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Calculating the Equilibrium Constant02:46

Calculating the Equilibrium Constant

The equilibrium constant for a reaction is calculated from the equilibrium concentrations (or pressures) of its reactants and products. If these concentrations are known, the calculation simply involves their substitution into the Kc expression.
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
The Equilibrium Binding Constant and Binding Strength02:18

The Equilibrium Binding Constant and Binding Strength

The equilibrium binding constant (Kb) quantifies the strength of a protein-ligand interaction. Kb can be calculated as follows when the reaction is at equilibrium:
Calculating Equilibrium Concentrations02:05

Calculating Equilibrium Concentrations

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...
Complexation Equilibria: Overview01:23

Complexation Equilibria: Overview

Complexation reactions take place when dative or coordinate covalent bonds form between metal ions and ligands. The compounds formed in these reactions are called coordination compounds. The number of bonds formed between the metal ion and the ligands is called its coordination number. Generally, most metal ions in an aqueous solution are solvated by water molecules and thus exist as aqua complexes.
The equilibrium constant of the complexation reaction is represented as the formation constant...
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...

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Related Experiment Video

Updated: Jun 28, 2026

Determination of the Photoisomerization Quantum Yield of a Hydrazone Photoswitch
09:33

Determination of the Photoisomerization Quantum Yield of a Hydrazone Photoswitch

Published on: February 7, 2022

Calculation of stability constants from photometric data.

F Ingman1

  • 1Department of Inorganic and Analytical Chemistry, Abo Akademi, Abo, Finland.

Talanta
|October 1, 1973
PubMed
Summary

This study adapts a wedge calorimeter method for determining stability constants using simple photometric techniques. The new approach is ideal when individual species absorptivities are unknown, simplifying chemical analysis.

Area of Science:

  • Analytical Chemistry
  • Physical Chemistry

Background:

  • Determining stability constants is crucial for understanding chemical interactions.
  • Traditional methods often require knowing the absorptivities of individual species, which can be challenging.
  • Wedge calorimetry offers a potential alternative but requires adaptation for broader use.

Purpose of the Study:

  • To adapt a wedge calorimeter-based method for determining stability constants.
  • To enable stability constant determination using standard photometric techniques.
  • To provide a method applicable even when individual species absorptivities are unknown.

Main Methods:

  • Adaptation of a wedge calorimeter method for photometric measurements.
  • Development of simplified calculation procedures.

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Related Experiment Videos

Last Updated: Jun 28, 2026

Determination of the Photoisomerization Quantum Yield of a Hydrazone Photoswitch
09:33

Determination of the Photoisomerization Quantum Yield of a Hydrazone Photoswitch

Published on: February 7, 2022

Analysis of Protein Complex Formation at Micromolar Concentrations by Coupling Microfluidics with Mass Photometry
06:39

Analysis of Protein Complex Formation at Micromolar Concentrations by Coupling Microfluidics with Mass Photometry

Published on: January 26, 2024

A Fluorescence Fluctuation Spectroscopy Assay of Protein-Protein Interactions at Cell-Cell Contacts
08:43

A Fluorescence Fluctuation Spectroscopy Assay of Protein-Protein Interactions at Cell-Cell Contacts

Published on: December 1, 2018

  • Application to systems where individual absorbing species cannot be isolated.

    • Main Results:

    • Successful adaptation of the wedge calorimeter method to photometric techniques.
    • Demonstration of simple calculations for stability constant determination.
    • Validation of the method's utility in cases of unavailable absorptivities.

    Conclusions:

    • The adapted photometric method provides a straightforward approach to determining stability constants.
    • This technique is particularly valuable for complex solutions where individual component analysis is difficult.
    • The method offers a practical alternative for stability constant studies in analytical and physical chemistry.