Amide ion, H2 N^-, is a much stronger base than hydroxide ion, HO^- . Which is the stronger aci

step 1 They tell us that amid is a much stronger base than hydroxide, and we want to determine what is

Amide ion, H2 N^-, is a much stronger base than hydroxide...

Amide ion, $\mathrm{H}_{2} \mathrm{~N}^{-},$ is a much stronger base than hydroxide ion, $\mathrm{HO}^{-} .$ Which is the stronger acid, $\mathrm{NH}_{3}$ or $\mathrm{H}_{2} \mathrm{O}$ ? Explain.

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Key Concepts

Basicity and Conjugate Stability

The basicity of a conjugate base reflects its ability to accept a proton. A highly basic conjugate base indicates that the corresponding acid is weak since the base is very reactive and less stable. Conversely, a less basic conjugate base suggests a stronger parent acid due to its relative stability upon deprotonation.

Proton Transfer Equilibrium

Proton transfer equilibrium involves a balance between the forward reaction (acid donating a proton) and the reverse reaction (base accepting a proton). This equilibrium is governed by the relative strengths of the acid and its conjugate base in the wider context of the solvent and reaction conditions.

Acid Strength

Acid strength refers to the tendency of a species to donate a proton (H?). It is typically quantified by the acid dissociation constant (Ka) or pKa value, where lower pKa values indicate stronger acids. The strength of an acid is directly linked to the stability of its conjugate base after proton donation.

Conjugate Acid-Base Pairs

A conjugate acid-base pair consists of two species that differ by one proton. The relationship between the strength of an acid and its conjugate base is inverse; a strong acid forms a weak conjugate base, while a weak acid forms a strong conjugate base.

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