Acid and Base Properties

Question 1

What is a bronsted acid and bronsted base?

Answer 1

BS Acid : Proton donator

BS Base: Proton acceptor

Question 2

What is K_a and what does it tell us?

Answer 2

• dissociation constant, and describes whether products or reactants are favoured

Question 3

Give equations of Ka

Answer 3

Question 4

What do acids with pKa lower than -1.7 cause?

Answer 4

protonation of H2O completely

Question 5

What do bases with conjugate acid with a pKa higher than 15.7 cause?

Answer 5

deprotonation of H2O

Question 6

What is the strongest acid?

Answer 6

H3O+

Question 7

What is the strongest base?

Answer 7

OH-

Question 8

What are standard pKa ranges of compounds?

Answer 8

-10 to 50

Question 9

What is the pKa of H2O

Answer 9

pKa = 15.74

Question 10

What is the pKa of H3O

Answer 10

pKa = -1.74

Question 11

How is the strength of an acid determined?

Answer 11

electronic properties and properties &stabilty of conjugate base

Question 12

How is acidity increased

Answer 12

Electron withdrawing groups

Question 13

How does Inductive Effect affect acidity?

Answer 13

• -I Effect causes increase in acidity
• • I effect increases basisty

Question 14

How do double and triple bonds influence acid base properties?

Answer 14

• the higher the p (orbital) character, the higher pKa (the more basic)
• triple bonds (sp hybridized) have more s character, therefore hold onto electrons more tightly
  
  • proton is less easily donated
• single bonds are longer, donates proton more easily = more acidic

Question 15

What is a Lewis acid/base?

Answer 15

Lewis acid: electron pair acceptor

Lewis base: electron pair donator