Textbook Question
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. c. KOH(aq)
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Ch.16 - Acids and Bases
Chapter 16, Problem 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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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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02:08
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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01:30Conjugate 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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Related Practice
Open Question
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base in aqueous solution according to the Arrhenius definition. a. NaOH(aq) b. H2SO4(aq) c. HBr(aq) d. Sr(OH)2(aq)
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. a. H2CO3(aq) + H2O(l) ⇌ H3O+(aq) + HCO3–(aq) c. HNO3(aq) + H2O(l) → H3O+(aq) + NO3–(aq)
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Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. d. C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH–(aq)
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Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH–(aq)
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Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO32–(aq) + H2O(l) ⇌ HCO3–(aq) + OH–(aq)
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