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Indicators02:39

Indicators

48.6K
Certain organic substances change color in dilute solution when the hydronium ion concentration reaches a particular value. For example, phenolphthalein is a colorless substance in any aqueous solution with a hydronium ion concentration greater than 5.0 × 10−9 M (pH < 8.3). In more basic solutions where the hydronium ion concentration is less than 5.0 × 10−9 M (pH > 8.3), it is red or pink. Substances such as phenolphthalein, which can be used to determine the pH of a solution, are...
48.6K
Titration of a Weak Acid with a Weak Base01:08

Titration of a Weak Acid with a Weak Base

2.8K
Weak acids and bases do not undergo dissociation completely, and titrations between these two are rarely studied. When such studies are performed, say, for the titration of a weak acid with a weak base, the titration curve plots the change in pH as a function of the volume of base added. Take the titration of acetic acid with ammonia, for instance. During the titration, these two species form ammonium acetate and water, but the pH change is slow and gradual.
As a result, there is no simple...
2.8K
Strong Acid and Base Solutions03:22

Strong Acid and Base Solutions

31.7K
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.
31.7K
Titration of a Strong Acid with a Strong Base01:23

Titration of a Strong Acid with a Strong Base

5.4K
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...
5.4K
Titration of a Weak Acid with a Strong Base01:30

Titration of a Weak Acid with a Strong Base

2.2K
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...
2.2K
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

44.3K
Calculating pH for Titration Solutions: Weak Acid/Strong Base
For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as:
44.3K

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Synthesis of pH Dependent Pyrazole, Imidazole, and Isoindolone Dipyrrinone Fluorophores using a Claisen-Schmidt Condensation Approach
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pH Indicators for Strong Molecular Bases: A Theoretical Approach.

Andrey V Kulsha1, Oleg A Ivashkevich2

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

The Journal of Physical Chemistry. A
|May 31, 2024
PubMed
Summary
This summary is machine-generated.

This study theoretically explores transition points in hexamethylphosphoramide (HMPA) using novel acid-base indicators. New indicators were designed, establishing a basicity scale for highly basic HMPA solutions.

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Area of Science:

  • Chemistry
  • Physical Chemistry
  • Analytical Chemistry

Background:

  • Hexamethylphosphoramide (HMPA) is a unique solvent with high basicity.
  • Understanding transition points in HMPA is crucial for its application in acid-base chemistry.
  • Existing basicity scales are limited for extremely basic environments.

Purpose of the Study:

  • To theoretically investigate the transition points of acid-base indicators in HMPA.
  • To design novel acid-base indicators suitable for highly basic HMPA solutions.
  • To establish a general basicity scale for HMPA, extending beyond known molecular bases.

Main Methods:

  • Theoretical study of transition points in hexamethylphosphoramide.
  • Design of three new acid-base indicators featuring multiple transition points.
  • Development of deeply colored, low-nucleophilic anions for indicator design.

Main Results:

  • Successfully designed three novel acid-base indicators for HMPA.
  • These indicators possess multiple transition points and exhibit deep coloration.
  • A comprehensive basicity scale for HMPA solutions was established.

Conclusions:

  • The theoretical study provides insights into indicator behavior in HMPA.
  • The designed indicators are effective for characterizing highly basic HMPA solutions.
  • This work expands the fundamental understanding of basicity scales in non-aqueous systems.