Multiple Choice
Which of the following equations correctly shows how the BrO⁻ ion acts as a Bronsted-Lowry base?
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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In the chemical equation HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO₂⁻(aq), which species act as Bronsted-Lowry acids?
A
HNO2 and H3O+
B
HNO2 and NO₂⁻
C
H2O and NO₂⁻
D
H2O and H3O+
Verified step by step guidance1
Identify the Bronsted-Lowry acid concept: A Bronsted-Lowry acid is a species that donates a proton (H⁺) to another species.
Examine the chemical equation: HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO₂⁻(aq).
Determine which species donate protons: In the forward reaction, HNO2 donates a proton to H2O, forming H3O⁺ and NO₂⁻.
Recognize the role of H3O⁺: In the reverse reaction, H3O⁺ can donate a proton back to NO₂⁻, reforming HNO2 and H2O.
Conclude which species are Bronsted-Lowry acids: Based on the ability to donate protons, HNO2 and H3O⁺ act as Bronsted-Lowry acids in this equilibrium.
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