Which of the following acids have relatively strong...

Which of the following acids have relatively strong conjugate bases?
a. $\mathrm{CH}_{3} \mathrm{COOH}\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)$
b. HF
c. $\mathrm{H}_{2} \mathrm{S}$
d. $\mathrm{HCl}$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Acid Strength

Acid strength refers to the tendency of an acid to donate a proton (H+). It is determined by the stability of the resulting conjugate base: the more stable the conjugate base, the stronger the acid. Factors such as bond strength, electronegativity, and resonance stabilization influence acid strength.

Conjugate Base Stability and Basicity

The conjugate base is what remains after an acid donates its proton, and its stability plays a key role in determining the strength of the acid. A less stable conjugate base will tend to be a strong base, while a very stable conjugate base corresponds to a weak base. This stability is affected by factors like the distribution of charge, inductive effects, and resonance.

Inverse Relationship Between Acid and Conjugate Base Strength

There is an inherent inverse relationship between the strength of an acid and the basicity of its conjugate base. A strong acid typically has a very weak conjugate base because the conjugate base is highly stabilized and does not readily re-accept a proton, whereas a weak acid has a stronger conjugate base, indicating less stabilization of the negative charge.

Transcript

Please give Ace some feedback