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Related Concept Videos

Acid/Base Strengths and Dissociation Constants03:02

Acid/Base Strengths and Dissociation Constants

The relative strength of an acid or base is the extent to which it ionizes when dissolved in water. If the ionization reaction is essentially complete, the acid or base is termed strong; if relatively little ionization occurs, the acid or base is weak. There are many more weak acids and bases than strong ones. The most common strong acids and bases are listed below:
Acid and Bases: Ka, pKa, and Relative Strengths02:35

Acid and Bases: Ka, pKa, and Relative Strengths

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.
Relative Strengths of Conjugate Acid-Base Pairs02:29

Relative Strengths of Conjugate Acid-Base Pairs

Brønsted-Lowry acid-base chemistry is the transfer of protons; thus, logic suggests a relation between the relative strengths of conjugate acid-base pairs. The strength of an acid or base is quantified in its ionization constant, Ka or Kb, which represents the extent of the acid or base ionization reaction. For the conjugate acid-base pair HA / A−, the ionization equilibrium equations and ionization constant expressions are
Solution Composition During Acid/Base Titrations01:17

Solution Composition During Acid/Base Titrations

The titration of a weak acid with a strong base results in the formation of water and the conjugate base of the acid. For instance, titrating acetic acid with sodium hydroxide leads to the formation of water and sodium acetate. A solution of acetic acid and sodium acetate constitutes a buffer whose relative concentration at different stages of the titration is indicated by the α values, which represent percentages of the weak acid and its conjugate base.
The α0 and α1 values represent the...
Titration of a Weak Acid with a Strong Base01:30

Titration of a Weak Acid with a Strong Base

In titrating a weak acid with a strong base, different calculation methods are applied at various stages. Initially, the pH of a weak acid like acetic acid is calculated using its dissociation constant (Ka) and an ICE table. Upon addition of a strong base such as sodium hydroxide, a buffer forms, and its pH is determined using the Henderson-Hasselbalch equation. As more base is added and the titration reaches the halfway point, the pH becomes equal to the pKa of the acid, indicating equal...
Polyprotic Acids03:38

Polyprotic Acids

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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Related Experiment Video

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Determination of the Gas-phase Acidities of Oligopeptides
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Determination of the Gas-phase Acidities of Oligopeptides

Published on: June 24, 2013

Equilibrium acidities of superacids.

Agnes Kütt1, Toomas Rodima, Jaan Saame

  • 1Institute of Chemistry, University of Tartu, Ravila 14a, Tartu, 50411, Estonia.

The Journal of Organic Chemistry
|December 21, 2010
PubMed
Summary

This study presents the most comprehensive equilibrium superacidity scale, measuring molecular acidities in a constant 1,2-dichloroethane medium. This new scale provides crucial data for designing and utilizing superacidic molecules.

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Area of Science:

  • Chemistry
  • Physical Chemistry
  • Acid-Base Chemistry

Background:

  • Superacidity research traditionally focused on media acidity, limiting molecular characterization.
  • Existing scales often lack comprehensive data across diverse acid types.
  • A need exists for a standardized scale measuring intrinsic molecular acidities.

Purpose of the Study:

  • To establish the most comprehensive equilibrium superacidity scale to date.
  • To characterize the intrinsic acidities of 62 diverse superacids and mineral acids.
  • To provide a complementary scale to the H(0) scale for detailed acidity analysis.

Main Methods:

  • Utilized 1,2-dichloroethane (DCE) as a constant composition solvent with weak basicity and high polarity.
  • Performed 176 interlinked relative acidity measurements.
  • Developed a scale spanning 15 orders of magnitude.

Main Results:

  • Reported DCE acidities for numerous superacids (e.g., triflic acid, bis(triflyl)imide) and mineral acids (sulfuric acid, hydroiodic acid).
  • Established a superacidity scale covering a 15-order-of-magnitude range.
  • The scale ranges from picric acid to 1,1,2,3,3-pentacyanopropene.

Conclusions:

  • The developed superacidity scale offers a robust tool for understanding and quantifying molecular acidities.
  • This scale is valuable for the design, application, and further study of superacidic compounds.
  • The findings advance the field of superacidity by providing a standardized and comprehensive measurement system.