Acids and Bases

Question 1

What is an Arrhenius base?

Answer 1

A compound that produces OH- and a cation in aqueous solution

Question 2

What is Arrhenius acid?

Answer 2

A compound that produces H+ when dissolved in water

Question 3

What is a Lewis acid?

Answer 3

A potential electron-pair acceptor

Question 4

What is a Lewis base?

Answer 4

A potential electron-pair donor

Question 5

What is a Bronsted-Lowry acid?

Answer 5

H+ donor

Question 6

What is a Bronsted-Lowry base?

Answer 6

H+ acceptor

Question 7

Which acid/base definition accounts for neutrality?

Answer 7

Arrhenius

Question 8

Are acids lone pair acceptors or donors?

Answer 8

Acceptor

Acids accept lone pairs, donate protons

Question 9

Strong acids __?__ dissociate in solution

Answer 9

Completely

Question 10

Weak acids __?__ dissociate in solution

Answer 10

Partially

Question 11

What is a neutralisation reaction?

Answer 11

Acid + Base = Salt + Water

Question 12

What is CH3COOH known as?

Answer 12

Acetic acid/Ethanoic acid

Question 13

What is H3O+ known as?

Answer 13

Hydroxonium ion

Question 14

H2O is amphiphilic. What does amphiphilic mean?

Answer 14

It can act as either an acid or a base

Question 15

How is acid strength quantified?

Answer 15

The acid dissociation constant, Ka

Question 16

What is the difference between Kc and Ka?

Answer 16

Kc accounts for all concentrations in the reaction. Ka ignores the H2O as it is a very large value and doesn’t change significantly in the reaction.

Question 17

True or false: To calculate Kc:

[product1]x[product2])/([reactant1]x[reactant2]

Answer 17

True.

To calculate Ka or Kb, you don’t include water

Question 18

How do you calculate pH?

Answer 18

pH= -log([H+])

Question 19

How do you calculate pOH?

Answer 19

pOH= -log([OH-])

Question 20

pH+pOH always add up to __?__

Answer 20

14

Question 21

What is the Henderson-Hasselbach equation?

Answer 21

pH = pKa + log([A-]/[HA])