Explore the Brønsted-Lowry acid-base concept, which defines acids as proton donors and bases as proton acceptors. This theory extends beyond Arrhenius's definition, covering acid-base behavior in various solvents. It includes water's amphoteric behavior, common acids like HCl and H2SO4, bases such as NaOH and NH3, and the formation of conjugate acid-base pairs. Neutralization reactions and the relative strengths of acids and bases are also discussed, highlighting their importance in chemical reactions and industrial applications.
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Acids are substances that dissociate in water to yield hydrogen ions (H+) and bases are substances that produce hydroxide ions (OH-) in solution
Acids are defined as proton (H+) donors and bases as proton acceptors, applicable in any solvent system
The Brønsted-Lowry theory allows for a more comprehensive understanding of acid-base behavior in various chemical environments, not just aqueous solutions
Water can function as both an acid and a base, depending on the context of the chemical reaction
Water can donate a proton to a base, transforming into the hydroxide ion (OH-) or accept a proton from an acid, becoming the hydronium ion (H3O+)
The Brønsted-Lowry theory effectively describes the versatile role of water in acid-base chemistry, accommodating its ability to switch between acting as an acid or a base
Examples of Brønsted-Lowry acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3), and acetic acid (CH3COOH)
Examples of Brønsted-Lowry bases include sodium hydroxide (NaOH), potassium hydroxide (KOH), ammonia (NH3), and sodium bicarbonate (NaHCO3)
The Brønsted-Lowry theory introduces the concept of conjugate acid-base pairs, formed in acid-base reactions
Neutralization is a fundamental reaction in acid-base chemistry where an acid and a base react to form a salt and usually water
00
The ______-______ theory expanded the definition of acids and bases beyond the ______ theory's limitations.
Brønsted-Lowry
Arrhenius
01
In the Brønsted-Lowry framework, acids are identified as proton (______) ______, and bases as proton ______, which can be applied in any solvent, not limited to ______ solutions.
H+
donors
acceptors
aqueous
02
Water acting as a base
Water accepts a proton, forming H3O+; seen in reaction with acids like CH3COOH.
