Abstract
There are several definitions of acids and bases. We are especially interested here in the Brønsted–Lowry definition and its consequences. After reviewing definitions, we shall study the strength concept of acids and bases. It is important because it allows us to predict acid–base reactions.
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- 1.
Svante Arrhenius: swedish chemist (1859–1927), winner of Nobel Prize in Chemistry in 1903. His theory figured in his state thesis defended at Uppsala University when he was 25 years old. His thesis was judged too revolutionary and the examining board was doubtful!
Wilhelm Ostwald: german chemist (1853–1932). He was awarded the Nobel Prize in Chemistry in 1909. His work concerned chemical equilibria. He was one of the mentors of the famous Walther Nernst.
- 2.
In Sect. 4.4, we consider in more detail the structure of the hydrated proton in water, which, at the present time, we write as H+ (w).
- 3.
J. N. Brønsted: danish chemist and biochemist (1879–1947). T. M. Lowry: english chemist (1874–1936).
- 4.
In this book, we symbolize bases by B or B− depending on whether or not they are charged.
- 5.
Alfred Werner: swiss chemist (1866–1919), won the Nobel Prize (1913) in Chemistry. Author of several works concerning complexes (see Part IV).
- 6.
Curiously, neither does an official definition (IUPAC) of K a exist, nor is a name available for it. The definition and the nomenclature used here are those of R. G. Bates in his book, Determination of pH: Theory and Practice, John Wiley and Sons, New York, 1975. The constant K a is also called the acid ionization constant.
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Burgot, JL. (2012). Definitions of Acids and Bases: Strength of Acids and Bases. In: Ionic Equilibria in Analytical Chemistry. Springer, New York, NY. https://doi.org/10.1007/978-1-4419-8382-4_4
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DOI: https://doi.org/10.1007/978-1-4419-8382-4_4
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