Multiple Choice
Which of the following represents the reaction when a weak base, B, is dissolved in water?
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17. Acid and Base Equilibrium
Bronsted-Lowry Acids and Bases
Multiple Choice
In the Brønsted–Lowry model, what is the conjugate acid of the sulfate ion (i.e., )?
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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\(\textsuperscript{+}\)).
Identify the given base: the sulfate ion, which is \$\(\mathrm{SO_4^{2-}\)}\$.
To find the conjugate acid, add one proton (H\(\textsuperscript{+}\)) to the sulfate ion, increasing its hydrogen count by one and reducing its negative charge by one.
Write the formula of the conjugate acid by adding H\(\textsuperscript{+}\) to \$\(\mathrm{SO_4^{2-}\)}\$, resulting in \$\(\mathrm{HSO_4^-}\)\$.
Understand that \$\(\mathrm{HSO_4^-}\)\$ is called the bisulfate ion, which is the conjugate acid of the sulfate ion in the Brønsted–Lowry model.
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