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Related Concept Videos

1° Amines to Diazonium or Aryldiazonium Salts: Diazotization with NaNO2 Overview01:26

1° Amines to Diazonium or Aryldiazonium Salts: Diazotization with NaNO2 Overview

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Nitrous acid and nitric acids are two types of acids containing nitrogen, among which nitrous acid is weaker than nitric acid. Nitrous acid with a pKa value of 3.37 ionizes in water to give a nitrite ion and the hydronium ion.
The nitrous acid is unstable. Hence, it is formed in situ from a solution of sodium nitrite and cold aqueous acids such as hydrochloric or sulfuric acid. In an acidic solution, the –OH group of nitrous acid undergoes protonation to give oxonium ion, followed by...
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1° Amines to Diazonium or Aryldiazonium Salts: Diazotization with NaNO2 Mechanism01:37

1° Amines to Diazonium or Aryldiazonium Salts: Diazotization with NaNO2 Mechanism

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Nitrous acid is a relatively weak and unstable acid prepared in situ by the reaction of sodium nitrite and cold, dilute hydrochloric acid. In an acidic solution, the nitrous acid undergoes protonation when it loses water to form a nitrosonium ion—an electrophile. Nitrous acid reacts with primary amines to give diazonium salts. The reaction is called diazotization of primary amines.
5.1K
2° Amines to N-Nitrosamines: Reaction with NaNO201:20

2° Amines to N-Nitrosamines: Reaction with NaNO2

5.6K
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.
5.6K
Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

69.3K
Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
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Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

3.0K
The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
3.0K
Preparation of Nitriles01:12

Preparation of Nitriles

2.8K
One of the common methods to prepare nitriles is the dehydration of amides. This method requires strong dehydrating agents like phosphorous pentoxide or boiling acetic anhydride for converting amides to nitriles. Another reagent namely, thionyl chloride also accomplishes the dehydration of amides, where amide acts as a nucleophile. The first step of the mechanism involves the nucleophilic attack by the amide on the thionyl chloride to form an intermediate. In the next step, the electron pairs...
2.8K

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Solution structures in alkali nitrates and nitrites at high concentrations.

Sebastian T Mergelsberg1, Trent R Graham1, Emily T Nienhuis1

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Cation identity governs solution structure in concentrated electrolytes. Smaller cations form ion pairs, while larger ones create extended networks, impacting bulk properties and phase behavior.

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Area of Science:

  • Physical Chemistry
  • Materials Science
  • Solution Chemistry

Background:

  • Classical models struggle with highly concentrated electrolyte solutions.
  • Ion-solvent interactions are critical for determining bulk properties in these systems.

Purpose of the Study:

  • To link molecular coordination to mesoscale structure in concentrated alkali nitrate and nitrite solutions.
  • To elucidate the role of cation identity in dictating solution architecture.

Main Methods:

  • Small-angle X-ray scattering (SAXS) to probe mesoscale structure.
  • Raman spectroscopy to analyze molecular coordination.
  • Investigation across various alkali metal cations (Li+, Na+, K+, Rb+, Cs+) and anions (nitrate, nitrite).

Main Results:

  • Smaller cations (Li+, Na+) form discrete contact ion pairs.
  • Larger cations (K+, Rb+) lead to disordered local coordination and extended solute-solvent networks.
  • Cesium cations (Cs+) exhibit a concentration-induced transition to a highly ordered state.

Conclusions:

  • Cation identity establishes a structural hierarchy in concentrated electrolyte solutions.
  • The findings offer a mechanistic explanation for solution behavior and a predictive basis for industrial and environmental applications.