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Chem 152 > Quiz 2 > Flashcards

Quiz 2 Flashcards

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1
Q

What is an acid (Arrhenius theory)?

A

a substance containing H+ and whose aqueous solution contains more H+ ions than OH- ions. Disolves “HA” in water

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2
Q

Acid equation (Arrhenius theory)

A

HA (aq) = H+ (aq) + A- (aq)

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3
Q

What is a base? (Arrhenius theory)

A

a substance containing OH- and whose aqueous solution contains more OH- ions than H+ ions. Dissolves “BOH” in water

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4
Q

Base equation (Arrhenius theory)

A

BOH (aq) = B+ (aq) + OH- (aq)

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5
Q

Neutralization (Arrhenius theory)

A

Produces water and an aqueous salt

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6
Q

Acid (Bronsted-Lowry Theory)

A

Proton-donor (H+ ion donor)

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7
Q

Base (Bronsted-Lowry Theory)

A

Proton-acceptor (H+ ion acceptor)

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8
Q

When does water act as a base?

A

When an acid gives its proton to water

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9
Q

Acid (Lewis Acids)

A

Electron pair acceptor

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10
Q

Base (Lewis Acids)

A

Electron pair donator

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11
Q

What is the driving force in all three acid/base schemes?

A

The formation of covalent bonds

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12
Q

What happens when we put an acid in water?

A

Acid donates a proton to water

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13
Q

What happens when we put a base in water?

A

The base grabs a proton from water

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14
Q

Conjugate acid

A

Formed when a proton is transferred to the base

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15
Q

Conjugate base

A

Everything that remains of the acid molecule after a proton is lost

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16
Q

Conjugate acid-base pair

A

Consists of two substances related to each other by donating and accepting a single proton

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17
Q

Are small K values weak or strong acids?

A

Weak

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18
Q

Are large K values weak or strong acids?

A

Strong

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19
Q

What is the magnitude of Ka?

A

A measure of how likely the acid is to dissociate in water

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20
Q

Do strong acids dissociate completely in water?

A

Yes

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21
Q

Do weak acids dissociate in water?

A

No

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22
Q

What approaches 0 in a dilute solution of a strong acid?

A

[HA]

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23
Q

What approaches 0 in a dilute solution of a weak acid?

A

[H3O+]

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24
Q

Stronger the acid, the higher the _______ at equilibrium

A

[H3O+]

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25
Q

The weaker an acid, the stronger its _____________

A

Conjugate base

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26
Q

Strong acids

A

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

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27
Q

Are large Kb values strong or weak bases?

A

Strong

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28
Q

Are small Kb values strong or weak bases?

A

Weak

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29
Q

Do strong or weak bases completely dissociate in water?

A

Strong bases

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30
Q

Strong bases

A

M2O or MOH (M= group 1A metals) and MO or M(OH)2 (M=group 2A metals)

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31
Q

What are most weak bases similar to?

A

NH3

32
Q

Amphoteric

A

Can be an acid or base (water)

33
Q

What is Kw and what does it equal?

A

The equilibrium constant for the autoionization of water and equals
1.0 x 10^ -14

34
Q

Equation for Kw

A

Ka x Kb = Kw (conjugate acid/base pair)

35
Q

pH of [H3O+] in pure water

A

1 x 10^ -4

36
Q

Equation for pH

A

pH = -log[H3O+]

37
Q

Equation for [H3O+]

A

[H3O+] = 10^ -pH

38
Q

Find pH directly (acid)

A

[H3O+] = [HA]o

39
Q

Find pH directly (base)

A

[OH-] = [XOH]o

40
Q

Equation for power of hydroxide

A

pOH = -log[OH-]

41
Q

Power of hydroxide in aqueous solution at 25 degrees C

A

pH + pOH = 14.00

42
Q

In a dilute solution of a weak acid ______

A

[HA]initial = [HA]eq

43
Q

Which compound will be the dominant producer of H+ in a solution?

A

The compound that has the greatest Ka value

44
Q

Is an ionic compound (salt) dissolved in water neutral, acidic, or basic?

A

Neutral

45
Q

What do salts consist of?

A

Cations of strong bases and the anions of strong acids

46
Q

Do salts have an effect on pH when dissolved in water?

A

No

47
Q

A salt whose cation alone has neutral properties and anion is the conjugate base of a weak acid produces a ________

A

Basic solution in water

48
Q

A salt whose anion alone has neutral properties and cation is the conjugate acid of a weak base or a small, highly charged metal will produce _________

A

Acidic solution in water

49
Q

Metals

A

Small, highly charged cations produce acidic solution in water

50
Q

What do you pair metals with?

A

H2O

51
Q

Equivalence Point

A

Point at which the amounts of titrant and sample are stoichiometrically equal.

52
Q

Stoichiometry titration

A

Add a strong base to a weak acid and determine extent of neutralization

53
Q

Equilibrium titration

A

Concentration of all species are determined and equilibrium expression evaluated

54
Q

Common ion effect

A

A shift in the equilibrium position that occurs because of the addition of an ion already involved in the equilibrium rxn

55
Q

Buffer

A

Solution of a weak acid and its conjugate base or weak base and conjugate acid

56
Q

What do buffers prevent?

A

Large changes in pH when strong acid or base is added

57
Q

Buffer capacity

A

Amount of strong acid or base a buffer can absorb without a significant change in pH

58
Q

What determines a greater buffer capacity?

A

Solution with larger concentrations of acid

59
Q

Ratio of the pH of a buffered solution

A

[A-]/[HA]

60
Q

Higher concentration of buffer components=

A

Larger buffering capacity

61
Q

Titration curve

A

A plot of pH as a function of NaOH

62
Q

What is the pH at equivalence for titrations between strong acids and bases?

A

7

63
Q

What’s present at equivalence (strong acid/base)?

A

Water and spectator ions

64
Q

What are the 4 parts of a titration curve?

A

Initial, midpoint, equivalence, and after equivalence

65
Q

Saturated solution

A

Max amount of dissolved solute

66
Q

Ksp

A

Solubility product constant - equilibrium constant of a dissolution process

67
Q

Molar solubility

A

x value in ICE table

68
Q

Large Ksp

A

Mostly products

69
Q

Small Ksp

A

Mostly reactant

70
Q

Do strong acid anions react with H3O+?

A

No

71
Q

Do weak acid anions react with H3O+?

A

Yes

72
Q

Qsp=Ksp

A

Solution is saturated and at equilibrium

73
Q

Qsp>Ksp

A

Precipitate will form until solution becomes saturated (to the right)

74
Q

Qsp<Ksp

A

Solution is unsaturated and no precipitate will form (to the left)

75
Q

Ka to pKa

A

-log(Ka) = pKa

76
Q

Henderson Hasselbalch Equation

A

pH = pKa + log([base]/[acid])

77
Q

pKa to Ka

A

Ka = 10^-pKa

Chem 152 (4 decks)

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