Podcast
Questions and Answers
According to the Arrhenius definitions of acids and bases, which of these are bases? (Select all that apply)
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the Bronsted-Lowry acid?
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the conjugate base?
In the reaction HCO3− + H2S → H2CO3 + HS−, which is the Bronsted-Lowry base?
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In the reaction HCO3− + H2S → H2CO3 + HS−, which is the conjugate acid?
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Identify the Lewis base in the equation Fe3+ + H2O → Fe(H2O)6^3+
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Identify the Lewis acid in the equation N(CH3)3 + BH3 → (CH3)3N:BH3
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How does water behave in this reaction? Which definition of acids and bases would you apply?
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Which is a characteristic of a Lewis base?
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What is the Bronsted-Lowry definition of an acid?
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Which statement best describes a Bronsted-Lowry base?
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Study Notes
Arrhenius Acids and Bases
- Arrhenius Base Examples: Ba(OH)₂ and CsOH are classified as bases according to Arrhenius definitions due to their ability to produce hydroxide ions (OH⁻) in solution.
- Definition of Arrhenius Acids and Bases: Acids increase the concentration of hydrogen ions (H⁺) in water, while bases increase hydroxide ion (OH⁻) concentration.
Bronsted-Lowry Acids and Bases
- Bronsted-Lowry Acid in Reaction: NH₄⁺ acts as the Bronsted-Lowry acid as it donates a proton in the reaction with HPO₄²⁻.
- Conjugate Base: NH₃ is the conjugate base formed after NH₄⁺ donates a proton, indicating it can accept a proton back in reverse reactions.
- Bronsted-Lowry Base in Reaction: HCO₃⁻ functions as the Bronsted-Lowry base by accepting a proton in the reaction with H₂S.
- Conjugate Acid: H₂CO₃ is the conjugate acid produced when HCO₃⁻ gains a proton during the reaction.
Lewis Acids and Bases
- Lewis Base Identification: In the formation of Fe(H₂O)₆³⁺, H₂O acts as a Lewis base as it donates a pair of electrons to Fe³⁺.
- Lewis Acid Identification: BH₃ is recognized as a Lewis acid because it accepts electron pairs from Lewis bases like (CH₃)₃N.
Water's Role in Acid-Base Reactions
- Water as a Base: In specific reactions, water can act as a Bronsted-Lowry base by accepting a proton, resulting in the formation of hydronium ion (H₃O⁺).
Characteristics of Lewis Bases
- Electron Donor: A defining characteristic of Lewis bases is their ability to donate electron pairs to other species.
Bronsted-Lowry Acid Definition
- Proton Donation: A Bronsted-Lowry acid is defined as any compound that donates protons (H⁺ ions).
Bronsted-Lowry Base Definition
- Proton Acceptance: The Bronsted-Lowry base must accept protons to form a conjugate acid, emphasizing its role in proton transfer reactions.
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Description
Test your understanding of Arrhenius, Bronsted-Lowry, and Lewis definitions of acids and bases with these flashcards. Each card presents questions that challenge you to identify acids and bases in various reactions. Perfect for chemistry students looking to reinforce their knowledge on this fundamental topic.
