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Related Concept Videos

Polyprotic Acids03:38

Polyprotic Acids

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Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
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Intermolecular Forces03:13

Intermolecular Forces

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Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
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Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

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The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
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Acidity of Carboxylic Acids01:21

Acidity of Carboxylic Acids

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Carboxylic acids are the strongest organic acids. However, their acidic strength is much less than mineral acids like HCl. Carboxylic acids ionize in water and readily lose the hydroxyl proton to form a resonance-stabilized carboxylate ion.
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Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

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Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le...
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Common Ion Effect03:24

Common Ion Effect

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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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Carboxylate Ion Availability at the Air-Water Interface.

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|October 28, 2016
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Amphiphilic carboxylate ions at the air-water interface increase with chain length and surface area. Aromatic carboxylates are least available due to water interactions, impacting atmospheric aerosol processes.

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Area of Science:

  • Environmental Chemistry
  • Atmospheric Chemistry
  • Surface Science

Background:

  • Amphiphilic organic compounds are crucial for atmospheric aerosol formation and evolution.
  • Understanding their interfacial behavior is key to predicting atmospheric chemical reactions.
  • The availability of these species to oxidants at the air-water interface remains a challenge.

Purpose of the Study:

  • To quantify the interfacial availability of atmospheric carboxylate ions (Rn-COO-) at the air-water interface.
  • To investigate the influence of chain length, structure, and solvent-accessible surface area (SASA) on interfacial affinity.
  • To elucidate the mechanisms governing carboxylate ion availability under ambient conditions.

Main Methods:

  • Utilized a novel mass spectrometry approach analyzing aqueous microjet breakup.
  • Determined relative interfacial affinities of various carboxylate ions in equimolar solutions.
  • Operated within atmospherically relevant concentrations (1 μM to 1 mM) and ambient conditions.

Main Results:

  • Interfacial affinity of Rn-COO- increases exponentially with chain length and SASA, with an exception for R1-COO-.
  • Established relative affinities: n-heptanoate > cyclohexanecarboxylate > benzoate.
  • Identified strong π-H bonding in benzoate as the cause for its reduced interfacial availability.

Conclusions:

  • The study provides molecular insights into carboxylate ion availability at the air-water interface.
  • Findings are critical for understanding atmospheric aerosol aging and chemical transformations.
  • The developed method offers a new tool for studying interfacial phenomena in atmospheric chemistry.