Brønsted-Lowry Theory & Polyprotic Acids - AB 1&3 Flashcards
What is the Arrhenius definition of acids and bases?
Acids ionize in solution to produce H⁺, while bases dissociate to release OH⁻.
Give an example of an Arrhenius acid and base.
HCl (acid) → H⁺ + Cl⁻, NaOH (base) → Na⁺ + OH⁻.
How does the Brønsted-Lowry theory define acids and bases?
Acids are proton donors (H⁺), and bases are proton acceptors.
Why do acids and bases always come in pairs?
When an acid donates a proton, a conjugate base forms; when a base accepts a proton, a conjugate acid forms.
What is a conjugate acid-base pair?
Two species that differ by only one proton (H⁺).
What is the relationship between acid strength and conjugate base strength?
The stronger the acid, the weaker its conjugate base, and vice versa.
What is a monoprotic acid? Give an example.
An acid that donates only one proton per molecule (e.g., HCl, HNO₃).
What is a diprotic acid? Give an example.
An acid that donates two protons per molecule (e.g., H₂SO₄, H₂CO₃).
What is a triprotic acid? Give an example.
An acid that donates three protons per molecule (e.g., H₃PO₄).
What are amphoteric substances?
Substances that can act as both an acid and a base depending on the reaction conditions.
Give an example of an amphoteric substance.
Water (H₂O) can donate a proton (acting as an acid) or accept a proton (acting as a base).
How do you determine if a hydrogen atom is acidic?
It must be attached to an electronegative atom, usually oxygen.
Why is only one hydrogen acidic in CH₃COOH, while both are acidic in H₂C₂O₄?
In CH₃COOH, only one H is bonded to oxygen, but in H₂C₂O₄, both H atoms are bonded to oxygen.
