Ch 2: Acids and Bases

Question 1

State the Bronsted-Lowry definitions of acids and bases.

Answer 1

acids are proton donors (and must contain a proton), and bases are proton acceptors (and must contain a lone pair of electrons or a pi bond)

Question 2

State the Lewis definition of acids and bases.

Answer 2

Acids are electron pair acceptors, and bases are electron pair donors.

Question 3

The loss of a proton from an acid forms its….

Answer 3

….conjugate base.

Question 4

The gain of a proton by a base forms its….

Answer 4

….conjugate acid.

Question 5

The basicity of a conjugate base A− decreases as the stability of its negative charge increases.

A more electronegative atom has a greater ability to stabilize negative charge.

Therefore… the compound with the negative charge on the most electronegative element will have lowest basicity, while the compound with the negative charge on the least electronegative element will have the highest basicity.

Answer 5

(From homework #2 problems)

Example attached.

Question 6

What is the pKa of water?

Answer 6

about 15.7

Question 7

What 4 factors affect the acidity of a given acid, HA?

Answer 7

1. ) element effects
2. ) inductive effects
3. ) resonance effects
4. ) hybridization effects

Question 8

The most important factor in determining the acidity of HA is…

Answer 8

….the location of A in the periodic table.