Open Question
The conjugate acid of H2O is ________.
17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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Which of the following equations correctly shows how the ClO⁻ ion acts as a Bronsted-Lowry base?
A
ClO⁻ + OH⁻ → ClO⁻ + H₂O
B
ClO⁻ + H⁺ → HClO
C
ClO⁻ + H₂O → ClO⁻ + H₂O
D
ClO⁻ + H₂O → HClO + OH⁻
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 ClO⁻ in the reaction: As a Bronsted-Lowry base, ClO⁻ should accept a proton from another molecule.
Examine the given reactions: Look for the reaction where ClO⁻ accepts a proton from another molecule, resulting in the formation of a new product.
Analyze the correct equation: In the equation ClO⁻ + H₂O → HClO + OH⁻, ClO⁻ accepts a proton from H₂O, forming HClO and releasing OH⁻.
Conclude the reasoning: The correct equation demonstrates ClO⁻ acting as a Bronsted-Lowry base by accepting a proton from water, which aligns with the definition of a Bronsted-Lowry base.
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