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Related Concept Videos

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.
Solubility is important in biological and environmental processes. A notable...
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Theories of Dissolution: The Danckwerts' Model and Interfacial Barrier Model01:09

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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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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
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Intermolecular Forces in Solutions

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The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
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Theories of Dissolution: Diffusion Layer Model01:15

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Dissolution, the process by which drug particles dissolve in a solvent, is explained by the diffusion layer model, a theoretical framework that simulates the absorption of oral drugs and allows us to analyze experimental data.
This process starts with a thin layer, saturated with the drug, forming at the interface between the solid and liquid. The solute then diffuses from this layer into the main solution. The Noyes-Whitney equation suggests that the rate of dissolution relies on the diffusion...
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Effect of variable solubility on reactive dissolution in partially miscible systems.

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Chemical reactions can enhance solute transfer between phases. A reaction consuming reactant A and producing C, which reduces A’s solubility, can optimize dissolution, aiding applications like CO2 sequestration.

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Area of Science:

  • Physical Chemistry
  • Chemical Engineering
  • Environmental Science

Background:

  • Solubility of a reactant (A) in a host phase can be affected by chemical reactions.
  • Product species (C) can alter the solubility of reactant A, influencing mass transfer.

Purpose of the Study:

  • To theoretically investigate optimal conditions for reactive transfer of solute A into a host phase.
  • To analyze the impact of a bimolecular reaction (A + B → C) where product C decreases A's solubility.

Main Methods:

  • Theoretical modeling of reaction-diffusion (RD) processes.
  • Numerical quantification of concentration profiles and reaction front evolution.
  • Analytical computation of asymptotic concentration profiles.

Main Results:

  • Increased reactant B concentration or diffusion rates of B and C enhance A's flux.
  • A stronger negative effect of C on A's solubility decreases mass transfer.
  • Optimized conditions for reactive transfer were identified.

Conclusions:

  • Chemical reactions can significantly influence and potentially optimize solute transfer.
  • Understanding these dynamics is crucial for applications like geological CO2 sequestration.