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Joshua Mitchell
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They both produce H+ right? How do I tell the difference in a reaction?
What's the difference between an Arrhenius acid and a Bronsted-Lowry acid?
- Thread starter Joshua Mitchell
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- Acid Arrhenius Difference
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SUMMARY
The discussion clarifies the distinction between Arrhenius acids and Bronsted-Lowry acids. Arrhenius acids are defined as substances that produce H+ ions in aqueous solution, while Bronsted-Lowry acids are characterized by their ability to donate protons (H+ ions) in any reaction, not limited to aqueous solutions. The conversation highlights that Bronsted-Lowry theory extends Arrhenius theory by addressing scenarios where Arrhenius does not apply, such as the acidity of FeCl3 in solution.
PREREQUISITES- Understanding of acid-base theories, specifically Arrhenius and Bronsted-Lowry definitions.
- Familiarity with chemical reactions and ionization processes.
- Knowledge of aqueous solutions and their properties.
- Basic grasp of proton donation and acceptance in chemical reactions.
- Research the specific characteristics of Arrhenius acids and their limitations.
- Study the Bronsted-Lowry acid-base theory in detail.
- Explore examples of acid-base reactions that illustrate both theories.
- Investigate the behavior of metal chlorides, such as FeCl3, in aqueous solutions.
Chemistry students, educators, and professionals seeking to deepen their understanding of acid-base theories and their applications in various chemical reactions.
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