compound. The work presented here is restricted to one of the interesting subsystems; it deals with the solubility of ammonia in pure methanol. ...
A high-pressure view-cell technique based on the synthetic method was used to determine the solubility of ammonia in liquid methanol (total pressure at a preset temperature and liquid-phase composition). The solubility pressure ranges up to about 4.2 MPa. The temperature amounts to (313.75, 354.35, and 395.0) K. The molality of ammonia in methanol (the mole fraction of ammonia in the liquid) ranges up to about 66.4 mol·kg-1 (about 0.68). Furthermore, a high-pressure cell technique based on the analytical method was used to investigate the vapor−liquid equilibrium of that same system (equilibrium pressure as well as liquid- and gas-phase compositions at a preset temperature). The solubility pressure ranges up to about 1.6 MPa. The temperature amounts to (353.1 and 393.1) K. The molality of ammonia in methanol (the mole fraction of ammonia in the liquid) ranges up to 13 mol·kg-1 (about 0.3). The experimental results are used to determine Henry's constant of ammonia in methanol. Furthermore, the experimental data are correlated by applying Pitzer's molality scale based equation for the Gibbs excess energy.
... Furthermore, similar work was performed for aqueous solutions of ammonia and sulfur dioxide, 7 ammonia and phosphoric acid, 8 and ammonia and hydrogen sulfide. 9 Additionally, the solubility of the single gases ammonia, 10,11 carbon dioxide, [12][13][14][15][16][17] sulfur dioxide, [18][19][20] and hydrogen sulfide [21][22][23] in aqueous solutions of strong electrolytes was investigated in recent years. The experimental data were used to determine parameters in a thermodynamic framework to describe the simultaneous solubility of ammonia and a sour gas in aqueous electrolyte solutions. ...
... , and τ Na + ,Na + ,NO3 -were taken from Sing et al. 11 ...
... Sing et al. 11 used experimental results for the solubility of ammonia in aqueous solutions of the single strong electrolytes NaCl and NaNO 3 to determine B NH 3 ,MX (0) and Γ NH3,NH3,MX (neglecting Γ NH3,MX,MX ). From eqs 27 and 29, the following binary and ternary interaction parameters are derived from these properties: ...
New experimental results for the simultaneous solubility of ammonia and carbon dioxide in (about 4 m) aqueous solutions of NH4Cl, NH4NO3, and NaNO3 at (313, 353, and 393) K and total pressures up to about 0.7 MPa are reported. The maximum loading of carbon dioxide to ammonia, i.e., the molar ratio of carbon dioxide to ammonia, in the liquid phase was about 1 (at 313 K), about 0.7 (at 353 K), and about 0.3 (at 393 K). The experimental results are used to assess predictions from a thermodynamic model for the solubility of ammonia and sour gases in aqueous solutions of strong electrolytes.
