Acidity, Basicity, pKa

Question 1

Ionization Constant Equation

Answer 1

[H3O+][OH-] = 10^-14

Question 2

Ka = ?

Answer 2

Ka = ([H3O+][A-])/([AH])
Ka = (H3O+*conjugate base)/(acid)

Question 3

As acid strength increases, what happens to CB strength?

Answer 3

Decreases

Question 4

As base strength increases, what happens to CA strength?

Answer 4

Decreases

Question 5

As acid strength increases, what happens to CB stability?

Answer 5

Increases

Question 6

As EN increases, what happens to CB stability? Why?

Answer 6

Increases bc of neg charge on EN element

Question 7

What does the presence of weak A-H bonds do to acid strength?

Answer 7

Increases it

Question 8

How are delocalization and CB stability related?

Answer 8

Delocalization of neg charge of EN element increases CB stability

Question 9

Amine vs. Amide

Answer 9

Amine: Nitrogen w/ LP
Amide: N w/ carbonyl (C=O) and H/C

Question 10

What orbital increases acidity?

Answer 10

Acidity increases if e- are in an orbital w/ greater s-character [double-check]

Question 11

Conjugation

Answer 11

Delocalization; result: decrease in energy

Question 12

Nucleophile

Answer 12

Tendency to donate e-

Question 13

Electrophile

Answer 13

Need e-

Question 14

Nucleophilic Addition

Answer 14

Nucleophile makes a sigma bond w/ an electrophile

Question 15

Lewis vs. Bronsted Acids/Bases

Answer 15

Lewis:
- Acids accept e-
- Bases donate e-

Bronsted: BAAD
- Bases attract H+
- Acids donate H+

Question 16

The more stable the conjugate base….the more BLANK the acid it came from is.

Answer 16

acidic

Question 17

Which side of acid/base reactions are favored at equilibrium?

Answer 17

The side that is less reactive (weaker acid) is favored