Explique las observaciones siguientes: (a) el HCl es un ácido más fuerte que el H2 S; (b) el H3

step 1 Problem 90, Part A. For binary hydride, acid strength increases going across a row. So HCL is a

Explique las observaciones siguientes: (a) el HCl es un...

Explique las observaciones siguientes: (a) el $\mathrm{HCl}$ es un ácido más fuerte que el $\mathrm{H}_2 \mathrm{~S}$; (b) el $\mathrm{H}_3 \mathrm{PO}_4$ es un ácido más fuerte que el $\mathrm{H}_3 \mathrm{AsO}_4$; (c) el $\mathrm{HBrO}_3$ es un ácido más fuerte que el $\mathrm{HBrO}_2$; (d) el $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$ es un ácido más fuerte que el $\mathrm{HC}_2 \mathrm{O}_4{ }^{-}$; (e) el ácido benzóico $\left(\mathrm{C}_6 \mathrm{H}_5 \mathrm{COOH}\right)$ es un ácido más fuerte que el fenol $\left(\mathrm{C}_6 \mathrm{H}_5 \mathrm{OH}\right)$.

Key Concepts

Electronegativity and Bond Polarity

This concept addresses how the electronegativity of the atom bonded to hydrogen affects the acid’s strength. A more electronegative atom pulls electron density from the hydrogen more effectively, leading to a weaker H–X bond and a more stable anion after deprotonation, both of which enhance acid strength.

Conjugate Base Stability

The strength of an acid is largely determined by the stability of its conjugate base. A conjugate base that can effectively stabilize the negative charge—whether through factors such as high electronegativity, solvation, or distribution of charge—is associated with a stronger acid.

Inductive Effects in Oxyacids

In oxyacids, the presence of additional oxygen atoms increases acidity via an inductive electron-withdrawing effect. These oxygen atoms pull electron density away from the acidic proton and help delocalize the negative charge on the conjugate base, thereby stabilizing it and resulting in a stronger acid.

Resonance Stabilization

Resonance stabilization refers to the delocalization of the negative charge over multiple atoms in the conjugate base. When a conjugate base can spread out the charge through resonance, as seen in many organic and aromatic acids, it becomes more stable, which in turn increases the strength of the corresponding acid.

Polyprotic Acidity and Charge Effects

In polyprotic acids, each successive deprotonation step creates an anion with an additional negative charge. The increased negative charge can lead to greater charge repulsion and less effective stabilization, often making the loss of the next proton less favorable compared to the initial deprotonation.

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