Write the formula for the conjugate acid of each base. c. HCO3–

검증된 단계별 안내

Identify the base in the problem: \( \text{HCO}_3^- \).

Recall that a conjugate acid is formed by adding a proton (\( \text{H}^+ \)) to the base.

Add a proton to the base \( \text{HCO}_3^- \) to form the conjugate acid.

The addition of \( \text{H}^+ \) to \( \text{HCO}_3^- \) results in \( \text{H}_2\text{CO}_3 \).

Write the formula for the conjugate acid: \( \text{H}_2\text{CO}_3 \).

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주요 개념

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Conjugate Acid-Base Pair

In acid-base chemistry, a conjugate acid is formed when a base accepts a proton (H+). This relationship is part of the Brønsted-Lowry theory, which defines acids as proton donors and bases as proton acceptors. Each acid-base pair differs by one proton, illustrating the dynamic nature of proton transfer in chemical reactions.

Bicarbonate Ion (HCO3–)

The bicarbonate ion (HCO3–) is an important buffer in biological systems and plays a crucial role in maintaining pH balance. It can act as a base by accepting a proton to form carbonic acid (H2CO3), which is essential in processes like respiration and metabolic regulation. Understanding its behavior is key to identifying its conjugate acid.

Protonation

Protonation is the process by which a molecule gains a proton (H+), resulting in the formation of a conjugate acid. This process is fundamental in acid-base reactions, as it alters the charge and reactivity of the molecule. For the bicarbonate ion, protonation leads to the formation of carbonic acid, illustrating how bases can transform into acids through protonation.