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Related Concept Videos

Potentiometric Titration: Overview01:31

Potentiometric Titration: Overview

4.2K
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...
4.2K
Acid-Base Titration Curves02:23

Acid-Base Titration Curves

140.6K
A titration curve is a plot of some solution property versus the amount of added titrant. For acid-base titrations, solution pH is a useful property to monitor because it varies predictably with the solution composition and, therefore, may be used to monitor the titration’s progress and detect its endpoint. Acid-base titration can be performed with a strong acid and a strong base, a strong acid and a weak base, or a strong base and a weak acid.
For a titration carried out for 25.00 mL of...
140.6K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

49.1K
Calculating pH for Titration Solutions: Weak Acid/Strong Base
For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as:
49.1K
Titration Calculations: Strong Acid - Strong Base02:28

Titration Calculations: Strong Acid - Strong Base

33.8K
Calculating pH for Titration Solutions: Strong Acid/Strong Base
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:
33.8K
Titration of a Polyprotic Acid02:08

Titration of a Polyprotic Acid

104.1K
A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process.  If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three...
104.1K
Acid–Base Titration: Overview01:26

Acid–Base Titration: Overview

17.9K
An acid-base titration is a technique used to determine the concentration of an unknown acid or base, using a titrant of known concentration–either a base for acid titration or an acid for base titration. The process involves gradually adding the titrant, leading to a predictable change in the pH of the solution. This change is plotted on a titration curve, showing how a solution's pH varies with the amount of titrant added. Such curves are instrumental in monitoring the...
17.9K

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Related Experiment Video

Updated: Jan 23, 2026

Determination of Carbonyl Functional Groups in Bio-oils by Potentiometric Titration: The Faix Method
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Determination of Carbonyl Functional Groups in Bio-oils by Potentiometric Titration: The Faix Method

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Activity-based analysis of potentiometric pH titrations.

Somaiyeh Khodadadi Karimvand1, Xuan Anh Nguyen2, Hamid Abdollahi3

  • 1Department of Chemistry, The University of Newcastle, University Drive, Newcastle, Australia; Department of Chemistry, Institute for Advanced Studies in Basic Sciences, Zanjan, Iran.

Analytica Chimica Acta
|June 15, 2019
PubMed
Summary

This study introduces a new computational method for chemical equilibrium analysis that bypasses the need for constant ionic strength. This approach provides more robust determination of thermodynamic equilibrium constants at low ionic strength.

Keywords:
Activity coefficientsLaw of mass actionPotentiometric titrationpH titration

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Area of Science:

  • Analytical Chemistry
  • Physical Chemistry
  • Computational Chemistry

Background:

  • Determining activity coefficients is challenging in quantitative equilibrium studies.
  • Traditionally, constant ionic strength is maintained using excess inert salts.
  • This method simplifies equilibrium constant calculations but can introduce inaccuracies.

Purpose of the Study:

  • To propose a novel computational approach for chemical equilibrium analysis.
  • To eliminate the requirement of maintaining constant ionic strength.
  • To enable more robust determination of thermodynamic equilibrium constants.

Main Methods:

  • Activity coefficients are approximated using Debye-Hückel equations during numerical analysis.
  • Titration data is analyzed computationally, adhering to mass conservation.
  • Mass action is applied approximately within the computational framework.

Main Results:

  • The addition of inert salts is no longer necessary.
  • Measurements can be performed at minimal ionic strength (I).
  • Thermodynamic equilibrium constants are determined more robustly at low I.

Conclusions:

  • The proposed method replaces the artificial maintenance of constant ionic strength.
  • Improved computational analysis offers a more accurate determination of equilibrium constants.
  • Validated with phosphoric and citric acids, demonstrating the technique's efficacy.