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Chem1120 > unit 3 > Flashcards

unit 3 Flashcards

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1
Q

define WATER IONIZATION

A

water dissociates slightly in water

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2
Q

what self ionizes into

A

H3O+ and OH-

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3
Q

the kc of pure water is equal to/referred to as

A

Kw

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4
Q

Kw is dependent on what

A

temperature

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5
Q

H3O+ and OH- are ___ to each other and __ present

A

inverse; always

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6
Q

greater H3O+ means there will be ___ OH-

A

less

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7
Q

a pH of less than 7 and pOH of more than 7 means the solution is

A

acidic

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8
Q

a solution is __ if the pH is more than 7 and the pOH is less than 7

A

basic

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9
Q

a solution is __ if the pH and pOH both equal 7

A

neutral

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10
Q

pH and pOH are ___ proportional

A

inversely

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11
Q

pH correlates with

A

acids

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12
Q

pOH correlates with

A

bases

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13
Q

define STRONG ACIDS

A

strong acid that is a strong electrolyte and completely dissociates into its conjugate base

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14
Q

t/f: all strong acids are converted into its products

A

true

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15
Q

what are the products of strong acids

A

H3O+ and conjugate base

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16
Q

what is the Kc of strong acids

A

much bigger than 1

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17
Q

list the strong acids

A

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

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18
Q

what are the two classifications of strong acids

A
  • hydrohalic acids
  • oxoacid with at least 2 or more oxygen than hydrogens
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19
Q

define STRONG BASES

A

strong base that are strong electrolytes

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20
Q

strong bases have __ and are group 1A or 2A ___

A
  • oxygen/OH ions
  • cations
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21
Q

how is the pOH found for group 2a strong bases

A

-log(coefficient * concentration)

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22
Q

define WEAK ACIDS

A

acid that is not strong that dissociates slightly

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23
Q

t/f: weak acids are not at equilibrium but strong acids are

A

false, strong acids are not at equilibrium bc they completely dissociate. weak acids are at equilibrium bc they dissociate slightly

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24
Q

in weak acids, the concentration of strong acid at equilibrium is about ____ as the initial concentration of strong acid

A

the same

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25
what is the concentration of conjugate base compared to initial concentration of acid in a weak acid
little (less conjugate base than the initial concentration of acid)
26
how do the amounts of H3O+ and conjugate base compare to each other in a weak acid
they are equal and both are less than the initial concentration of the weak acid
27
what is the Kc of weak acids
way smaller than 1
28
list types of weak acids
- hydrohalic - acids where hydrogen is not bonded to O or halogen - oxoacids where # of oxygens are the same or one more than # of hydrogens - organic carboxylic acids (RCOOH)
29
what is the formular for percent dissociation for weak acids
[H3O+]/[HA]init
30
if the concentration of initial weak acid decreases, the percent dissociation __
increases
31
why does the percent dissociation increase even though the concentration of weak acid dissociated decreases with a decrease in initial weak acid concentration
fraction of ions increases
32
a decrease in initial weak acid concentration causes a shift to the
right
33
define POLYPROTIC ACIDS
acids with more than 1 ionizable hydrogen
34
define BINARY ACIDS
nonmentals and hydrogen
35
define HYDROHALIC ACIDS
hydrogen bonded to halogen
36
what does the oxoacid strength depend on
- electronegativity on nonmetal - # of oxygen around nonmetal
37
in oxoacids with the same # of oxygens: if the ___ increases the acidity increases
electronegativity
38
in oxoacids of different #s of oxygen: the ___ increases the acidity increases
number of oxygens
39
define HYDRATED METAL IONS
small and highly charged ions that release hydrogen and increase acid strength
40
water acts as a __ in the presence of hydrated metal ions
base
41
Fe(H2O)3 is a
hydrated metal ion
42
t/f: weak bases dissociate in water and produce ions upon rxns
false, weak bases do NOT dissociate in water BUT they do produce ions upon rxns
43
define Kb
base dissociation
44
define Ka
acid dissociation
45
a strong acid has a __ Ka and ___ pKa than a weak acid
higher, lower
46
a strong acid has a ___ pH causing a ___ pKa
smaller, smaller
47
a weak acid has a ___ pH causing a __ pKa
higher, higher
48
if something has a smaller pH, then it has a __ concentration of H3O+
larger
49
if something has a larger pH, it has a ___ concentration of H3O+
lower
50
t/f: anions of weak acids generally function as weak bases
true
51
if both cations and anions in a salt reacts, the pH depends on the ___ of the acid and base
relative strength
52
define the LEVELING EFFECT (exerted by water)
all strong acids & bases are equally strong in water
53
what is the strongest acid in water
H3O+
54
what is the strongest base in water
OH-
55
define LEWIS BASE
donates electron pair and is typically negative
56
define LEWIS ACID
accepts electron pair and is typically positive
57
give two examples of famous lewis acids
boron and aluminum
58
the product of a lewis acid-base rxn is called an
adduct
59
t/f: all bronsted-lowry bases are lewis bases
true
60
t/f: all bronsted-lowry acids are lewis acids
false, lewis acids expand the classification of acids from bronsted-lowry
61
metal cations acts as __ when dissolved in water
acids
62
a weak acid produces a __ conjugate base
weak
63
the weaker the weak acid the __ the conjugate base
stronger
64
a weak base produces a ___ conjugate acid
weak
65
a strong base cation and anion of strong acids are
neutral
66
a cation of a weak base, and small and charged metal cation, and anion of a weak acid produces __ solutions
acidic
67
what determines the pH of a cation of weak base/small metal cation and an anion of a weak acid
the Ka and Kb
68
a cation weak base and anion of strong acid produces a __ solution
acidic
69
a small and charged metal cation and anion of strong acid produces a __ solution
acidic
70
a cation of a strong base and anion of a weak acid produces a ___ solution
acidic
71

Chem1120 (4 decks)

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