Topic 8/18: Acids and Bases Flashcards
1
Q
Define a Bronsted-Lowry acid.
A
Proton (H+) donor
2
Q
Define a Bronsted-Lowry base.
A
Proton (H+) acceptor
3
Q
Define acid-base conjugate pairs.
A
A conjugate pair is two species that differ by a single proton: The acid becomes the conjugate base while the base becomes the conjugate acid
4
Q
Define amphiprotic.
A
A chemical species capable of accepting and donating protons, thus able to act as a Bronsted-Lowry acid and base (e.g. H2O that donates to form OH- or accepts a proton to form H3O+)
5
Q
Define neutralization.
A
- A chemical reaction where a base and an acid react to form a salt and water
- Exothermic (releases heat)
6
Q
Outline neutralization reactions.
A
- Acid + Base ➜ Salt + Water
- Acid + Carbonate Base ➜ Salt + Water + CO2
- Acid + Metal ➜ Salt + H2
7
Q
Outline strong and weak acid.
A
Strong
- Completely dissociates in solution
- Forms strong electrolytes in water
- E.g. HCl, HNO3, H2SO4
Weak
- Partially dissociates in solution
- Forms weak electrolytes in water
- E.g. CH3COOH, H2CO3, H3PO4
8
Q
Outline strong and weak acid.
A
Strong
- Completely dissociates in solution
- Forms strong electrolytes in water
- E.g. HCl, HNO3, H2SO4
Weak
- Partially dissociates in solution
- Forms weak electrolytes in water
- E.g. CH3COOH, H2CO3, H3PO4
