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Related Concept Videos

EDTA: Chemistry and Properties01:22

EDTA: Chemistry and Properties

Polydentate ligands are most widely used in complexometric titrations because they form more stable complexes with the metal ions than mono- or bidentate ligands due to the chelate effect. Examples of polydentate ligands are ethylenediaminetetraacetic acid (EDTA), crown ethers, and cryptands. The most important feature of optimal polydentate ligands is the ability to form 1:1 complexes in a single-step process. Amino carboxylic acid derivatives are frequently used as complexing agents. EDTA is...
Masking and Demasking Agents01:19

Masking and Demasking Agents

EDTA titrations may necessitate masking and demasking agents to temporarily protect a particular metal ion in a mixture from the EDTA reaction. These agents facilitate the sequential analysis of the metal ions by forming stable complexes with some—but not all—metal ions during certain steps.
There are many masking agents, such as cyanide, fluoride, triethanolamine, thiourea, and 2,3-bis(sulfanyl)propan-1-ol (formerly 2,3-dimercapto-1-propanol), with the masking agent chosen based on the metal...
EDTA: Auxiliary Complexing Reagents01:26

EDTA: Auxiliary Complexing Reagents

EDTA titrations are usually carried out in highly basic conditions, where the fully deprotonated form of EDTA, Y4−, actively complexes with the free metal ions in the solution. Several metal ions precipitate as hydrous oxide (hydroxides, oxides, or oxyhydroxides) under these conditions, lowering the concentration of free metal ions in the solution. For this reason, auxiliary complexing agents or ligands such as ammonia, tartrate, citrate, or triethanolamine are used in EDTA titrations to...
Effects of EDTA on End-Point Detection Methods01:18

Effects of EDTA on End-Point Detection Methods

Different methods, such as visual observance of metal-ion indicators, spectroscopic techniques, and potentiometric methods, can determine the endpoint of an EDTA titration.
In the visual method, metal-ion indicators (metallochromic dyes), which have distinct colors in their free and complex forms, are added to the mixture to signal the titration's end point. They form stable complexes with metal ions, but these complexes are weaker than the corresponding metal–EDTA complexes. As a result, EDTA...
EDTA: Conditional Formation Constant01:09

EDTA: Conditional Formation Constant

Each EDTA molecule has six binding sites: four carboxyl groups and two amino groups. The fully protonated form of EDTA is represented as H6Y2+. However, it can exist in different forms, H5Y+, H4Y, H3Y−, H2Y2−, and HY3−, depending on the pH of the solution. In very basic solutions with pH > 10.17, the fully deprotonated form, Y4−, is the predominant species that readily complexes with metal ions in a 1:1 ratio.
For the equilibrium reaction of the metal with the Y4− form of EDTA, the formation...
EDTA: Direct, Back-, and Displacement Titration01:30

EDTA: Direct, Back-, and Displacement Titration

The EDTA titration types for metal ion analysis include direct titration, back-titration, and replacement titration.
Direct titration involves buffering the metal ion solution to the desired pH and directly titrating with standard EDTA until the endpoint. The optimum pH ensures a large conditional formation constant of metal−EDTA and visibility of the free indicator color in the solution. In addition, auxiliary complexing reagents are used to prevent the precipitation of metal hydroxides and...

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Related Experiment Video

Updated: Jun 27, 2026

A Mice Model of Chlorhexidine Gluconate-Induced Peritoneal Damage
04:25

A Mice Model of Chlorhexidine Gluconate-Induced Peritoneal Damage

Published on: April 28, 2022

Interaction between chlorhexidine digluconate and EDTA.

Brian J Rasimick1, Michelle Nekich, Megan M Hladek

  • 1Essential Dental Laboratories, South Hackensack, NJ 07606, USA. brasimick@edsdental.com

Journal of Endodontics
|November 26, 2008
PubMed
Summary

Chlorhexidine and EDTA form a precipitate, but do not chemically degrade. Analysis confirmed the precipitate is primarily a salt formed between chlorhexidine and EDTA, with no harmful byproducts detected.

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Hydrolysis of a Ni-Schiff-Base Complex Using Conditions Suitable for Retention of Acid-labile Protecting Groups
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Hydrolysis of a Ni-Schiff-Base Complex Using Conditions Suitable for Retention of Acid-labile Protecting Groups

Published on: April 6, 2017

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Last Updated: Jun 27, 2026

A Mice Model of Chlorhexidine Gluconate-Induced Peritoneal Damage
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Hydrolysis of a Ni-Schiff-Base Complex Using Conditions Suitable for Retention of Acid-labile Protecting Groups
06:44

Hydrolysis of a Ni-Schiff-Base Complex Using Conditions Suitable for Retention of Acid-labile Protecting Groups

Published on: April 6, 2017

Area of Science:

  • Analytical Chemistry
  • Materials Science

Background:

  • Chlorhexidine and EDTA are commonly used in various applications.
  • Their combination can result in a white precipitate, raising questions about chemical interactions.

Purpose of the Study:

  • To investigate the nature of the precipitate formed by combining chlorhexidine and EDTA.
  • To determine if chlorhexidine undergoes chemical degradation in the presence of EDTA.

Main Methods:

  • Precipitate formation and redissolution in trifluoroacetic acid.
  • Quantitative analysis of chlorhexidine and EDTA using reverse-phase high performance liquid chromatography (HPLC).
  • Detection of potential chlorhexidine decomposition products.

Main Results:

  • The precipitate consists of over 90% chlorhexidine and EDTA.
  • No detectable levels of parachloroaniline, a chlorhexidine decomposition product, were found.
  • The molar ratio of chlorhexidine to EDTA in the precipitate was approximately 1.6:1.

Conclusions:

  • The white precipitate is a salt formed between chlorhexidine and EDTA.
  • Chlorhexidine does not chemically degrade when combined with EDTA under these conditions.