Write the formula for the conjugate base of each acid. b. H₂SO₃

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Identify the acid given in the problem: \( \text{H}_2\text{SO}_3 \).

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

Remove one \( \text{H}^+ \) from \( \text{H}_2\text{SO}_3 \) to form the conjugate base.

After removing \( \text{H}^+ \), the remaining species is \( \text{HSO}_3^- \).

Thus, the formula for the conjugate base of \( \text{H}_2\text{SO}_3 \) is \( \text{HSO}_3^- \).

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Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate base is formed when an acid donates a proton (H+). The relationship between an acid and its conjugate base is fundamental to understanding acid-base reactions, as it illustrates how substances can interchange between donating and accepting protons.

Sulfurous Acid (H2SO3)

Sulfurous acid (H2SO3) is a weak diprotic acid that can donate two protons. When it loses one proton, it forms its conjugate base, bisulfite (HSO3-), and if it loses both protons, it forms sulfite (SO3^2-). Understanding the structure and behavior of sulfurous acid is essential for identifying its conjugate base.

Acid-Base Equilibrium

Acid-base equilibrium refers to the balance between acids and their conjugate bases in solution. This concept is crucial for predicting the direction of acid-base reactions and understanding the strength of acids and bases, which is determined by their ability to donate or accept protons in a chemical reaction.

Write the formula for the conjugate base of each acid. b. H2SO3