Explain theory of Arrhenius with 10examples. Incorrect answer will be reported.
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In 1884, the Swedish chemist Svante Arrhenius proposed two specific classifications of compounds, termed acids and bases. When dissolved in an aqueous solution, certain ions were released into the solution. The Arrhenius definition of acid-base reactions is a development of the "hydrogen theory of acids". It was used to provide a modern definition of acids and bases, and followed from Arrhenius's work with Friedrich Wilhelm Ostwald in establishing the presence of ions in aqueous solution in 1884. This led to Arrhenius receiving the Nobel Prize in Chemistry in 1903.
An Arrhenius acid is a compound that increases the concentration of H+ ions that are present when added to water. These H+ ions form the hydronium ion ( H3O+ ) when they combine with water molecules. This process is represented in a chemical equation by adding H2O to the reactants side.
HCl(aq)→H+(aq)+Cl−(aq)(16.1.1)
In this reaction, hydrochloric acid ( HCl ) dissociates into hydrogen ( H+ ) and chlorine ( Cl− ) ions when dissolved in water, thereby releasing H+ ions into solution. Formation of the hydronium ion equation:
HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)(16.1.2)
The Arrhenius definitions of acidity and alkalinity are restricted to aqueous solutions and refer to the concentration of the solvated ions. Under this definition, pure H2SO4 or HCl dissolved in toluene are not acidic, despite the fact that both of these acids will donate a proton to toluene. In addition, under the Arrhenius definition, a solution of sodium amide ( NaNH2 ) in liquid ammonia is not alkaline, despite the fact that the amide ion ( NH−2 ) will readily deprotonate ammonia. Thus, the Arrhenius definition can only describe acids and bases in an aqueous environment.
Limitation of the Arrhenius Definition of Acids and Bases
The Arrhenius definition can only describe acids and bases in an aqueous environment.
In chemistry, acids and bases have been defined differently by three sets of theories: One is the Arrhenius definition defined above, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen ( H+ ) ions while bases produce hydroxide ( OH− ) ions in solution. The other two definitions are discussed in detail alter in the chapter and include the Brønsted-Lowry definition the defines acids as substances that donate protons ( H+ ) whereas bases are substances that accept protons and the Lewis theory of acids and bases states that acids are electron pair acceptors while bases are electron pair donors.
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