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Questions and Answers
According to the Arrhenius definitions of acids and bases, choose the bases from the list of acids and bases. Check all that apply.
According to the Arrhenius definitions of acids and bases, choose the bases from the list of acids and bases. Check all that apply.
- a (correct)
- d (correct)
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the Bronsted-Lowry acid?
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the Bronsted-Lowry acid?
NH4+
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the conjugate base?
In the reaction NH4+ + HPO42− → NH3 + H2PO4−, which is the conjugate base?
H2PO4−
In the reaction HCO3− + H2S → H2CO3 + HS−, which is the Bronsted-Lowry base?
In the reaction HCO3− + H2S → H2CO3 + HS−, which is the Bronsted-Lowry base?
In the reaction HCO3− + H2S → H2CO3 + HS−, which is the conjugate acid?
In the reaction HCO3− + H2S → H2CO3 + HS−, which is the conjugate acid?
Identify the Lewis base in this balanced equation.
Identify the Lewis base in this balanced equation.
Identify the Lewis acid in this balanced equation.
Identify the Lewis acid in this balanced equation.
Explain how water behaves in this reaction. Which definition of acids and bases would you apply?
Explain how water behaves in this reaction. Which definition of acids and bases would you apply?
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Study Notes
Arrhenius Acids and Bases
- Arrhenius acids produce H⁺ ions in solution; bases produce OH⁻ ions.
- Identify bases from substances according to Arrhenius definitions.
Bronsted-Lowry Acid and Base Concept
- Bronsted-Lowry acids donate protons (H⁺); bases accept protons.
- In the reaction NH₄⁺ + HPO₄²⁻ → NH₃ + H₂PO₄⁻:
- NH₄⁺ acts as a Bronsted-Lowry acid by donating a proton.
Conjugate Bases
- A conjugate base is formed when an acid donates a proton.
- In the same reaction, the conjugate base of NH₄⁺ is NH₃.
Bronsted-Lowry Base Identification
- A Bronsted-Lowry base accepts a proton during a reaction.
- In the reaction HCO₃⁻ + H₂S → H₂CO₃ + HS⁻:
- HCO₃⁻ functions as the Bronsted-Lowry base by accepting a proton.
Conjugate Acids
- A conjugate acid is what remains after a base accepts a proton.
- In the reaction with HCO₃⁻, H₂CO₃ is identified as the conjugate acid.
Lewis Acids and Bases
- Lewis acids accept electron pairs; Lewis bases donate electron pairs.
- Identify Lewis bases and acids in chemical equations to understand their roles.
Water’s Role in Acid-Base Reactions
- Water can act as both an acid and a base depending on the reaction context.
- Evaluate which acid-base definition (Arrhenius, Bronsted-Lowry, or Lewis) applies based on water's behavior in reactions.
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