2000
DOI: 10.1002/1521-4125(200006)23:6<521::aid-ceat521>3.0.co;2-g
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Sulphur Dioxide Solubility in Aqueous Solutions of Calcium or Magnesium Sulphites

Abstract: Based on the physical and chemical equilibria conditions, a model for gaseous sulphur dioxide solubility in a saturated solution of calcium or magnesium sulphites was developed. The dissociation constant of the reaction Ca2++HSO–3CaHSO+3 as a function of temperature is presented. The value of a similar parameter for the system with magnesium sulphite is evaluated as less than 10–2.

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Cited by 5 publications
(7 citation statements)
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“…According to assumptions 2 and 3, the concentration of dissolved SO 2 or CO 2 in the solution is assumed to be the sum of the gas solubility in pure water and the amount converted into an ion pair involving CaHSO 3 or CaHCO 3 . It has to be stressed that the model formulated according to assumption 2 [15] reproduces experimental data very well [14] for systems consisting of SO 2 (with inert gas)-water with CaSO 3 crystals. Considering experimental data [16] for the system consisting of CO 2 (with inert gas)-water with CaCO 3 particles, assumption 3 is also adequate.…”
Section: The Modelmentioning
confidence: 99%
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“…According to assumptions 2 and 3, the concentration of dissolved SO 2 or CO 2 in the solution is assumed to be the sum of the gas solubility in pure water and the amount converted into an ion pair involving CaHSO 3 or CaHCO 3 . It has to be stressed that the model formulated according to assumption 2 [15] reproduces experimental data very well [14] for systems consisting of SO 2 (with inert gas)-water with CaSO 3 crystals. Considering experimental data [16] for the system consisting of CO 2 (with inert gas)-water with CaCO 3 particles, assumption 3 is also adequate.…”
Section: The Modelmentioning
confidence: 99%
“…However, the content of dissolved limestone in the solution has to be equal to zero (assumption 1) in view of its complete reaction with ªsulfurousº acid. The presence of dissolved CaSO 3 in the solution causes conversion of calcium sulfite to calcium hydrogen sulfite at the beginning of sulfur dioxide absorption [15,18]. Before the transformation of calcium sulfite to hydrogen sulfite is completed whole absorbed SO 2 are consumed in the conversion.…”
Section: The Modelmentioning
confidence: 99%
“…Additionally, CaHSO 3 + ions formation and/or the neutralization of SO 2 by sorbent result in a decrease of the concentration of HSO 3 - ions in the solution. In such a case, formation of pyrosulfite ions can be neglected. , …”
Section: The Modelmentioning
confidence: 99%
“…Points 2 and 3 allow one to assume that the amounts of dissolved SO 2 or CO 2 in the solution are sums of their content in pure water and the amount converted into MeHSO 3 + or MeHCO 3 + forms, respectively. Considering experimentally verified results of modeling of sulfur dioxide solubility in calcium sulfite water solutions and moderately concentrated solutions of magnesium sulfite, 9 the influence of calcium and magnesium salts content on Henry's constant can be neglected. A similar assumption can be introduced for Henry's constant describing carbon dioxide solubility.…”
Section: The Modelmentioning
confidence: 99%
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