Write the formula for the conjugate acid for each of the following bases:
a. CO₃^2-

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Identify the base given in the problem. In this case, the base is the carbonate ion, CO₃²⁻.

Recall the definition of a conjugate acid: it is formed when a base accepts a proton (H⁺).

Add one proton (H⁺) to the base, CO₃²⁻. This involves increasing the hydrogen count by 1 and reducing the charge by 1, as the proton carries a positive charge.

Write the resulting formula after adding the proton. The formula becomes HCO₃⁻, which is the conjugate acid of CO₃²⁻.

Verify the result by checking that the conjugate acid has one more hydrogen atom and a charge that is one unit less positive than the original base.

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Conjugate Acid-Base Theory

Conjugate acid-base theory, rooted in the Brønsted-Lowry definition, describes acids as proton donors and bases as proton acceptors. When a base accepts a proton (H⁺), it forms its conjugate acid. Understanding this relationship is crucial for predicting the behavior of chemical species in acid-base reactions.

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Acid and Base Strength Concept 3

Carbonate Ion (CO₃²⁻)

The carbonate ion (CO₃²⁻) is a polyatomic ion consisting of one carbon atom covalently bonded to three oxygen atoms, carrying a -2 charge. It acts as a base in chemical reactions, capable of accepting protons to form its conjugate acid. Recognizing its structure and charge is essential for determining its conjugate acid.

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Polyatomic Ions

Formation of Conjugate Acids

The formation of a conjugate acid involves the addition of a proton to a base. For the carbonate ion (CO₃²⁻), when it accepts a proton, it transforms into bicarbonate (HCO₃⁻), which is its conjugate acid. This process illustrates the dynamic nature of acid-base chemistry and the importance of understanding proton transfer.

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