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Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

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When a substance such as sodium chloride is added to water, it dissolves, forming an aqueous solution. The extent of dissolution is called solubility. The process of dissolution can exist in equilibrium, just like other chemical processes. Solubility equilibria are also called precipitation equilibria because the process of solubility can be reversible. The reverse of the solubility process is called precipitation.
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Distillation is a separation technique that takes advantage of the boiling point properties of disparate elements in a mixture. To perform distillation, we begin by heating a miscible mixture of two liquids with a significant difference in boiling points (at least 20°C). As the solution heats up and reaches the bubble point of the more volatile component, some molecules of the more volatile component transition into the gas phase and travel upward into the condenser, which is a glass tube...
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Various dissolution theories provide insight into the factors that influence the dissolution rate. Danckwerts' Model suggests that turbulence, rather than a stagnant layer, characterizes the dissolution medium at the solid-liquid interface. In this model, the agitated solvent contains macroscopic packets that move to the interface via eddy currents, facilitating the absorption and delivery of the drug to the bulk solution. The regular replenishment of solvent packets maintains the...
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The free energy change associated with dissolving a solute in a liter of solvent is called the free energy of a solution, ΔGsolution. The overall ΔGsolution is expressed as the balance of ΔGinteraction against the always-favorable free-energy of mixing, ΔGmixing. Solution formation is favorable if  ΔGsolution is less than zero, whereas it is unfavorable if ΔGsolution is greater than zero. In short, for a solution to form and complete dissolution to take place,...
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Activity modelling of the solid-liquid equilibrium of deep eutectic solvents.

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Deep eutectic solvents (DESs) offer a sustainable alternative to traditional solvents. This study details their phase diagrams and shows how a modified thermodynamic model accurately describes their non-ideal liquid behavior.

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Area of Science:

  • Green Chemistry
  • Materials Science
  • Thermodynamics

Background:

  • Deep eutectic solvents (DESs) are emerging as sustainable alternatives in the chemical industry.
  • DESs are binary mixtures exhibiting significant melting point depression due to strong intermolecular interactions.
  • Understanding their phase behavior is crucial for their application and design.

Purpose of the Study:

  • To experimentally determine phase diagrams for novel DESs with varying non-ideality.
  • To evaluate the accuracy of thermodynamic models in describing DES solid-liquid equilibria.
  • To correlate model parameters with the non-ideal behavior of DES mixtures.

Main Methods:

  • Experimental measurement of solid-liquid phase diagrams for multiple DESs.
  • Application and assessment of thermodynamic models, including the orthogonal polynomial (OP) expansion.
  • Analysis of activity coefficients to understand asymmetric behavior.

Main Results:

  • Presented experimental phase diagrams for various DESs, showcasing a range of non-ideality.
  • Demonstrated that the orthogonal Redlich-Kister-like polynomial (OP) expansion accurately describes the solid-liquid equilibria.
  • Established a link between model parameters and the observed non-ideal and asymmetric behaviors.

Conclusions:

  • The modified OP expansion provides an accurate thermodynamic description of DES phase behavior.
  • This model, an extension of regular solution theory, allows for physical interpretation of parameters.
  • Findings facilitate the design and application of DESs by predicting their liquid range and behavior.