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High School > Chem 30 Unit 3 > Flashcards

Chem 30 Unit 3 Flashcards

1
Q

Equilibrium

A

a state of a closed system in which all measurable properties are constant

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2
Q

Dynamic equilibrium

A

a balance between forward and reverse processes occurring at the same rate

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3
Q

Ice tables

A

Initial, Changes, Equilibrium

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4
Q

in an ice table…

A

Products always start at zero
Reactants go down; products go up

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5
Q

<50% reaction =

A

reactants favoured, reverse reaction, k <1

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6
Q

> 50% reaction =

A

products favoured, forward reaction, k>1

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7
Q

> 99% reaction =

A

quantitative, complete reaction, k is a very large number

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8
Q

if there is no reaction

A

k = 0

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9
Q

when is a reaction quantitative (arrow)?

A

single arrow

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10
Q

what to not include in K value calculations?

A

a solid in a gas reaction or water (l) in an aqueous solution reaction)

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11
Q

Le Chatelier’s Principle

A

disturbed close systems will shift to restore equilibrium

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12
Q

Le Chatelier’s Principle says…

A

Conditions affecting equilibrium are temperature, pressure, and concentration

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13
Q

3 stages of Le Chatelier’s

A

Initial equilibrium state, Shifting non-equilibrium state, New equilibrium state

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14
Q

in concentration shifts…

A

k value remains constant

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15
Q

in temperature shifts…

A

k value changes

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16
Q

in an endothermic reaction…

A

when temp increases, k value increases, vice versa

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17
Q

in an exothermic reaction…

A

when temp increases, k value decreases, vice versa

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18
Q

pressure/volume shifts

A

k value remains constant. (pressure/volume shifts are only for gases)

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19
Q

Pressure increase/volume decrease:

A

shift towards the side with fewer moles of molecules

20
Q

Pressure decrease/volume increase:

A

shift towards the side with more moles of molecules

21
Q

when there is equal moles on each side and a volume/pressure shift…

A

no change occurs / no shift

22
Q

a catalyst…

A

Changes the rate of both forward and reverse reaction by the same amount, therefore it does not affect the position of the equilibrium.

23
Q

If inert gases are added to increase the total pressure of the system…

A

nothing will change. The equilibrium pressure will not change.

24
Q

pH/pOH sig digs

A

the numbers behind the decimal place are significant

25
Q

strong acid

A

an acid that completely dissociates/ionizes (100%) into its ions

26
Q

weak acid

A

an acid that slightly ionizes/dissociates into water

27
Q

dilute solution

A

solution w/low ratio of solute to solvent

28
Q

concentrated solution

A

a solution w/high ratio of solute to solvent

29
Q

SO2 and CO2 react with water to form

A

H2SO3 and H2CO3

30
Q

bronsted-lowry neutralization

A

results in a proton (hydrogen) transfer from the strongest acid to the strongest base.

31
Q

in bronsted-lowry, a hydrogen =

A

a proton

32
Q

conjugate acid base pairs

A

chemical species whose formulas differ only by one proton

33
Q

amphiprotic

A

substances that can act as both a Bronsted Lowry acid and base.

34
Q

if acid is above base…

A

it is products favoured

35
Q

if acid is below base…

A

it is reactants favoured

36
Q

polyprotic acids

A

acid species capable of donating more than one hydrogen during a reaction

37
Q

monoprotic acids

A

possess only one hydrogen

38
Q

polybasic species

A

base species capable of accepting more than one hydrogen during a reaction

39
Q

monobasic

A

capable of accepting only one hydrogen

40
Q

‘continuously added’ or ‘reacted until ___endpoints’

A

write more than one reaction (for polyprotic/basic)

41
Q

endpoint

A

pH. the point where there is a colour change

42
Q

equivalence point

A

volume. where endpoint occurs; measured quantity of titrant

43
Q

buffer zone

A

period on titration curve before big change in pH

44
Q

buffers

A

conjugate acid-base pair in a solution that resists sudden changes in pH when an acid or base is added

45
Q

buffers must…

A

Has to be a weak conjugate acid-base pair (e.g. H2CO3 and HCO3-)

46
Q

empirical

A

based on observations or experience

High School (18 decks)

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