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Related Concept Videos

Acid/Base Strengths and Dissociation Constants03:02

Acid/Base Strengths and Dissociation Constants

63.5K
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:
63.5K
Strong Acid and Base Solutions03:22

Strong Acid and Base Solutions

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A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
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Titration of a Weak Base with a Strong Acid01:20

Titration of a Weak Base with a Strong Acid

5.8K
The titration curve of a weak base like ammonia with a strong acid like hydrochloric acid is the mirror image of the titration curve of a weak acid with a strong base.
Using the ICE table and substituting the Kb value, we calculate the initial pH of 50 mL of 0.1 M ammonia to be 11.11. Addition of 25 mL of 0.1 M hydrochloric acid to this solution of ammonia results in a buffer with an equal concentration of ammonia and ammonium ions. The pH of this buffer can be calculated by substituting these...
5.8K
Titration of a Strong Acid with a Strong Base01:23

Titration of a Strong Acid with a Strong Base

6.4K
During the titration of a strong acid with a strong base, pH calculations are primarily based on the concentration of residual hydronium or hydroxide ions. Initially, a strong acid like hydrochloric acid fully dissociates, creating hydronium and chloride ions, resulting in a low pH. The addition of a strong base like sodium hydroxide alters the concentration of hydronium ions by neutralizing them. As more base is added, the pH gradually increases. At the equivalence point, all hydronium ions...
6.4K
Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

1.9K
Titration of a polyprotic acid, which contains multiple ionizable protons, involves distinct dissociation steps, each with its own dissociation constant (Ka). Each successive Ka is weaker than the previous one. In the titration of a polyprotic acid like sulfurous acid with a strong base such as sodium hydroxide, the base first neutralizes the initial ionizable proton, forming an intermediate species (e.g., hydrogen sulfite ions). This step's titration curve resembles that of a weak...
1.9K
Titration of Polyprotic Base with a Strong Acid01:18

Titration of Polyprotic Base with a Strong Acid

884
The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...
884

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Measurement and Analysis of Extracellular Acid Production to Determine Glycolytic Rate
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Strong Bases Design: Predicted Limits of Basicity.

Andrey V Kulsha1, Ekaterina G Ragoyja1, Oleg A Ivashkevich2

  • 1Chemical Department, Belarusian State University, 4 Nezavisimosti Avenue, 220030 Minsk, Republic of Belarus.

The Journal of Physical Chemistry. A
|June 3, 2022
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Researchers investigated the instability of strong neutral bases using quantum-chemical calculations. They propose a new, stable superbase for organic chemistry applications, potentially advancing C-H bond activation.

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Area of Science:

  • Organic Chemistry
  • Computational Chemistry
  • Physical Chemistry

Background:

  • Brønsted superbases are crucial for activating C-H bonds in organic synthesis.
  • Substituted aminophosphazenes represent the strongest neutral bases to date, developed in the late 1980s.
  • Ongoing research aims to synthesize even stronger neutral bases for enhanced chemical reactivity.

Purpose of the Study:

  • To investigate the theoretical reasons behind the instability of highly basic compounds.
  • To establish theoretical limits for basicity in both solution and gas phases.
  • To propose a novel, stable superbase synthesizable under ambient conditions.

Main Methods:

  • High-level quantum-chemical calculations were employed to analyze molecular stability and basicity.
  • Theoretical models were used to predict basicity limits in different environments.
  • Hexamethylphosphoramide was identified as a suitable ionizing solvent for superbases.

Main Results:

  • The study elucidates the factors contributing to the instability of extremely basic molecules.
  • Theoretical basicity limits were determined for gas-phase and solution-phase conditions.
  • A promising candidate for a record-breaking, stable superbase at ambient conditions was identified.

Conclusions:

  • Understanding instability is key to designing stable, potent superbases.
  • The proposed superbase offers potential for significant advancements in C-H bond activation.
  • Hexamethylphosphoramide is a viable solvent for working with these powerful bases.