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An arbitrary correction function for CO(2) evolution in acid-base titrations and its use in multiparametric
1Ecole Nationale Supérieure de Chimie de Lille, Université de Lille I, BP 40, 59650 Villeneuve d'Ascq, France.
Talanta
|August 1, 1981
Summary
This study introduces a new method to accurately perform acid-base titrations by accounting for carbon dioxide evolution. This improves mass-balance calculations and provides a parameter for CO(2) departure.
Area of Science:
- Analytical Chemistry
- Physical Chemistry
Background:
- Acid-base titrations are crucial in chemical analysis.
- Inert gas flow can lead to carbon dioxide loss, complicating mass-balance calculations.
- Accurate determination of concentrations and acidity constants is vital.
Purpose of the Study:
- To develop a method for precise acid-base titrations involving carbon dioxide evolution.
- To introduce a function for CO(2) evolution into titration calculations.
- To improve the accuracy of multiparametric refinement in titrations.
Main Methods:
- Proposed a function to model carbon dioxide evolution during titration.
- Integrated this function into the general titrant volume expression.
- Introduced a modified weighting factor to address equilibrium departures.
- Applied multiparametric refinement for data analysis.
Main Results:
- The method accurately determines concentrations and acidity constants even with CO(2) loss.
- A new parameter characterizing CO(2) departure was successfully obtained.
- The approach was validated using three distinct titration scenarios.
Conclusions:
- The developed functions enable accurate acid-base titrations under conditions of CO(2) evolution.
- The method enhances the reliability of chemical analysis involving carbonated species.
- This approach is applicable to complex mixtures and various neutralization reactions.
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02:23Acid-Base Titration Curves
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For a titration carried out for 25.00 mL of 0.100...
For a titration carried out for 25.00 mL of 0.100...
01:26Acid–Base Titration: Overview
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 titration's progress...
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The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...
01:30Titration of a Weak Acid with a Strong Base
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01:17Solution Composition During Acid/Base Titrations
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The α0 and α1 values represent the...
The α0 and α1 values represent the...
01:29Conductometric Titrations: Strong Acid-Base and Weak Acid-Base Titrations
In acid-base titrations, conductance measurements are utilized to detect the endpoint. This method is grounded on the fact that electrical conductance relies on the number and mobility of ions. For instance, consider titrating strong acid HCl with a strong NaOH base. Initially, the HCl in the conductivity vessel conducts electricity due to the presence of hydrogen ions and chloride ions. As NaOH is gradually added from the burette, the fast-moving hydrogen ions are replaced by slower-moving...