Use resonance forms of the conjugate bases to explain why methanesulfonic acid (CH₃SO₃H, pK_a = –2.6) is a much stronger acid than acetic acid (CH₃COOH, pK_a = 4.8).

Verified step by step guidance

1. Identify the conjugate bases of methanesulfonic acid (CH3SO3H) and acetic acid (CH3COOH). The conjugate base of methanesulfonic acid is the methanesulfonate ion (CH3SO3⁻), and the conjugate base of acetic acid is the acetate ion (CH3COO⁻).
2. Recall that the stability of the conjugate base is a key factor in determining the strength of an acid. A more stable conjugate base corresponds to a stronger acid because the equilibrium of the acid dissociation reaction shifts more toward the ionized form.
3. Analyze the resonance structures of the methanesulfonate ion (CH3SO3⁻). The negative charge on the oxygen atom is delocalized over three oxygen atoms through resonance, which significantly stabilizes the conjugate base. Write the resonance forms of CH3SO3⁻ using MathML: ${\mathrm{CH}3}_{(}$.
4. Compare this to the resonance structures of the acetate ion (CH3COO⁻). The negative charge on the oxygen atom is delocalized over only two oxygen atoms, which provides less stabilization compared to the methanesulfonate ion. Write the resonance forms of CH3COO⁻ using MathML: ${\mathrm{CH}3}_{(}$.
5. Conclude that the greater resonance stabilization of the methanesulfonate ion (CH3SO3⁻) compared to the acetate ion (CH3COO⁻) makes methanesulfonic acid (CH3SO3H) a much stronger acid than acetic acid (CH3COOH). This is reflected in their respective pKa values, where a lower pKa indicates a stronger acid.

Key Concepts

Resonance Structures

Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In the context of acids, resonance can stabilize the conjugate base by distributing negative charge over multiple atoms, making the acid stronger. For methanesulfonic acid, its conjugate base can be represented by several resonance forms, enhancing stability compared to the conjugate base of acetic acid.

Acid Strength and pKa

The strength of an acid is often measured by its pKa value, which indicates the tendency of the acid to donate a proton (H+). A lower pKa value signifies a stronger acid, as it more readily donates protons. Methanesulfonic acid has a pKa of -2.6, indicating it is a much stronger acid than acetic acid, which has a pKa of 4.8, reflecting its weaker tendency to lose a proton.

Conjugate Bases

The conjugate base of an acid is what remains after the acid donates a proton. The stability of the conjugate base is crucial in determining the strength of the corresponding acid. In this case, the conjugate base of methanesulfonic acid is more stable due to resonance stabilization, while the conjugate base of acetic acid is less stable, contributing to the significant difference in their acid strengths.