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Related Concept Videos

Calculating the Equilibrium Constant02:46

Calculating the Equilibrium Constant

37.6K
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:
37.6K
The Equilibrium Binding Constant and Binding Strength02:18

The Equilibrium Binding Constant and Binding Strength

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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:
14.9K
The Equilibrium Binding Constant and Binding Strength02:18

The Equilibrium Binding Constant and Binding Strength

10.0K
10.0K
The Equilibrium Constant03:10

The Equilibrium Constant

56.1K
Consider the oxidation of sulfur dioxide:
56.1K
Chemical Equilibria: Redefining Equilibrium Constant01:20

Chemical Equilibria: Redefining Equilibrium Constant

1.1K
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...
1.1K
Free Energy and Equilibrium02:56

Free Energy and Equilibrium

27.0K
The free energy change for a process may be viewed as a measure of its driving force. A negative value for ΔG represents a driving force for the process in the forward direction, while a positive value represents a driving force for the process in the reverse direction. When ΔGrxn is zero, the forward and reverse driving forces are equal, and the process occurs in both directions at the same rate (the system is at equilibrium).
Recall that Q is the numerical value of the mass action...
27.0K

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Sedimentation Equilibrium of a Small Oligomer-forming Membrane Protein: Effect of Histidine Protonation on Pentameric Stability
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Where to find equilibrium constants?

Wolfgang Hummel1, Montserrat Filella2, Darren Rowland3

  • 1Laboratory for Waste Management, Paul Scherrer Institute, Forschungsstrasse 111, CH-5232 Villigen PSI, Switzerland.

The Science of the Total Environment
|July 24, 2019
PubMed
Summary
This summary is machine-generated.

Finding reliable equilibrium constants for metal-ligand interactions is vital for accurate modelling. This study reviews eleven major compilations, detailing their scope, methods, and accessibility for solution chemistry researchers.

Keywords:
Chemical equilibriaConstant compilationsEquilibrium constantsSpeciation calculationsSpeciation modelling

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Area of Science:

  • Solution Chemistry
  • Chemical Thermodynamics
  • Computational Chemistry

Background:

  • Accurate equilibrium constants are essential for chemical equilibrium modeling.
  • Selecting appropriate constants is challenging for new researchers due to numerous, varied compilations.
  • Existing compilations have limitations in coverage, availability, and critical assessment methods.

Purpose of the Study:

  • To survey and critically evaluate eleven major compilations of equilibrium constants.
  • To provide researchers with information on the scope, background, and accessibility of these databases.
  • To discuss the methodologies used by data compilers in assessing equilibrium constant values.

Main Methods:

  • Systematic review of eleven prominent equilibrium constant compilations.
  • Analysis of each compilation's historical context and project scope.
  • Assessment of database coverage (metals, ligands) and current availability (publications, digital formats).
  • Examination of the critical assessment and data evaluation techniques employed by compilers.

Main Results:

  • Detailed profiles of eleven key equilibrium constant databases are presented.
  • Information on the historical development, scope (metal/ligand range), and accessibility of each compilation is provided.
  • Comparative analysis of the data assessment methodologies used across different compilations.

Conclusions:

  • This review aids researchers in selecting appropriate equilibrium constant compilations for their specific needs.
  • Understanding the strengths and limitations of various databases improves the reliability of equilibrium modeling.
  • The survey highlights the importance of critical data assessment and accessibility in chemical thermodynamics databases.