Multiple Choice
Which of the following explains why HCO3^- is a stronger conjugate base than CO3^2^-?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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In the Brønsted–Lowry model, what is the conjugate base of after it donates a proton?
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Verified step by step guidance1
Recall that in the Brønsted–Lowry acid-base theory, an acid is a species that donates a proton (H\^+), and the species that remains after the proton is lost is called the conjugate base.
Identify the acid given in the problem, which is hydrogen iodide (HI). This molecule can donate a proton (H\^+) to another species.
When HI donates a proton, it loses an H\^+ ion, so the remaining species is the iodide ion (I\^-).
Write the conjugate base of HI as I\^- to represent the species after proton donation.
Therefore, the conjugate base of HI in the Brønsted–Lowry model is the iodide ion, I\^-.
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