Open Question
Which compound forms a powerful acid and also contains a halogen? H2S, HBr, Li2O, or LiBr?
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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Which of the following equations correctly shows how the BrO⁻ ion acts as a Bronsted-Lowry base?
A
BrO⁻ + H₂O → HBrO + OH⁻
B
BrO⁻ + OH⁻ → BrO⁻ + H₂O
C
BrO⁻ + H₂O → BrO⁻ + H₂O
D
BrO⁻ + H⁺ → BrOH
Verified step by step guidance1
Understand the concept of a Bronsted-Lowry base: A Bronsted-Lowry base is a substance that can accept a proton (H⁺) from another substance.
Identify the role of BrO⁻ in the given options: As a Bronsted-Lowry base, BrO⁻ should be accepting a proton from another molecule.
Examine the first equation: BrO⁻ + H₂O → HBrO + OH⁻. Here, BrO⁻ accepts a proton from H₂O, forming HBrO and releasing OH⁻, which is consistent with the behavior of a Bronsted-Lowry base.
Review the other options: In BrO⁻ + OH⁻ → BrO⁻ + H₂O and BrO⁻ + H₂O → BrO⁻ + H₂O, there is no proton transfer involving BrO⁻, so these do not demonstrate Bronsted-Lowry base behavior.
Consider the last option: BrO⁻ + H⁺ → BrOH. While BrO⁻ accepts a proton, the equation does not involve water, which is typically present in Bronsted-Lowry acid-base reactions. The first equation is more representative of the concept.
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