Multiple Choice
In the Brønsted–Lowry model, what is the conjugate acid of the sulfate ion (i.e., )?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
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In the Brønsted–Lowry framework, what is the conjugate acid of (HS−)?
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Verified step by step guidance1
Recall that in the Brønsted–Lowry acid-base theory, a conjugate acid is formed when a base gains a proton (H\^+).
Identify the species given: HS\^− (hydrogen sulfide ion) acts as a base in this context because it can accept a proton.
Add one proton (H\^+) to HS\^− to form its conjugate acid. This means increasing the number of hydrogen atoms by one while keeping the charge balanced.
Write the formula for the conjugate acid by adding H\^+ to HS\^−, resulting in H\_2S (dihydrogen sulfide), which is neutral.
Confirm that the conjugate acid has one more proton than the base and that the charge is adjusted accordingly, verifying that H\_2S is the correct conjugate acid of HS\^−.
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