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Related Concept Videos

Chemical Reactions in Aqueous Solutions03:03

Chemical Reactions in Aqueous Solutions

Chemical substances interact in many different ways. Certain chemical reactions exhibit common patterns of reactivity. Due to the vast number of chemical reactions, it becomes necessary to classify them based on the observed patterns of interaction.
SN2 Reaction: Kinetics02:14

SN2 Reaction: Kinetics

Kinetic Studies and Significance
In a chemical reaction, a relationship exists between the concentration of reactants and the rate at which the reaction proceeds. The study to measure this relationship is known as the kinetics of a chemical reaction. Kinetic studies are used to deduce the rate law of a chemical reaction, which provides information about the species involved during the transition state of the rate-determining step. Thus, kinetic studies help to derive the mechanism of a reaction.
Acid Halides to Amides: Aminolysis01:07

Acid Halides to Amides: Aminolysis

Aminolysis is a nucleophilic acyl substitution reaction, where ammonia or amines act as nucleophiles to give the substitution product. Acid halides react with ammonia, primary amines, and secondary amines to yield primary, secondary, and tertiary amides, respectively.
In the first step of the aminolysis mechanism, the amine attacks the carbonyl carbon of the acyl chloride to form a tetrahedral intermediate. In the second step, the carbonyl group is re-formed with the elimination of a chloride...
2° Amines to N-Nitrosamines: Reaction with NaNO201:20

2° Amines to N-Nitrosamines: Reaction with NaNO2

Secondary amines react with nitrous acid to form N-nitrosamines, as depicted in Figure 1. Nitrous acid, a weak and unstable acid, is formed in situ from an aqueous solution of sodium nitrite and strong acids, such as hydrochloric acid or sulfuric acid, in cold conditions. In the presence of an acid, the nitrous acid gets protonated. The subsequent loss of water results in the formation of the electrophile known as nitrosonium ion.
Diazonium Group Substitution with Halogens and Cyanide: Sandmeyer and Schiemann Reactions01:20

Diazonium Group Substitution with Halogens and Cyanide: Sandmeyer and Schiemann Reactions

Arenediazonium substitution reactions occur when the diazonium group is substituted by various functional groups such as halides, hydroxyl, nitrile, etc. For instance, arenediazonium salts react with copper(I) salts of chloride, bromide, or cyanide to form corresponding aryl chlorides, bromides, and nitriles. These reactions are named Sandmeyer reactions. Although the mechanism of this reaction is complicated, as illustrated in Figure 1, they are believed to progress via an aryl copper...
Precipitation Titration Curve: Analysis01:21

Precipitation Titration Curve: Analysis

The precipitation titration curve demonstrates the change in concentration of one reactant with the volume of titrant added. During the titration of chloride ions with silver nitrate, the precipitation titration curve is divided into three regions: before, at, and after the equivalence point. Before the equivalence point, low redissolution of the sparingly soluble silver chloride precipitate gives a low silver ion concentration. However, in the second region, representing the equivalence point,...

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Related Experiment Video

Updated: Jun 28, 2026

The Synthesis of [Sn10(Si(SiMe3)3)4]2- Using a Metastable Sn(I) Halide Solution Synthesized via a Co-condensation Technique
12:43

The Synthesis of [Sn10(Si(SiMe3)3)4]2- Using a Metastable Sn(I) Halide Solution Synthesized via a Co-condensation Technique

Published on: November 28, 2016

Iron(II)-chloramine-T reaction.

V R Rao1, G Aravamudan

  • 1Department of Chemistry, Indian Institute of Technology, Madras-36, India.

Talanta
|January 1, 1973
PubMed
Summary

Free radicals form during the iron(II)-chloramine-T reaction, consuming excess oxidant. This radical dimerization and oxidation explains chloramine-T destruction, highlighting potential issues with metal container storage.

Area of Science:

  • Analytical Chemistry
  • Reaction Kinetics

Background:

  • The iron(II)-chloramine-T reaction exhibits oxidant consumption exceeding stoichiometric requirements.
  • This phenomenon has been linked to the involvement of free radicals.

Purpose of the Study:

  • To experimentally demonstrate free radical formation in the iron(II)-chloramine-T reaction.
  • To elucidate the mechanism of excess chloramine-T consumption and its implications.

Main Methods:

  • Investigation of the iron(II)-chloramine-T reaction at acidic pH (2.56-5.6).
  • Experimental demonstration of free radical generation.
  • Analysis of reaction products, including dimerized species (R-NCl-NCl-R).
  • Study of iodine liberation from acidified potassium iodide by dimerized species.

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Last Updated: Jun 28, 2026

The Synthesis of [Sn10(Si(SiMe3)3)4]2- Using a Metastable Sn(I) Halide Solution Synthesized via a Co-condensation Technique
12:43

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Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy
07:49

Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy

Published on: February 20, 2020

Main Results:

  • Free radicals are experimentally confirmed during the reaction.
  • Dimerization of free radicals forms R-NCl-NCl-R species.
  • These dimers are further oxidized by chloramine-T.
  • The dimerized species slowly liberate iodine from acidified potassium iodide.
  • The proposed mechanism accounts for excess chloramine-T destruction with Fe(II) or bromide catalysts.

Conclusions:

  • Free radical mechanisms drive excess chloramine-T consumption in the presence of iron(II) and bromide.
  • Storage of chloramine-T in metal containers may lead to significant oxidant degradation via this mechanism and should be prevented.