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Chemistry Chapter 10 : Topic 1
Brønsted–Lowry Acids and Bases
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In the Bronsted-Lowry theory, acids are best defined as substances that:
Reasoning: Bronsted-Lowry acids are proton (H⁺) donors, meaning they release or transfer a proton to another species.
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A Bronsted-Lowry base is a substance that:
Reasoning: A base in Bronsted-Lowry theory is defined as a proton acceptor, not necessarily containing OH⁻.
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Which statement correctly describes the reaction between HCl and water according to Bronsted-Lowry theory?HCl+H₂O → H₃O⁺+Cl⁻
Reasoning: HCl donates a proton (acid), and water accepts it (base), forming H₃O⁺ .
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In the reaction NH₃+H₂O ⇌ NH₄⁺+OH⁻, ammonia acts as:
Reasoning: NH₃ accepts a proton from water, so it behaves as a base.
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Which of the following best explains why water is considered amphoteric?
Reasoning: Water can act as both proton donor and acceptor, making it amphoteric.
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In the reaction H₂O+NH₃ ⇌ NH₄⁺+OH⁻, which species acts as the proton donor?
Reasoning: Water donates a proton to ammonia, acting as the acid.
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Which of the following pairs represents a conjugate acid-base pair?
Reasoning: NH₃ gains a proton to become NH₄⁺, forming a conjugate pair.
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A substance that increases H⁺ concentration in solution according to Brønsted-Lowry theory is:
Reasoning: Increasing H⁺ concentration indicates proton donation, hence an acid.
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Which species acts as a base in the reaction?HCl+NH₃ → NH₄⁺+Cl⁻
Reasoning: NH₃ accepts a proton from HCl, so it is the base.
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Which statement about Bronsted-Lowry acids and bases is correct?
Reasoning: The theory is based on proton (H⁺) transfer, not composition or medium.
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In the reaction H₂SO₄+H₂O → H₃O⁺+HSO₄⁻, sulfuric acid acts as:
Reasoning: H₂SO₄ donates a proton to water, acting as an acid.
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Which of the following species can act both as an acid and a base?
Reasoning: Water can both donate and accept protons depending on the reaction.
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A Bronsted-Lowry base is best described as a substance that:
Reasoning: Bases accept H⁺ and form conjugate acids.
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Which of the following reactions shows NH₃ acting as a proton acceptor?
Reasoning: NH₃ accepts a proton from water forming NH₄⁺.
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Which of the following correctly identifies the role of water in the reaction with HCl?HCl+H₂O → H₃O⁺+Cl⁻
Reasoning: Water accepts a proton from HCl forming hydronium ion.
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Which of the following is NOT consistent with Bronsted-Lowry theory?
Reasoning: Producing OH⁻ is related to Arrhenius bases, not Bronsted-Lowry acids.
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In Bronsted-Lowry theory, the conjugate base of an acid is formed when the acid:
Reasoning: Removing a proton from an acid forms its conjugate base.
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In a proton transfer reaction, the species formed after an acid donates a proton is called:
Reasoning: Loss of a proton from an acid forms its conjugate base.
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