What is the conjugate acid of each of the following? What is...

What is the conjugate acid of each of the following? What is the conjugate base of each? (a) $\mathrm{H}_{2} \mathrm{S}$ (b) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ (c) $\mathrm{PH}_{3}$ (d) $\mathrm{HS}$ (e) $\mathrm{HSO}_{3}^{-}$ (f) $\mathrm{H}_{3} \mathrm{O}_{2}^{+}$ (g) $\mathrm{H}_{4} \mathrm{N}_{2}$ (h) $\mathrm{CH}_{3} \mathrm{OH}$

What is the conjugate acid of each of the following? What is the conjugate base of each?
(a) $\mathrm{H}_{2} \mathrm{S}$
(b) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
(c) $\mathrm{PH}_{3}$
(d) $\mathrm{HS}$
(e) $\mathrm{HSO}_{3}^{-}$
(f) $\mathrm{H}_{3} \mathrm{O}_{2}^{+}$
(g) $\mathrm{H}_{4} \mathrm{N}_{2}$
(h) $\mathrm{CH}_{3} \mathrm{OH}$

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

Bronsted-Lowry Acid-Base Theory

This theory defines acids as proton donors and bases as proton acceptors. It is fundamental in understanding how acids and bases react, especially in reversible reactions where a proton is transferred between species, forming conjugate acid-base pairs.

Conjugate Acid

A conjugate acid is the species that results when a base accepts a proton. It is one half of a conjugate acid-base pair and its formation is critical in proton transfer reactions, reflecting the reversible nature of acid-base equilibria.

Conjugate Base

A conjugate base is the species that remains after an acid donates a proton. It represents the other half of a conjugate acid-base pair and is key to understanding the balance in acid-base reactions, as it can often accept a proton to reform the original acid.

Proton Transfer Reactions

These reactions involve the movement of a proton from one species to another. They play a central role in establishing the relationship between conjugate acids and bases, showing the dynamic equilibrium that exists in acid-base chemistry.

Transcript

Please give Ace some feedback