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Related Concept Videos

Factors Affecting Solubility04:01

Factors Affecting Solubility

34.3K
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:
34.3K
Solubility Equilibria03:07

Solubility Equilibria

54.0K
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation.
The...
54.0K
Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

969
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...
969
Precipitation of Ions03:11

Precipitation of Ions

28.6K
Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
28.6K
Common Ion Effect03:24

Common Ion Effect

42.9K
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:
42.9K
Calculating Equilibrium Concentrations02:05

Calculating Equilibrium Concentrations

49.5K
Being able to calculate equilibrium concentrations is essential to many areas of science and technology—for example, in the formulation and dosing of pharmaceutical products. After a drug is ingested or injected, it is typically involved in several chemical equilibria that affect its ultimate concentration in the body system of interest. Knowledge of the quantitative aspects of these equilibria is required to compute a dosage amount that will solicit the desired therapeutic effect.
A more...
49.5K

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Related Experiment Video

Updated: Oct 9, 2025

Combining Solid-state and Solution-based Techniques: Synthesis and Reactivity of ChalcogenidoplumbatesII or IV
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Combining Solid-state and Solution-based Techniques: Synthesis and Reactivity of ChalcogenidoplumbatesII or IV

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Theoretical equilibrium lead(II) solubility revisited: Open source code and practical relationships.

David G Wahman1, Matthew D Pinelli2, Michael R Schock1

  • 1United States Environmental Protection Agency, Office of Research & Development, Cincinnati, Ohio, USA.

AWWA Water Science
|December 23, 2021
PubMed
Summary
This summary is machine-generated.

A new R code model simulates lead(II) solubility, offering accessible tools for researchers to explore lead(II) concentrations in various water conditions and aiding future model development.

Keywords:
DICLEADSOLTELSSchlorideleadphosphatesolubility modelsulfate

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Area of Science:

  • Environmental Chemistry
  • Computational Chemistry
  • Water Quality Modeling

Background:

  • Lead(II) (Pb(II)) solubility is critical for understanding lead contamination in aquatic environments.
  • Existing models like LEADSOL provide theoretical frameworks but may lack accessibility and flexibility.
  • Accurate modeling of soluble Pb(II) is essential for environmental risk assessment and remediation strategies.

Purpose of the Study:

  • To update and implement a theoretical equilibrium lead(II) solubility model in open-source R code.
  • To provide a user-friendly and reproducible tool for simulating total soluble Pb(II) (TOTSOLPb) concentrations.
  • To explore the influence of various environmental factors on Pb(II) solubility.

Main Methods:

  • The Fortran-based LEADSOL model was translated and implemented into R code (app.R).
  • The R code was verified against the original LEADSOL model output for accuracy.
  • Simulations were conducted using the R code to generate solubility diagrams under diverse conditions.

Main Results:

  • The R code (app.R) is publicly available on GitHub, enabling local execution and user customization.
  • Solubility diagrams were generated, illustrating the impact of pH, dissolved inorganic carbon, orthophosphate, sulfate, and chloride on TOTSOLPb.
  • The model provides a reproducible baseline for further development and improvement of lead solubility models.

Conclusions:

  • The developed R code offers an accessible and flexible tool for investigating lead(II) solubility.
  • The model facilitates the exploration of key water quality parameters affecting soluble lead concentrations.
  • This open-source approach promotes reproducibility and collaborative advancement in environmental modeling.