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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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Carboxylic acids are the strongest among organic acids, as they readily lose the hydroxyl proton to form a resonance-stabilized carboxylate ion. In comparison, the acid derivatives lack acidic hydrogens directly attached to a functional group. In these compounds, the acidic nature arises from their ability to lose α hydrogens, making them weakly acidic.
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The acidity of carboxylic acids is influenced by the nature of the substituents bounded to the functional group. The acid strength is determined by the stability of the carboxylate anion—the conjugate base formed by dissociating the corresponding carboxylic acid.
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Acid Strength and Molecular Structure03:05

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Binary Acids and Bases
In the absence of any leveling effect, the acid strength of binary compounds of hydrogen with nonmetals (A) increases as the H-A bond strength decreases down a group in the periodic table. For group 17, the order of increasing acidity is HF < HCl < HBr < HI. Likewise, for group 16, the order of increasing acid strength is H2O < H2S < H2Se < H2Te. Across a row in the periodic table, the acid strength of binary hydrogen compounds increases with increasing...
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This lesson delves into a critical aspect of the relative strengths of acids and bases. The strength of an acid is evaluated by the acid dissociation into its conjugate base and a hydronium ion in water. The complete dissociation of a strong acid is confirmed with a very high concentration of hydronium ions. As a result, an incomplete dissociation process affirms a weak acid. Therefore, the equilibrium is in the forward direction for strong acids and backward for weak acids in these reactions.
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In 1923, the Brønsted–Lowry definition of acids and bases was proposed by Johannes Brønsted and Thomas Lowry. According to this theory, a Brønsted acid is defined as a species that donates a proton in a chemical reaction and gets converted to its conjugate base. A Brønsted base is defined as a species that accepts a proton in a chemical reaction and gets converted into its conjugate acid. These transfers of protons are caused by the displacement of electrons in these reactions, which is...
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Basic Remarks on Acidity.

Daniel Himmel1, Valentin Radtke1, Burkhard Butschke1

  • 1Institut für Anorganische und Analytische Chemie and Freiburger Materialforschungszentrum (FMF), Universität Freiburg, Albertstrasse 21, 79104, Freiburg, Germany.

Angewandte Chemie (International Ed. in English)
|November 25, 2017
PubMed
Summary

This review introduces a unified pH scale to understand Brønsted acidity and acid-base chemistry. It also presents a unified redox scale, enabling a comprehensive comparison of all acid-base and redox reactions.

Keywords:
Brønsted aciditychemical potentialpH valuepe valuereducity

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Area of Science:

  • Chemistry
  • Physical Chemistry
  • Chemical Thermodynamics

Background:

  • Brønsted acidity and acid-base chemistry concepts require a unified framework for accurate comparison.
  • Existing scales for acidity and pH present challenges in medium-independent analysis.
  • Analogies between acid-base and redox chemistry can provide deeper insights.

Purpose of the Study:

  • To present a unified view of Brønsted acidity using a novel pH scale.
  • To introduce a unified redox scale analogous to the pH scale.
  • To establish a method for classifying and comparing all acid-base and redox reactions universally.

Main Methods:

  • Overview of acidity, acid strengths, and pH value concepts.
  • Introduction and application of the unified pHabs /pHabsH2O scale.
  • Development of the unified redox scale (peabs).
  • Integration of pHabs and peabs into the protoelectric potential map (PPM).

Main Results:

  • The pHabs scale offers a unifying concept for understanding Brønsted acidity.
  • Unified pHabs values are accessible and applicable in various contexts.
  • The peabs scale provides a unified approach to redox chemistry.
  • The protoelectric potential map (PPM) integrates both scales for comprehensive reaction analysis.

Conclusions:

  • A unified framework for acid-base and redox chemistry is established.
  • The pHabs and peabs scales, combined in the PPM, allow for medium-independent classification and comparison of reactions.
  • This approach provides a powerful tool for understanding chemical reactivity across diverse systems.