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Related Concept Videos

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:
Formation of Complex Ions03:45

Formation of Complex Ions

A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
Chemical Equilibria: Redefining Equilibrium Constant01:20

Chemical Equilibria: Redefining Equilibrium Constant

The effect of an inert salt on the solubility of a sparingly soluble salt is known as the salt effect. The degree of the salt effect varies with the ionic strength of the solution, which in turn depends on the activity of the species in the solution. The activity is expressed as the product of concentration and the activity coefficient of the species.
To calculate the equilibrium constants of solutions of moderately high ionic strength, one must account for the salt effect. This redefined...
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary cation—the calcium...
Ion Exchange01:17

Ion Exchange

Ion exchange chromatography separates charged molecules from a solution by reversibly exchanging them with mobile, or 'active', ions associated with the oppositely charged stationary phase. This method can be used to separate ions, soften and deionize water, and purify solutions. The polymers comprising the ion-exchange column are high-molecular-weight and chemically stable polymers, crosslinked to be porous and essentially insoluble. They are also functionalized with either acidic or basic...

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Related Experiment Video

Updated: Jun 28, 2026

Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
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Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry

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Ionic medium effects on equilibrium constants Part II. Binary systems comprising some bivalent cations and

L Pezza1, M Molina, C B Melios

  • 1Instituto de Química, UNESP, Araraquara, SP, Brazil.

Talanta
|October 1, 1996
PubMed
Summary

Simple equations were developed to predict protonation and formation constants for monocarboxylates and bivalent cations across various ionic strengths. This allows for parameter interconversion and estimation of thermodynamic constants and activity coefficients.

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Area of Science:

  • Analytical Chemistry
  • Solution Chemistry

Background:

  • Accurate determination of protonation and formation constants is crucial for understanding chemical equilibria.
  • Ionic strength significantly influences these constants in aqueous solutions.

Purpose of the Study:

  • To derive simple equations relating protonation and formation constants of monocarboxylates and bivalent cations.
  • To enable interconversion of parameters between different ionic strengths (up to 3.00 M).
  • To estimate thermodynamic formation constants and activity coefficients.

Main Methods:

  • Development of simple equations based on experimental data.
  • Calculations performed in aqueous sodium perchlorate media at 25°C.
  • Systematic variation of ionic strength.

Main Results:

  • Equations successfully relate stoichiometric protonation and formation constants.
  • The method allows for accurate parameter interconversion across ionic strengths.
  • Estimated thermodynamic formation constants and activity coefficients show consistency.

Conclusions:

  • The derived equations provide a consistent and reliable method for predicting chemical equilibria.
  • This approach simplifies the analysis of complexation reactions in solutions of varying ionic strength.
  • The findings are valuable for researchers in analytical and solution chemistry.