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Related Concept Videos

Complexometric Titration: Overview00:39

Complexometric Titration: Overview

Complexometric titration involves the formation of a complex by reacting a metal ion with one or more ligands. A visual indicator often detects the end point of a complexometric titration. It is added to the metal solution before the titration, forming a stable metal–indicator complex and imparting color to the solution. As the titration approaches the equivalence point, the excess of the added ligand displaces the indicator from the metal–indicator complex, releasing the free indicator. The...
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...
Indicators02:39

Indicators

Certain organic substances change color in dilute solution when the hydronium ion concentration reaches a particular value. For example, phenolphthalein is a colorless substance in any aqueous solution with a hydronium ion concentration greater than 5.0 × 10−9 M (pH < 8.3). In more basic solutions where the hydronium ion concentration is less than 5.0 × 10−9 M (pH > 8.3), it is red or pink. Substances such as phenolphthalein, which can be used to determine the pH of a solution, are called...
Complexometric Titration: Ligands00:43

Complexometric Titration: Ligands

Different monodentate and polydentate ligands are used as complexing agents in complexometric titration reactions. The formation of complexes by mono- and bidentate ligands involves two or more intermediate steps, limiting their use as complexing agents. In comparison, polydentate ligands can form complexes with metal ions in a single-step process, facilitating sharper end points. This means polydentate ligands, such as amino carboxylic acid derivatives, are most commonly employed in...
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...
Qualitative Analysis03:46

Qualitative Analysis

For solutions containing mixtures of different cations, the identity of each cation can be determined by qualitative analysis. This technique involves a series of selective precipitations with different chemical reagents, each reaction producing a characteristic precipitate for a specific group of cations. Metal ions within a group are further separated by varying the pH, heating the mixture to redissolve a precipitate, or adding other reagents to form complex ions.
For instance, group IV...

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Related Experiment Video

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Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks
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Two possible colorimetric indicators for use in studying magnesium complexation kinetics.

R S Taylor1

  • 1Department of Inorganic and Structural Chemistry University of Leeds Leeds LS29JT England.

Talanta
|November 1, 1974
PubMed
Summary

This study presents complexation rate data for magnesium with two indicators, 3,5-dinitrosalicylic acid and kojic acid. Findings suggest an S(N)1 mechanism for forward rate constants and provide equilibrium constants for magnesium complex formation.

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Area of Science:

  • Analytical Chemistry
  • Inorganic Chemistry
  • Chemical Kinetics

Background:

  • Colorimetric indicators are crucial for determining metal ion concentrations.
  • Understanding the kinetics and equilibrium of metal-indicator complexation is essential for accurate analysis.

Purpose of the Study:

  • To present complexation-rate equilibrium data for magnesium.
  • To investigate the reaction mechanism of magnesium complex formation with 3,5-dinitrosalicylic acid and kojic acid.

Main Methods:

  • Equilibrium data collection at 25.0 °C in a 0.5M KCl medium.
  • Determination of forward rate constants and complex formation constants.

Main Results:

  • Forward rate constants for both indicators are consistent with an S(N)1 mechanism.
  • Complex formation constants were determined to be 145 L/mol for 3,5-dinitrosalicylic acid and 390 L/mol for kojic acid.

Conclusions:

  • The S(N)1 mechanism is proposed for the forward complexation reaction.
  • The determined constants provide valuable data for the quantitative analysis of magnesium using these indicators.