Multiple Choice
In the Brønsted–Lowry framework, what is the conjugate acid of (HS−)?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
Multiple Choice
According to the Brønsted–Lowry definition, what is the conjugate acid of ?
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Verified step by step guidance1
Recall the Brønsted–Lowry acid-base theory, which defines an acid as a proton (H⁺) donor and a base as a proton acceptor.
Identify the species given: water (H₂O) can act as a base by accepting a proton (H⁺).
Determine the conjugate acid of H₂O by adding a proton (H⁺) to it, since the conjugate acid is formed when a base gains a proton.
Write the chemical formula for the conjugate acid formed by protonating H₂O, which is H₃O⁺ (hydronium ion).
Conclude that according to the Brønsted–Lowry definition, the conjugate acid of H₂O is H₃O⁺.
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