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Weak Acid Solutions

Weak Acid Solutions

Few compounds act as strong acids. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Weak acids are commonly encountered in nature, being the substances partly responsible for the tangy taste of citrus fruits, the stinging sensation of insect bites, and the unpleasant smells associated with body odor. A familiar example of a...

Titration Calculations: Weak Acid - Strong Base

Titration Calculations: Weak Acid - Strong Base

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:

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Mixtures of Gases: Dalton's Law of Partial Pressures and Mole Fractions

Unless individual gases chemically react with each other, the individual gases in a mixture of gases do not affect each other’s pressure. Each gas in a mixture exerts the same pressure that it would exert if it were present alone in the container. The pressure exerted by each individual gas in a mixture is called its partial pressure.

Titration of a Weak Acid with a Weak Base

Titration of a Weak Acid with a Weak Base

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...

Weak Base Solutions

Weak Base Solutions

Some compounds produce hydroxide ions when dissolved by chemically reacting with water molecules. In all cases, these compounds react only partially and so are classified as weak bases. These types of compounds are also abundant in nature and important commodities in various technologies. For example, global production of the weak base ammonia is typically well over 100 metric tons annually, being widely used as an agricultural fertilizer, a raw material for chemical synthesis of other...

Titration of a Polyprotic Acid

Titration of a Polyprotic Acid

A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process. If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three...

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Predicting Mole-Fraction-Dependent Dissociation for Weak Acids.

Jan Blasius¹, Johannes Ingenmey¹, Eva Perlt²

¹Mulliken Center for Theoretical Chemistry, Universität Bonn, Beringstr. 4, 53115, Bonn, Germany.

Angewandte Chemie (International Ed. in English)

|December 28, 2018

Summary

The binary quantum cluster equilibrium (bQCE) approach accurately predicts acid strengths across all concentrations. This method offers valuable insights into ionization processes in concentrated solutions.

Keywords:

acetic acid acid strength bQCE conductivity maximum formic acid

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Area of Science:

Physical Chemistry
Computational Chemistry
Solution Chemistry

Background:

Understanding acid-base behavior in solutions is crucial for various chemical and biological systems.
Predicting acid strengths, especially in highly concentrated solutions, presents significant challenges.
Existing models often struggle to capture the complex interactions governing ionization processes.

Purpose of the Study:

To evaluate the binary quantum cluster equilibrium (bQCE) approach for predicting acid strengths in aqueous solutions.
To assess the bQCE method's ability to model complex acid-water interactions across a wide concentration range.
To validate calculated ion concentrations against experimental conductivity data.

Main Methods:

Application of the binary quantum cluster equilibrium (bQCE) approach to formic acid and acetic acid in water.
Calculation of acid strengths and ion concentrations as a function of acid mole fraction.
Comparison of predicted ion concentrations with experimental conductivity measurements.

Main Results:

The bQCE approach successfully predicts acid strengths over the entire concentration range studied.
Acid strength exhibits complex concentration dependence, influenced by the interplay of molecules and ions.
Calculated ion concentrations show excellent agreement with experimental conductivity for acetic acid and satisfactory agreement for formic acid.

Conclusions:

The bQCE method is a valuable tool for predicting acid strengths and ionization processes, even in highly concentrated solutions.
The approach requires only a limited number of quantum-chemical calculations, making it computationally efficient.
bQCE is applicable to both aqueous and non-aqueous solutions, broadening its utility in chemical and biological research.