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CHM012 > TOPIC 10- ACIDS AND BASES > Flashcards

TOPIC 10- ACIDS AND BASES Flashcards

1
Q

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

A

Acids

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2
Q

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

A

Bases

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3
Q

are proton (𝐻+) donors.

A

Acids

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4
Q

are proton (𝐻+) acceptors.

A

Bases

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5
Q

When 𝐻 receives a proton, it becomes

A

hydronium (H3O+)

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6
Q

If the acid is strong, use a

A

forward arrow

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7
Q

If the acid is weak, use a

A

double-headed arrow

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8
Q

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

A

conjugate base

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9
Q

is formed when the proton transfers to the base.

A

conjugate acid

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10
Q

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

A

conjugate acid-base pair

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11
Q

In strong acids, equilibrium lies far to the

A

right

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12
Q

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

A

dissociated (ionized)

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13
Q

Strong acids, yields a

A

weak conjugate base

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14
Q

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

A

Strong acids

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15
Q

What are the 7 strong acids?

A

● 𝐻𝐢𝑙 (hydrochloric acid)
● 𝐻𝐼 (hydroiodic acid)
● π»π΅π‘Ÿ (hydrobromic acid)
● 𝐻𝑁𝑂 (nitric acid) 3
● 𝐻𝐢𝑙𝑂 (chloric acid) 3
● 𝐻𝐢𝑙𝑂 (perchloric acid) 4
● 𝐻 (sulfuric acid)

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16
Q

In weak acids, equilibrium lies far to the

A

left

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17
Q

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

A

HA

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18
Q

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

A

Weak Acids

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19
Q

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

A

stronger acid

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20
Q

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

A

weaker acid

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21
Q

can act as either an acid or base

A

amphoteric substance

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22
Q

Example of amphoteric substance

A

water, 𝐻𝐢𝑂3- and
𝐻𝑃𝑂42-

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23
Q

The [H3O+] and [OH-] are

A

inversely proportional

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24
Q

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

A

acidic

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25
Q

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

A

basic

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26
Q

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

A

neutral

27
Q

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

A

p-scale

28
Q

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

A

pH

29
Q

As [H+] increases, the pH

A

decreases

30
Q

The lower the pH and pKa, the __________ the acid

A

stronger

31
Q

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

A

degree of ionization or percent ionization.

32
Q

is the fraction of the ionized acid molecules.

A

degree of ionization

33
Q

gives the percentage of ionized molecules.

A

percent ionization

34
Q

When you dilute a solution, the percent ionization

A

increases

35
Q

If the base is strong, use a

A

forward arrow

36
Q

If the base is weak, use a

A

double-headed arrow.

37
Q

completely dissociate when dissolved in an aqueous solution

A

strong bases

38
Q

strong bases include hydroxides of

A

Group 1A and 2A elements

39
Q

have larger 𝐾 values

A

strong bases

40
Q

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

A

Weak Bases

41
Q

have smaller 𝐾 values

A

Weak Bases

42
Q

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

A

equilibrium of acid-base reaction

43
Q

If equilibrium lies to the right, 𝐾a is

A

large (strong)

44
Q

If equilibrium lies to the left, 𝐾a is

A

small (weak)

45
Q

The equilibrium concentration of a strong acid/base is always

A

zero

46
Q

If 𝐾w increases as temperature increases, the process is

A

endothermic

47
Q

𝐾a and Kb are ____________________ to each other.

A

inversely proportional

48
Q

The sum of pH and pOH is always

A

14.00

49
Q

have a pH greater than 7.00.

A

Bases

50
Q

have a pH less than 7.00.

A

acids

51
Q

The lower the 𝑝𝐾 , the ___________ the acid

A

stronger

52
Q

The pH of pure water will always be______regardless of temperature.

A

7.00

53
Q

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

A

common ion effect

54
Q

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

A

common ion

55
Q

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

A

buffered solution

56
Q

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

A

blood

57
Q

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

A

buffered solution

58
Q

________ acids and bases cannot form buffer solutions.

A

Strong

59
Q

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

A

buffering capacity

60
Q

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

A

greater

61
Q

A buffer has the highest capacity when the component concentrations
are

A

equal

62
Q

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

A

1

63
Q

is the pH range over which the buffer acts effectively.

A

Buffer range

64
Q

Steps in Preparing Buffer Solutions

A
  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.

CHM012 (10 decks)

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