Acid-base chemistry explores the reactions between acids and bases, resulting in salt and water. It includes the pH scale, which measures acidity or basicity, and the Brønsted-Lowry theory, defining acids as proton donors and bases as proton acceptors. Polyprotic acids can donate multiple protons, while neutralization reactions involve strong acids and bases. The Lewis theory extends to electron pair transfers, forming complex ions.
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Acid-base reactions involve the transfer of a proton from an acid to a base, resulting in the formation of a salt and water
The general equation for an acid-base reaction is Acid + Base → Salt + Water
The reaction between hydrochloric acid and sodium hydroxide is an example of an acid-base reaction, producing sodium chloride and water
The pH scale is a logarithmic scale that measures the acidity or basicity of a solution based on the concentration of hydrogen ions present
The pH scale is categorized into acidic, neutral, and basic regions, with lower pH values indicating higher acidity
Understanding the pH scale is crucial for predicting the behavior of substances in acid-base reactions and assessing the strengths of acids and bases
The Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors, with water being amphoteric and able to serve as both an acid and a base
The relative strengths of acids and bases can be compared using the acid dissociation constant (Ka) and base dissociation constant (Kb), which measure their tendency to donate or accept protons in water
Polyprotic acids have the ability to donate more than one proton per molecule in acid-base reactions, with their degree of dissociation influenced by the pH and other reactants in the environment
Neutralization reactions are a subset of acid-base reactions where a strong acid reacts with a strong base to produce a salt and water, resulting in a neutral solution
Examples of strong acids include hydrochloric acid and sulfuric acid, while examples of strong bases include sodium hydroxide and potassium hydroxide
The Lewis acid-base theory focuses on the transfer of electron pairs rather than protons, with Lewis acids accepting electron pairs and Lewis bases donating them
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Definition of acid-base reaction
Chemical process where acid donates H+ to base, forming salt and water.
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Role of acids in acid-base reactions
Substances donating proton (H+), often becoming positively charged ions.
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Role of bases in acid-base reactions
Substances accepting proton (H+), typically becoming negatively charged ions.
