Question:
What is the conjugate base of \(H_2CO_3\) according to the Bronsted-Lowry theory?
What is the conjugate base of \(H_2CO_3\) according to the Bronsted-Lowry theory?
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A conjugate base is formed when an acid loses a proton.
Updated On: Dec 11, 2025
- \(CO_3^{2-}\)
- \(HCO_3^-\)
- \(H_3CO_3^+\)
- \(CO_2\)
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The Correct Option is B
Solution and Explanation
The conjugate base of an acid is what remains after the acid donates a proton. In this case, \(H_2CO_3\) (carbonic acid) donates a proton to become \(HCO_3^-\), which is the conjugate base.
Thus, the correct answer is (b).
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