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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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Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

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Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
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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.
3.9K
Common Ion Effect03:24

Common Ion Effect

41.9K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility02:34

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
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The Equilibrium Constant03:11

The Equilibrium Constant

48.0K
Consider the oxidation of sulfur dioxide:
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Supercritical Nitrogen Processing for the Purification of Reactive Porous Materials
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Does HNO3 dissociate on gas-phase ice nanoparticles?

Anastasiya Khramchenkova1, Andriy Pysanenko2, Jozef Ďurana2

  • 1Lehrstuhl für Physikalische Chemie, TUM School of Natural Sciences, Technische Universität München, Lichtenbergstraße 4, 85748 Garching, Germany. jozef.lengyel@tum.de.

Physical Chemistry Chemical Physics : PCCP
|July 17, 2023
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Summary
This summary is machine-generated.

Nitric acid dissociation is suppressed on small ice nanoparticles compared to larger surfaces. Proton transfer is significantly reduced, impacting atmospheric ice particle chemistry.

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Area of Science:

  • Physical Chemistry
  • Atmospheric Science
  • Surface Science

Background:

  • Nitric acid (HNO3) plays a crucial role in atmospheric chemistry.
  • Heterogeneous reactions on ice surfaces influence atmospheric composition.
  • Understanding HNO3 interactions with water ice is vital for climate modeling.

Purpose of the Study:

  • To investigate the dissociation of nitric acid on water ice nanoparticles.
  • To compare HNO3 dissociation on nanoparticles versus macroscopic ice surfaces.
  • To determine the influence of particle size on proton transfer.

Main Methods:

  • Utilizing a molecular beam to study (H2O)N clusters (N ≈ 30-500).
  • Doping water clusters with single HNO3 molecules.
  • Probing cluster ions via mass spectrometry after low-energy electron attachment (1.5-15 eV).

Main Results:

  • Direct evidence for HNO3 dissociation forming NO3-⋯H3O+ ion pairs was observed.
  • Over half of the observed cluster ions originated from non-dissociated HNO3.
  • Proton transfer was significantly suppressed on nanometer-sized particles compared to macroscopic ice.

Conclusions:

  • Nitric acid dissociation is significantly less efficient on ice nanoparticles than on bulk ice.
  • The suppressed proton transfer on small ice particles has implications for atmospheric heterogeneous processes.
  • Particle size is a critical factor in governing the reactivity of nitric acid on atmospheric ice.