Multiple Choice
Which of the following equations correctly shows how the BrO⁻ ion acts as a Bronsted-Lowry base?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
Multiple Choice
In the reaction C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH−(aq), which species acts as the Brønsted-Lowry base?
A
H2O(l)
B
C5H5NH+(aq)
C
C5H5N(aq)
D
OH−(aq)
Verified step by step guidance1
Identify the Brønsted-Lowry acid and base: In a Brønsted-Lowry acid-base reaction, the acid donates a proton (H⁺) and the base accepts a proton.
Examine the reactants: C5H5N(aq) and H2O(l). Determine which species is capable of accepting a proton.
Consider the products: C5H5NH⁺(aq) and OH⁻(aq). The formation of C5H5NH⁺ indicates that C5H5N has accepted a proton.
Recognize that C5H5N(aq) accepts a proton from H2O(l), forming C5H5NH⁺(aq). This makes C5H5N the Brønsted-Lowry base.
Conclude that in this reaction, C5H5N(aq) acts as the Brønsted-Lowry base because it accepts a proton from H2O(l).
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