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Related Concept Videos

Potentiometry: Overview01:06

Potentiometry: Overview

Potentiometry is an analytical technique that measures the potential difference between two electrodes in an electrochemical cell without drawing any significant current that could alter the solution's composition. This method employs an indicator electrode, which exchanges electrons with the analyte solution, and a reference electrode with a constant potential. Each electrode is immersed in a solution comprised of two half-cells. In a conventional setup, the reference electrode serves as the...
Potentiometric Titration: Overview01:31

Potentiometric Titration: Overview

Potentiometric titration is a quantitative analytical technique that determines the concentration of an analyte by measuring the potential difference between the two electrodes in the solution. The endpoint of a potentiometric titration is the point at which there is a significant change in the potential difference. It occurs when the stoichiometric reaction between the analyte and the titrant is complete. The endpoint is usually determined graphically by plotting the measured potential...
Controlled-Potential Coulometry: Electrolytic Methods01:17

Controlled-Potential Coulometry: Electrolytic Methods

Controlled-potential coulometry, also known as potentiostatic coulometry, employs a three-electrode system in which the working electrode's potential is precisely regulated using a potentiostat. Platinum working electrodes are utilized for positive potentials, while mercury pool electrodes are favored for extremely negative potentials. The platinum counter electrode is separated from the analyte using a membrane or salt bridge to avoid interference in the analysis.
The chosen potential ensures...
Potentiometry: Membrane Electrodes01:15

Potentiometry: Membrane Electrodes

Membrane electrodes, also known as p-ion electrodes, use membranes that selectively interact with free analyte ions, generating a potential difference across the membrane. The resulting membrane potential, known as the asymmetry potential, is not zero even when analyte concentrations on both sides of the membrane are equal. The membrane's response is typically not selective to a single analyte but proportional to the concentration of all ions in the sample solution capable of interacting at the...
Polyprotic Acids03:38

Polyprotic Acids

Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

Colligative Properties of ElectrolytesThe colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one dissolved...

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Related Experiment Video

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Dynamic Electrochemical Measurement of Chloride Ions
07:32

Dynamic Electrochemical Measurement of Chloride Ions

Published on: February 5, 2016

A computational method for approximate evaluation of ionization constants from potentiometric data.

A G Gonzalez1, D Rosales, J L Gomez Ariza

  • 1Department of Analytical Chemistry, Faculty of Chemistry, University of Sevilla, 41012-Sevilla, Spain.

Talanta
|April 1, 1988
PubMed
Summary

A new general equation and computer program accurately determine proton dissociation constants from potentiometric data for various acids. This method works for both simple and complex polybasic acids, even with overlapping steps.

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Area of Science:

  • Analytical Chemistry
  • Physical Chemistry

Background:

  • Accurate determination of proton dissociation constants is crucial for understanding acid-base equilibria.
  • Existing methods may have limitations with polybasic acids or overlapping dissociation steps.

Purpose of the Study:

  • To present a general equation for evaluating proton dissociation constants.
  • To develop a versatile method applicable to monobasic and polybasic acids, including those with overlapping dissociation steps.

Main Methods:

  • Utilized potentiometric data to derive a general equation.
  • Developed and employed a computer program for the calculations.
  • Applied the method to a range of acids from monobasic to octobasic.

Main Results:

  • The developed method successfully evaluated proton dissociation constants.
  • Satisfactory agreement was achieved between calculated and literature values for 22 tested acids.
  • The method demonstrated applicability to acids with successive, potentially overlapping, dissociation steps.

Conclusions:

  • The generalized equation and computational approach provide a reliable method for determining proton dissociation constants.
  • This approach offers a robust tool for analyzing acid-base properties across a spectrum of acidities.
  • The validated method enhances the accuracy of chemical equilibrium studies.