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Related Concept Videos

Theories of Dissolution: Diffusion Layer Model01:15

Theories of Dissolution: Diffusion Layer Model

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...
Theories of Dissolution: The Danckwerts' Model and Interfacial Barrier Model01:09

Theories of Dissolution: The Danckwerts' Model and Interfacial Barrier Model

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 concentration...
Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

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...
Common Ion Effect03:24

Common Ion Effect

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 Châtelier’s principle. Consider the dissolution of silver iodide:
Factors Affecting Solubility04:01

Factors Affecting Solubility

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:
Solubility03:00

Solubility

Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
In a solution, the solute particles (molecules, atoms, and/or ions)...

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Related Experiment Video

Updated: Jul 15, 2026

Synthesis of Zeolites Using the ADOR (Assembly-Disassembly-Organization-Reassembly) Route
08:26

Synthesis of Zeolites Using the ADOR (Assembly-Disassembly-Organization-Reassembly) Route

Published on: April 3, 2016

Understanding the dissolution of zeolites.

Ryan L Hartman1, H Scott Fogler

  • 1Department of Chemical Engineering, University of Michigan, 2300 Hayward Street, Ann Arbor, Michigan 48109-2136, USA.

Langmuir : the ACS Journal of Surfaces and Colloids
|April 14, 2007
PubMed
Summary

The silicon-to-aluminum ratio dictates zeolite dissolution in hydrochloric acid. This ratio controls aluminum removal, which in turn constrains silicon dissolution and influences silicate precipitation.

Area of Science:

  • Geochemistry
  • Materials Science
  • Chemical Engineering

Background:

  • Zeolites are microporous aluminosilicates with diverse natural and industrial applications.
  • Understanding zeolite dissolution in acidic environments is crucial for various processes.
  • Limited scientific knowledge exists regarding the dissolution mechanisms of zeolites in hydrochloric acid.

Purpose of the Study:

  • To investigate the influence of the silicon-to-aluminum (Si-to-Al) ratio on zeolite framework dissolution in aqueous hydrochloric acid solutions.
  • To elucidate the mechanism controlling selective aluminum removal and its effect on silicon dissolution.
  • To establish the general role of the Si-to-Al ratio in zeolite dissolution kinetics and outcomes.

Main Methods:

  • Experimental dissolution of Type 4A, analcime, and Type Y zeolites in hydrochloric acid.

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Organic Structure-directing Agent-free Synthesis for *BEA-type Zeolite Membrane
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Synthesis of Zeolites Using the ADOR (Assembly-Disassembly-Organization-Reassembly) Route
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  • Analysis of dissolution rates and products, including silicate precipitation.
  • Construction of zeolite framework models and comparison with experimental data (SEM, dissolution rates).

    • Main Results:

    • The Si-to-Al ratio universally controls zeolite dissolution, with selective aluminum removal preceding silicon dissolution.
    • Type 4A zeolite (Si-to-Al=1.0) showed stoichiometric dissolution, complete silicon dissolution, and subsequent silicate precipitation.
    • Analcime (Si-to-Al=2.0) dissolved non-stoichiometrically with partial silicon dissolution and precipitation.
    • Type Y zeolite (Si-to-Al=3.0) exhibited minimal silicon dissolution and amorphous silicate particle formation due to insufficient aluminum.

    Conclusions:

    • Zeolite dissolution is governed by the Si-to-Al framework ratio, impacting aluminum and silicon removal rates.
    • The dissolution mechanism is consistent across different zeolite framework types, emphasizing the Si-to-Al ratio's universal role.
    • Findings have significant implications for optimizing petroleum reservoir stimulation treatments.