TOPIC 10- ACIDS AND BASES

Question 1

increase hydrogen (𝐻+ ) concentrations in an aqueous solution.

Answer 1

Acids

Question 2

increases hydroxide (𝑂𝐻-) concentrations in an aqueous solution.

Answer 2

Bases

Question 3

are proton (𝐻+) donors.

Answer 3

Acids

Question 4

are proton (𝐻+) acceptors.

Answer 4

Bases

Question 5

When 𝐻 receives a proton, it becomes

Answer 5

hydronium (H3O+)

Question 6

If the acid is strong, use a

Answer 6

forward arrow

Question 7

If the acid is weak, use a

Answer 7

double-headed arrow

Question 8

is everything that remains of the acid molecule
after a proton is lost.

Answer 8

conjugate base

Question 9

is formed when the proton transfers to the base.

Answer 9

conjugate acid

Question 10

consists of two substances related to
each other by the donating and accepting of a single proton.

Answer 10

conjugate acid-base pair

Question 11

In strong acids, equilibrium lies far to the

Answer 11

right

Question 12

In strong acids, almost all the original HA is ____________________ at equilibrium

Answer 12

dissociated (ionized)

Question 13

Strong acids, yields a

Answer 13

weak conjugate base

Question 14

an acid whose conjugate base is a much weaker base than water

Answer 14

Strong acids

Question 15

What are the 7 strong acids?

Answer 15

● 𝐻𝐶𝑙 (hydrochloric acid)
● 𝐻𝐼 (hydroiodic acid)
● 𝐻𝐵𝑟 (hydrobromic acid)
● 𝐻𝑁𝑂 (nitric acid) 3
● 𝐻𝐶𝑙𝑂 (chloric acid) 3
● 𝐻𝐶𝑙𝑂 (perchloric acid) 4
● 𝐻 (sulfuric acid)

Question 16

In weak acids, equilibrium lies far to the

Answer 16

left

Question 17

In weak acids, most of the acid placed is still present as __ at equilibrium

Answer 17

HA

Question 18

has a conjugate base that is a much stronger base than water

Answer 18

Weak Acids

Question 19

has a higher (𝐻3O+) and a larger Ka value.

Answer 19

stronger acid

Question 20

has a lower (𝐻3O+) and a smaller Ka value.

Answer 20

weaker acid

Question 21

can act as either an acid or base

Answer 21

amphoteric substance

Question 22

Example of amphoteric substance

Answer 22

water, 𝐻𝐶𝑂3- and
𝐻𝑃𝑂42-

Question 23

The [H3O+] and [OH-] are

Answer 23

inversely proportional

Question 24

If [H3O+] > [OH-], the solution is

Answer 24

acidic

Question 25

If [H3O+] < [OH-], the solution is

Answer 25

basic

Question 26

If [H3O+] = [OH-], the solution is

Answer 26

neutral

Question 27

is the negative of the base-10 logarithm of a number.

Answer 27

p-scale

Question 28

is the negative logarithm of [H3O+] or [OH-]

Answer 28

pH

Question 29

As [H+] increases, the pH

Answer 29

decreases

Question 30

The lower the pH and pKa, the __________ the acid

Answer 30

stronger

Question 31

The extent of ionization of a weak acid can be described in terms of the

Answer 31

degree of ionization or percent ionization.

Question 32

is the fraction of the ionized acid molecules.

Answer 32

degree of ionization

Question 33

gives the percentage of ionized molecules.

Answer 33

percent ionization

Question 34

When you dilute a solution, the percent ionization

Answer 34

increases

Question 35

If the base is strong, use a

Answer 35

forward arrow

Question 36

If the base is weak, use a

Answer 36

double-headed arrow.

Question 37

completely dissociate when dissolved in an aqueous solution

Answer 37

strong bases

Question 38

strong bases include hydroxides of

Answer 38

Group 1A and 2A elements

Question 39

have larger 𝐾 values

Answer 39

strong bases

Question 40

partially dissociate when dissolved in an aqueous solution and exists in a solution as mixture of itself and its conjugate acid

Answer 40

Weak Bases

Question 41

have smaller 𝐾 values

Answer 41

Weak Bases

Question 42

will lie to where the weaker acids and bases are found.

Answer 42

equilibrium of acid-base reaction

Question 43

If equilibrium lies to the right, 𝐾a is

Answer 43

large (strong)

Question 44

If equilibrium lies to the left, 𝐾a is

Answer 44

small (weak)

Question 45

The equilibrium concentration of a strong acid/base is always

Answer 45

zero

Question 46

If 𝐾w increases as temperature increases, the process is

Answer 46

endothermic

Question 47

𝐾a and Kb are ____________________ to each other.

Answer 47

inversely proportional

Question 48

The sum of pH and pOH is always

Answer 48

14.00

Question 49

have a pH greater than 7.00.

Answer 49

Bases

Question 50

have a pH less than 7.00.

Answer 50

acids

Question 51

The lower the 𝑝𝐾 , the ___________ the acid

Answer 51

stronger

Question 52

The pH of pure water will always be______regardless of temperature.

Answer 52

7.00

Question 53

is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.

Answer 53

common ion effect

Question 54

The presence of a ______________ suppresses the ionization of a weak acid or a weak base.

Answer 54

common ion

Question 55

is one that resists a change in its pH when either hydroxide ions or protons are added.

Answer 55

buffered solution

Question 56

most important practical example of a buffered solution is our _______, absorbing acids/bases in biological reactions without changing its pH.

Answer 56

blood

Question 57

is a combination of a weak acid/base and a salt of that weak acid/base.

Answer 57

buffered solution

Question 58

________ acids and bases cannot form buffer solutions.

Answer 58

Strong

Question 59

of a buffered solution represents the amount of protons or hydroxide ions the buffer can absorb without a significant change in pH.

Answer 59

buffering capacity

Question 60

The more concentrated the components of a buffer, the _______ the buffer capacity.

Answer 60

greater

Question 61

A buffer has the highest capacity when the component concentrations are

Answer 61

equal

Question 62

The most efficient buffering occurs when the [A]/[HA] ratio is close to

Answer 62

1

Question 63

is the pH range over which the buffer acts effectively.

Answer 63

Buffer range

Question 64

Steps in Preparing Buffer Solutions

Answer 64

1. Choose the conjugate acid-base pair. 2. Calculate the ratio of buffer component concentrations. 3. Determine the buffer concentration. 4. Mix the solution and adjust the pH.