Some Equilibrium Relations in the System Magnesium Oxide—Sulfur Dioxide—Water (Acid Region) at Pressures below Atmospheric<sup>1</sup>

Conrad, Frank; Beuschlein, W. L.

doi:10.1021/ja01186a056

Cited by 8 publications

(4 citation statements)

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“…The solubility of MgSO3 increases with increasing SO2 content in the solutio Figure 3 shows experimental data as well as a correlation of literature data of the solu of magnesium sulfite over the SO2 content in the solution at 25 °C [2,11]. 3)).…”

Section: Influence Of So2 On Solubility Of Mgso3 Hydratesmentioning

confidence: 76%

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Weiß

Harasek

2020

Processes

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This review studies unwanted precipitation reactions, which can occur in SO2 absorption processes using a magnesium hydroxide slurry. Solubility data of potential salts in the MgO-CaO-SO2-H2O system are evaluated. The reviewed data can serve as a reliable basis for process modeling of this system used to support the optimization of the SO2 absorption process. This study includes the solubility data of MgSO3, MgSO4, Mg(OH)2, CaSO3, CaSO4, and Ca(OH)2 as potential salts. The solubility is strongly dependent on the state of the precipitated salts. Therefore, this review includes studies on the stability of different forms of the salts under different conditions. The solubility data in water over temperature serve as a base for modeling the precipitation in such system. Furthermore, influencing factors such as pH value, SO2 content and the co-existence of other salts are included and available data on such dependencies are reviewed. Literature data evaluated by the International Union of Pure and Applied Chemistry (IUPAC) are revisited and additional and newer studies are supplemented to obtain a solid base of accurate experimental values. For temperatures higher than 100 °C the available data are scarce. For a temperature range from 0 to 100 °C, the reviewed investigations and data provide a good base to evaluate and adapt process models for processes in order to map precipitations issues accurately.

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Section: Influence Of So2 On Solubility Of Mgso3 Hydratesmentioning

confidence: 76%

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Weiß

Harasek

2020

Processes

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“…Calculations of the parameter u wgry Q using experimental data obtained by Conrad and Brice [7] allow one to prepare Fig. 4 similar that presented in Fig.…”

Section: Resultsmentioning

confidence: 94%

Sulphur Dioxide Solubility in Aqueous Solutions of Calcium or Magnesium Sulphites

Michalski¹

2000

Chem. Eng. Technol.

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“…The model has been verified by comparing its predictions with experimental data (7)(8)(9)(10)(11)(12)(13)(14)(15) in the ranges: S02 partial pressure = 10-4 to 1 atm, pH = 3.0-6.5, fraction magnesium sulfite saturation = 0-1:0, MgSC>4 molality = 0-1.0, and Mg(HS03)2 molality = 0-4.0.…”

Section: Model Verificationmentioning

confidence: 94%

“…The design and operation of such magnesia-based scrubbing processes require an understanding of the liquor chemistry. Experimental data are available for sulfur dioxide partial pressure, pH, and magnesium sulfite solubility in some aqueous magnesium-sulfite-sulfate solutions (7)(8)(9)(10)(11)(12)(13)(14)(15). The chemical model described here predicts equilibria.…”

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confidence: 99%

Equilibriums for magnesia wet scrubbing of gases containing sulfur dioxide

Rowland¹,

Abdulsattar²

1978

Environ. Sci. Technol.

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H A chemical model is described that predicts thermodynamic equilibria for aqueous magnesium-sulfite-sulfate solutions in the range 15-60 "C. If three of the following variables are specified, then the other three are predicted: partial pressure of sulfur dioxide, pH, degree of saturation with solid magnesium sulfite hexahydrate, molality of dissolved magnesium, molality of dissolved sulfite, and fraction of dissolved sulfur species oxidized to sulfate. Published experimental data are used to test the model. The model predicts that the solubility of magnesium sulfite hexahydrate is independent of liquor composition for dissolved mole ratios of sulfite to active magnesium between 1.0 and 2.0, and that the solubility increases with increasing temperature. A simple set of correlations derived from the model predicts liquor composition and sulfur dioxide partial pressure for solutions saturated with magnesium sulfite.A variety of wet sulfur dioxide (S02) scrubbing processes using magnesium have been applied or proposed (1-6). The design and operation of such magnesia-based scrubbing processes require an understanding of the lic,uor chemistry. Experimental data are available for sulfur dioxide partial pressure, pH, and magnesium sulfite solubility in some aqueous magnesium-sulfite-sulfate solutions (7-15). The chemical model described here predicts equilibria. The model can be simplified for solutions saturated with magnesium sulfite hexahydrate (MgS03~6H20); for this special case, a set of correlations derived from the model predicts liquor composition and SO2 partial pressure. The model has also been used to prepare parametric plots. Variables i n the ModelIn the formulation employed here for the Mg-SOZ-SO3system, there are 13 species: H+, Mg2+, SO,'-, HSO;, SO,(aq), SO:-, MgSOg, MgSO:, OH-, MgOH+, H20(1), SOz(g), andOther species that were considered but not retained in the model are HSO,, MgHSO;, and MgS03-3H20(s). Use of a value of 0.0104 for the dissociation constant of HSO; at 25 "C (16) indicated that dissociation is complete for magnesia-SO2 scrubbing. The ion complex MgHS0; had no significance in explaining experimental data. The hexahydrate solid form of MgS03 is thermodynamically stable, or lower in solubility than trihydrate, at temperatures as high as 59 "C (17). Although trihydrate solid is occasionally encountered at temperatures of 50-60 "C ( I ) , it is assumed here that compositions of liquors saturated with MgS03 at temperatures below 60 "C are adequately predicted from hexahydrate solubilities.The activity coefficients of the three minor ionic species included in the modei, X+, OH-, and MgOH+, are arbitrarily set equal to unity, because the concentrations of these species are too low to affect the ionic and mass balances. The equations given below to describe the system determine the activity of each of these minor species.The individual activity coefficients of the neutral dissolved species SOAaq), MgSO:, and MgSO! are also set equal to unity because data for such coefficients are scarce and repo...

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Some Equilibrium Relations in the System Magnesium Oxide—Sulfur Dioxide—Water (Acid Region) at Pressures below Atmospheric¹

Cited by 8 publications

References 0 publications

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Sulphur Dioxide Solubility in Aqueous Solutions of Calcium or Magnesium Sulphites

Equilibriums for magnesia wet scrubbing of gases containing sulfur dioxide

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Some Equilibrium Relations in the System Magnesium Oxide—Sulfur Dioxide—Water (Acid Region) at Pressures below Atmospheric1

Cited by 8 publications

References 0 publications

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Solubility Data of Potential Salts in the MgO-CaO-SO2-H2O-O2 System for Process Modeling

Sulphur Dioxide Solubility in Aqueous Solutions of Calcium or Magnesium Sulphites

Equilibriums for magnesia wet scrubbing of gases containing sulfur dioxide

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Some Equilibrium Relations in the System Magnesium Oxide—Sulfur Dioxide—Water (Acid Region) at Pressures below Atmospheric¹