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CHM 142 +145 > CHM 142 Exam 2 > Flashcards

CHM 142 Exam 2 Flashcards

1
Q

Are pure solids and pure liquids written into Keq equations?

A

No, they have a value of 1 because their activity is 1

they have constant concentration

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2
Q

Reactant Quotient

A

similar to Keq but concentrations used can be from any point in the reaction

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3
Q

Q»K

A

reaction proceeds left, forming more reactants

right to left

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4
Q

Q«K

A

reaction proceeds right, forming more products

left to right

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5
Q

Q= K

A

reaction must be at equilibrium

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6
Q

Which way does the reaction proceed if the volume is decreased and pressure is increased?

A

the reaction will shift in the direction of less moles

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7
Q

which way does the reaction proceed if the pressure is decreased and the volume is increased?

A

The reaction will shift to the side that produces more moles

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8
Q

For an exothermic reaction (H is -) that has heat taken from the system, which way does it proceed?

A

exothermic = reactants— products + heat so the reaction moves right

increases K

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9
Q

For an endothermic reaction (H +) that has heat added to the system, which way does it proceed?

A

endothermic = reactants + heat—products so the reaction shifts to the right

Increases K

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10
Q

How does a catalyst affect equilibrium?

A

it does not affect Keq but it does get the reaction to meet eq faster than without it

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11
Q

Arrhenius Acid

A

Increases the concentration of H+ ions

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12
Q

Arrhenius Base

A

Increases the concentration of OH- ions

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13
Q

Bronsted-Lowry acid

A

proton donor

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14
Q

Bronsted Lowry base

A

proton acceptor

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15
Q

a substance that can be both an acid and a base with the right electron configuration and # of H+ ions

A

Amphiprotic

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16
Q

Conjugate base

A

-1 H+ from an acid

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17
Q

Conjugate acid

A

+1 H from a base

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18
Q

the stronger the acid the —- its conjugate base

A

weaker

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19
Q

the stronger the base the—its conjugate acid

A

weaker

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20
Q

In acid-base rxns what will eq favor?

A

the transfer of the proton from the stronger acid to the stronger base to form a weaker acid and weaker base

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21
Q

when water donates protons to other water molecules

A

Autoionization

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22
Q

Kw, Ion product constant

A

the eq constant for ionization of water

1.*10^-14

23
Q

what kind of solution is it when [H+]>[OH-]

A

acidic

24
Q

what kind of solution is it when [H+]<[OH-]

A

basic

25
Q

pH=

A

-log[H+]

26
Q

pOH=

A

-log[OH-]

27
Q

14.00=

A

pH+pOH

28
Q

true or false? everytime you move up a unit on the pH scale the [H+] increases *10

A

false, everytime you move down a unit on the pH the concentration increases *10

29
Q

a strong electrolyte that completely dissociates into H+ ions

A

strong acid

30
Q

a strong electrolyte that completely dissociates into OH- ions

A

strong base

31
Q

for strong monoprotic acids [H+]=

A

[base]

32
Q

for diprotic strong bases [OH]

A

= 2*[base]

33
Q

weak electrolytes that only partially dissociate into H+

A

weak acids

34
Q

what do weak acids do that strong acids dont?

A

they establish equilibrium

35
Q

the — the values of Ka the — the acid

A

larger, stronger

36
Q

[H+]=

strong acid

A

[acid]

37
Q

[H+]<

weak acid

A

[acid] initial

38
Q

percent ionization for HA

A

[H+]eq/[HA]eq *100

39
Q

ionization equation for weak acids

A

HA (aq)—[H3O+]+[A-]

40
Q

weak bases

A

partially dissociate into OH- ions + a conjugate acid in water

41
Q

Kb=

A

[CA+][OH-]/[B]

42
Q

What are the two types of weak bases?

A
  1. neutral substances that have a nb pair of electrons to accept the proton (typically have a N atom)
  2. anions that are conjugate bases of a weak acid
43
Q

[Ka]*[Kb]=

A

1.0*10^-14

44
Q

pKa+pKb=

A

14.00

45
Q

Cations can be — and —-

A

acidic and neutral

46
Q

Anions can be —,— and —

A

acidic, basic, and neutral

47
Q

are anions from a strong acid neutral, basic or acidic

A

neutral

48
Q

are anions from a weak acids basic, acidic or neutral

A

basic

49
Q

are anions from a polyprotic acid bases, acids or neutral

A

they can be both

compare Ka and Kb

50
Q

are cations from strong bases acidic or neutral

grp I and grp II cations

A

neutral

51
Q

are conjugate acids from weak bases acidic or neutral

A

acidic

52
Q

are transition and post transition metal cations acidic or neutral

A

acidic

53
Q

neutral ion + basic ion=

A

basic solution

54
Q

basic ion+ acidic ion=

A

compare Ka and Kb values

the larger values determines pH level

CHM 142 +145 (6 decks)

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