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Ch.16 - Acids and Bases
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.16 - Acids and BasesProblema 35b
Capitolo 16, Problema 35b

In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH–(aq)

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Identify the Brønsted–Lowry acid and base in the reactants: The Brønsted–Lowry acid is the species that donates a proton (H+), and the Brønsted–Lowry base is the species that accepts a proton.
In the reaction NH3(aq) + H2O(l) -> NH4+(aq) + OH-(aq), identify which species donates a proton and which accepts it.
Recognize that H2O donates a proton to NH3, making H2O the Brønsted–Lowry acid and NH3 the Brønsted–Lowry base.
Identify the conjugate acid and conjugate base in the products: The conjugate acid is formed when the base gains a proton, and the conjugate base is formed when the acid loses a proton.
In the products, NH4+ is the conjugate acid (formed from NH3), and OH- is the conjugate base (formed from H2O).

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Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework allows for a broader understanding of acid-base reactions beyond just the presence of hydroxide ions or hydronium ions. In this context, identifying the roles of substances in a reaction involves determining which species donates a proton and which accepts it.
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Bronsted-Lowry Acid-Base Theory

Conjugate Acid and Base

In the Brønsted–Lowry framework, a conjugate acid is formed when a base accepts a proton, while a conjugate base is what remains after an acid donates a proton. This relationship is crucial for understanding the dynamic nature of acid-base reactions, as it illustrates how substances can transform into different species depending on their interactions.
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Conjugate Acid-Base Pairs

Equilibrium in Acid-Base Reactions

Acid-base reactions often reach a state of equilibrium, where the rates of the forward and reverse reactions are equal. This concept is important for predicting the direction of a reaction and understanding the relative strengths of acids and bases involved. In the given reaction, recognizing the equilibrium helps in identifying the predominant species present in solution.
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Acid-Base Reaction
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