Chapter 10 Acids and Bases

Question 1

What is an Arrhenius acid?

Answer 1

Dissociate to form an excess of H+ in solution

Question 2

What is an Arrhenius base?

Answer 2

Dissociate to form an excess of OH− in solution

Question 3

What is a Bronsted-Lowry acid?

Answer 3

species that donates hydrogen ions (H+)

Question 4

What is Bronsted-Lowry base?

Answer 4

species that accepts hydrogen ions (H+),

Question 5

What is a Lewis acid?

Answer 5

electron pair acceptor

Question 6

What is a Lewis base?

Answer 6

electron pair donor

Question 7

What is an amphoteric species?

Answer 7

Reacts like an acid in a basic
environment and like a base in an acidic environment.

Question 8

What is an amphiprotic species?

Answer 8

Amphoteric species that specifically can behave as a Brønsted–Lowry acid or Brønsted–Lowry base.

Question 9

What is the water dissociation constant?

Answer 9

Kw, is 10^−14 at 298 K. Like other equilibrium constants, only affected by changes in temperature

*pH = 7 = neutral is only valid at 25 C

Question 10

What is pH + pOH?

Answer 10

14 at 298 K

Question 11

What happens to strong acid and bases in solution?

Answer 11

Completely dissociate

Question 12

What signifies weak acids and bases not dissociating completely?

Answer 12

dissociation constants (Ka and Kb)

Question 13

How are the conjugates produced from strong acids/bases and weak acids/bases?

Answer 13

All the conjugates are weak

Question 14

What is the scale for conjugates?

Answer 14

The stronger the acid/base the weaker its conjugate

Question 15

What do neutralization rxns form?

Answer 15

salts and (sometimes) water

Question 16

What is an equivalent?

Answer 16

one mole of the species of interest

Question 17

What is the titrant?

Answer 17

Has a known concentration and is added slowly to the titrand to reach the equivalence point.

Question 18

What is the titrand?

Answer 18

titrant added to it.
has an unknown concentration but a known volume.

Question 19

What is the half-equivalence point?

Answer 19

the midpoint of the buffering region, in which half of the titrant has been protonated (or deprotonated); thus, [HA] = [A−] and a buffer is formed.

Question 20

What is the equivalence point?

Answer 20

Indicated by the steepest slope in a titration curve.

When acid and base are equal

Question 21

What is the equivalence point for strong acid and strong base?

Answer 21

pH =7

Question 21

What is the equivalence point for weak acid and strong base?

Answer 21

pH >7

Question 21

What is the equivalence point for strong acid and weak base?

Answer 21

pH < 7

Question 22

What is the equivalence point for weak acid and weak base?

Answer 22

can have equivalence points above or below 7

Question 23

What is the endpoint of titration?

Answer 23

when the indicator reaches its final color

*indicator is always a weaker acid or base

Question 24

What are found in polyvalent acid and base titrations?

Answer 24

Multiple buffering regions and equivalence points

Question 25

What do buffer solutions consist of?

Answer 25

a mixture of a weak acid and its conjugate salt or a weak base and its conjugate salt

*optimally buffered means
pH = pKa and pOH = pKb

Question 26

What is the product of a rxn between strong acid and a weak base?

Answer 26

salt, but no water is formed