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Chem 30 > Equilibrium - Acids and Bases > Flashcards

Equilibrium - Acids and Bases Flashcards

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1
Q

When does equilibrium occur?

A

when the rate of forwards reactions = the rate of reverse reactions

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2
Q

Microscopic properties

A

are continually changing

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3
Q

Macroscopic properties

A

are constant

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4
Q

balance between forward and reverse reactions that are occuring at the same rate so the observable properties are constant

A

Dynamic equilibrium

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5
Q

explains that reverse reaction can occur and the final state is a competition between the forward and reverse reactions

A

Collision theory

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6
Q

What are the requirements to stay at equilibrium?

A

temp stays constant, system remains closed

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7
Q

Homogenous expression

A

same state

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8
Q

Heterogeneous expression

A

different state

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9
Q

What states must always be included in equilibrium expression by law?

A

gases and aqueous solutions

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10
Q

What is the rule about having liquids in equilibrium expressions?

A

if there is only one liquid, it is not included. if there is more than one liquid then all are added

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11
Q

What is never included in an equilibrium expression?

A

solids

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12
Q

Would an increase of decrease in temp affect the value of a systems equilibrium constant?

A

yes

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13
Q

What is favored if k > 1?

A

Products

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14
Q

What is favored if k < 1?

A

Reactants

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15
Q

What does it mean when Kc = 1?

A

Reactants = products

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16
Q

T or F: a reaction starts with 100% products and 0% reactants

A

F, it always starts with 100% reactants and 0% products

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17
Q

when a system at equililbrium is disturbed by a change in property, the system adjusts in a way that opposes the change

A

Le Chatelier’s principle

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18
Q

What are stresses that shift equilibriums?

A

temp, concentration, pressure/volume

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19
Q

What happens during a shift right?

A

concen. of products increase and forward reaction is momentarily favored (reactants also decrease)

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20
Q

What happens during a shift left?

A

concen. of reactants increase and reverse reaction is momentarily favored (products also decrease)

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21
Q

What occurs if you increase products?

A

we shift to reactant side or left

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22
Q

What occurs if you decrease products?

A

we shift to the product side or right

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23
Q

What occurs if you increase reactants?

A

we shift to the product side or right

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24
Q

What occurs if you decrease reactants?

A

we shift to the reactants or left

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25
Q

Endothermic reaction and location where energy/heat would be

A

absorbing heat, energy in reactants

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26
Q

Exothermic reaction and location where energy/heat would be

A

releasing heat, energy in products

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27
Q

Is endothermic energy positive or negative?

A

positive

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28
Q

Is exothermic energy positive or negative?

A

negative

29
Q

What happens when you add heat in an endothermic reaction?

A

shift right

30
Q

What happens when you remove heat in an endothermic reaction?

A

shift left

31
Q

What happens when you add heat in an exothermic reaction?

A

shift left

32
Q

What happens when you remove heat in an exothermic reaction?

A

shift right

33
Q

According to Boyle’s Law, what happens to volume as pressure goes up and vice versa?

A

volume decreases, and when pressure decreases volume increases

34
Q

Where will the system shift if you increase volume? (decreasing pressure)

A

the side with most amount of moles

35
Q

Where will the system shift if you decrease volume? (increasing pressure)

A

the side with least amount of moles

36
Q

How would no shift occur even if pressure/volume changed?

A

if there are equal moles on each side of expression

37
Q

What shift does the addition of a catalyst or inert gas cause?

A

no shift

38
Q

How would you be able to identify a heat stress on a graph?

A

all gradual changes

39
Q

How would you be able to identify a pressure/volume stress on a graph?

A

all sudden changes

40
Q

How would you be able to identify a concentration stress on a graph?

A

only one sudden change

41
Q

a proton donor

A

acids

42
Q

a proton acceptor

A

bases

43
Q

a pair of substances that differ by only one proton

A

Conjugate acid-base pair

44
Q

a substance that can act as either an acid or a base in different situations

A

Amphiprotic species

45
Q

Is water amphiprotic?

A

yes

46
Q

When is modified Arrhenius theory used?

A

when an acid or base is by itself

47
Q

When is Bronsted-Lowry used?

A

when an acid-base reaction occurs

48
Q

What is favored when the acid is above the base?

A

products

49
Q

What is favored when the base is above the acid?

A

reactants

50
Q

What are the species of HCl?

A

H3O+ and Cl- (NOT H+!)

51
Q

What is the value of Kw?

A

1.0 x 10^-14

52
Q

What is the shortcut equation to find pH?

A

pH= -log√(Ka)(Ci)

53
Q

What is the shortcut equation to find pOH?

A

pOH= 14-(-log√(Ka)(Ci))

54
Q

What will always be the greatest concentration in any solution?

A

H2O

55
Q

Monoprotic acid

A

can donate only 1 proton to base

56
Q

Polyprotic acid

A

can donate more than 1 proton to base

57
Q

Diprotic acid

A

can donate 2 protons to base

58
Q

Triprotic acid

A

can donate 3 protons to base

59
Q

Monoprotic base

A

can only accept 1 proton

60
Q

Polyprotic base

A

can accept more than 1 proton

61
Q

Diprotic base

A

can accept 2 protons from acid

62
Q

Triprotic base

A

can accept 3 protons from acid

63
Q

complex weak acid or base compound that changes color depending on the H3O+

A

Indicators

64
Q

What type of reactions are the only ones that produce detectable equivalence points in an acid-base titration?

A

Quantitative (full arrow)

65
Q

a solution that resists a change in pH when small amounts of acid or base are added to it

A

Buffer solution

66
Q

What is a buffer composed of?

A

weak acid and its conjugate base

67
Q

the limit of the ability of a buffer to maintain pH level

A

Buffering capacity

68
Q

Can strong acid bases be a buffer?

A

no

69
Q

any form of precipitation with acidic components that fall to the ground in wet or dry forms

A

Acid deposition

Chem 30 (3 decks)

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