Question

In an equilibrium reaction, the original acid has a lone pair of electrons after the reaction, so it will act as a/n (acid/base) in the reverse process.

H-A + :B ↔ _____ + _____
A) Acid
B) Base
C) Salt
D) Catalyst

Answer 1

In an equilibrium acid-base reaction, the original acid becomes a conjugate base once it donates a proton and thus would act as a base in the reverse reaction. The stability of the conjugate base affects the direction of the equilibrium and the strength of the acid.

Step-by-step explanation:

In an equilibrium reaction such as H-A + :B ↔ conjugate base + conjugate acid, the original acid H-A will act as a base in the reverse process after it donates a proton and is left with a lone pair of electrons. The correct reaction for H-A + :B ↔ _____ + _____ would be:

• Conjugate acid
• Conjugate base

Factors affecting the stability of the conjugate base, such as the number of lone pairs, influence its ability to re-accept a proton, impacting the overall acid-base equilibrium and determining the strength of the parent acid. In Brønsted-Lowry acid-base reactions, a stronger acid tends to form a weaker conjugate base, while a stronger base tends to form a weaker conjugate acid.