Acids and Bases

Question 1

Arrhenius definitions

Answer 1

Acids: Substances that release H+ ions.
Bases: Substances that release OH- ions.

Question 2

Bronsted - Lowry definitions + Examples

Answer 2

Acid: Proton / H+ donor
Base: Proton / H+ acceptor

• NH3 base in water and H20 acid!

Question 3

Lewis definitions + Examples

Answer 3

Acid: Lone (electron) pair acceptor.
Base: Lone (electron) pair donor.

• BF3 and NH3 can now be explained.

Question 4

Conjugate acid - base

Answer 4

Species that differ by a single proton.
- Base → Conjugate acid
- Acid → Conjugate base

Question 5

Amphoteric

Answer 5

Can act as either an acid or base.
- Al2O3

Question 6

Amphiprotic

Answer 6

A type of amphoteric substance that specifically can act as either an acid or base by accepting or donating hydrogen ions.
- water, diprotic acids

Question 7

Properties of Acids

Answer 7

1) Often produce H+ in water (also written as H30+, hydronium, which is a hydrogen ion attached to a water molecule)
2) Taste sour
3) Corrode metals
4) Electrolytes
5) pH is less than 7

Question 8

Key acid reactions

Answer 8

1. Acid + Base → Salt + Water
2. Acid + Metal → Salt + Hydrogen
3. Acid + Metal Carbonate → Salt + Water + Carbon dioxide

Question 9

Properties of Bases

Answer 9

1) Often produce OH- ions in water
2) Taste bitter
3) Feel soapy / slippery
4) pH greater than 7
5) Are electrolytes

Question 10

Alkali

Answer 10

A base than dissolves in water