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Sophomore- Spring 2024- Mac > Test 2- Chem 112- St. Thomas- Summer > Flashcards

Test 2- Chem 112- St. Thomas- Summer Flashcards

1
Q

True or false, The conjugate base of a strong acid has negligible acid-base properties.

A

true

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2
Q

the bigger Ka/Kb is, the ____ the acid/base is

A

stronger

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3
Q

hydronium

A

H3O+

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4
Q

hydroxide

A

OH-

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5
Q

higher pH means ____ concentration of H30

A

lower

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6
Q

lower pH means ____ concentration of H30

A

higher

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7
Q

Q

A

the reaction quotient at any time during reaction

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8
Q

K

A

equilibrium constant. Q, ONLY at equilibrium (the END of reaction)

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9
Q

Kc>1

A

favors products

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10
Q

Kc=1

A

they are the same

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11
Q

Kc<1

A

favors reactants

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12
Q

Q<K

A

reaction moves right (forward) to form products

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13
Q

Q=K

A

equilibrium

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14
Q

Q>K

A

reaction moves left (reverse) + forms reactants

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15
Q

Le Chatelier’s principle

A

a system in equilibrium will adjust to a stress by shifting to minimize or alleviate stress types

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16
Q

addition of products or reactants does what

A

shift in the opposite side

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17
Q

removal of products or reactants does what

A

shift in the same side

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18
Q

increasing temp does what

A

moves toward opposite side

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19
Q

decreasing temp does what

A

shifts toward the same side (energy side)

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20
Q

input energy (endothermic)

A

energy side is reactant

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21
Q

output energy (exothermic)

A

energy side is product

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22
Q

decrease in volume does what to pressure

A

increase

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23
Q

increase in volume does what to pressure

A

decrease

24
Q

when does volume/pressure cause a change in equilibrium

A

when the reaction is with gases, it is a result of a volume change, AND there is a change in moles

25
Q

increase in pressure when all conditions for eq change are met

A

shift toward the side with fewer gas molecules

26
Q

decrease in pressure when all conditions for eq change are met

A

shift toward the side with more gas molecules

27
Q

arrhenius definition for acids and bases

A

acid has H+ when dissolved, base had OH- when dissolved

28
Q

Bronsted-Lowry definition

A

focuses more on the transfer instead of dissasociation.

Acid- donates proton
Base- accepts proton

29
Q

conjugate base

A

deprotanated form of original acid

30
Q

conjugate acid

A

protonated form of original base

31
Q

ionization

A

acid-base reactions with water

32
Q

autoionization

A

happens in every solution with water

33
Q

what is not included in eq constant

A

liquids and solids(everything else is. g and aq)

34
Q

auto ionization formula

A

H2O+H2O –> <– H3O + OH-

35
Q

autoionization only happens in how many cases

A

in all cases but only in 2 out of 10^9 molecules *VERY small

36
Q

amphoteric

A

molecules or ions that either gain or lose a proton under appropriate conditions

37
Q

as [H3O] increases, pH levels ___

A

decrease

38
Q

[H30] > [OH-]

A

acidic, pH lower

39
Q

[H30] = [OH-]

A

neutral, pH 7

40
Q

[H30] < [OH-]

A

basic, pH higher

41
Q

pH <7

A

acidic

42
Q

pH > 7

A

basic

43
Q

pH=7

A

neutral

44
Q
A
45
Q

the higher the Ka is, the ____ the acid is

A

stronger

46
Q

the higher the Kb is, the ____ the base is

A

stronger

47
Q

% ionization

A

acid concentration eq/acid concentration original x100

48
Q

conjugate partners of strong acids and bases are ____

A

neutral

49
Q

conjugate partners of weak acids and weak bases are ___

A

weak

50
Q

neutralization reaction

A

acid + base –> salt + (water)
always IRREVERSABLE (initial part, use stoich)

51
Q

strong acid/strong base

A

neutral

52
Q

strong acid/weak base (and why)

A

con acid does this- slightly acidic

53
Q

weak acid/strong base and why

A

slightly basic (con base does this)

54
Q

buffers

A

mixtures of weak acids and bases w conjugate partners (and I think they cause H2O to form??)

55
Q

henderson-hassebach

A

use in buffers

56
Q

strong acids

A

HCl
HBr
HI
HNO3
HClO4
H2SO4

57
Q

strong bases

A

NaOH
KOH
Ba(OH)2
Sr(OH)2
Ca(OH)2
LiOH

Sophomore- Spring 2024- Mac (11 decks)

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