Write the formula for the conjugate acid of each base. a. NH₃ b. ClO₄^– c. HSO₄^– d. CO₃^2–

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Identify the base in the given problem, which is \( \text{HSO}_4^- \).

Recall that a conjugate acid is formed when a base gains a proton (\( \text{H}^+ \)).

Add a proton (\( \text{H}^+ \)) to the base \( \text{HSO}_4^- \).

Combine the added proton with the base to form \( \text{H}_2\text{SO}_4 \).

Verify that the charge is balanced: \( \text{HSO}_4^- + \text{H}^+ \rightarrow \text{H}_2\text{SO}_4 \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Conjugate Acid-Base Theory

According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. When a base accepts a proton (H+), it forms its conjugate acid. Understanding this relationship is crucial for identifying the conjugate acid of a given base.

HSO4 as a Base

HSO4, or hydrogen sulfate, can act as a base in acid-base reactions. When it accepts a proton, it transforms into its conjugate acid, H2SO4 (sulfuric acid). Recognizing the role of HSO4 in these reactions is essential for determining its conjugate acid.

Chemical Formulas and Proton Transfer

Chemical formulas represent the composition of substances, including the number of atoms and their types. In the context of acid-base reactions, understanding how to modify these formulas during proton transfer is key to identifying conjugate acids and bases accurately.

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