unit 4 test Flashcards
(116 cards)
1
Q
results a chem rxn took place
A
the temp of the rxn mixture increases
2
Q
is conducting electricity a sign if a chem rxn
A
no becuase if the initial solutions are ions they will anywyas
3
Q
what is the best way to determine a change occurred when water and X are mixed
A
measure the electrical conductivities of water and X mixture
4
Q
what is a compound that is an electrolyte
A
an ion compound
5
Q
strong electrolytes
A
strong acids bases and ionic compounds
6
Q
non electrolytes
A
covalently bonded molecular substances
except acids and bases
7
Q
weak electrolytes
A
weak acids
weak bases
8
Q
what is always a product for any combustion reaction
A
H2O is always a product in a combustion reaction
9
Q
what is broken in a chemical change
A
covalent and ionic bonds
10
Q
physical change breaks what attractions
A
intermolecular
11
Q
chemical change breaks what attractions
A
intra molecular attractions
12
Q
evidence of chem change
A
production of gas formation of precipitate or solid change in color production of heat- combustion produces heat sounds light
13
Q
for strong electrolytes to be separated into ions they have to be in what state of matter
A
they have to be aqueous
14
Q
strong electrolytes
A
are soluble ionic substances
15
Q
know your 7 strong acids
A
know your 7 strong bases
16
Q
know your polyatomic ions memorized
A
ok
17
Q
what happens to weka electrolytes
A
nothing they remain in tact(since they ar won’t aqueous?)
18
Q
as soon as you are given a particle diagram
A
count the number of particles
circle the groups based on the balanced equation
19
Q
always use law of conservation of mass
A
products equals reactants
20
Q
molar volume is used to
A
convert between moles and literdy
21
Q
what is molar volume
A
22.4 mol/1 L at STP
22
Q
what is density
A
grams per litee
23
Q
what is percent yield
A
what you got in the lab over what you are supposed to get based on stoich times 100
24
Q
the point of a titration
A
determine the mass of an unknown
25
analyze
what we are analyzing with the unknown concentration
26
titrant
in the burrette what we have a known concentration of
27
burrette
most precise piece of glassware in a lab
28
equivalence point
when the analyte is totally consumed by the titrant
29
end point
when the color has changed
30
based on the volume of the flask and the volume of what is in the burrette you cna
determine the concentration at equivalence point
31
precipitation reaction is a
DR (double replacement) reaction that creates a solid
32
acid base reaction
a neutralization reaction where an acid donates a proton and a salt and water are formed
33
neutralization run means
we form water
34
redox
involves transfer of electrons
35
combustion runs are
```
a subclass of redox reactions
carbon and water are always formed
```
36
an acid according to bronsted lowry
an acid is. proton donor
37
base according to bronsted lowry
proton acceptor
38
what is an amphoteric substance
water, it cna be an acid or a base
39
what are elements
substances that can’t be decomposed into simpler substances by chemical or physical means
40
what is important to to note about physical changes
they are usually reversible
41
Na + Cl2 -> NaCl
composition (synthesis) rxn
42
KClO3 -> KCl + O2
Decompostion
43
Mg+HCl-> MgCl2 + H2
single ionic replacement
44
LiCl + AgNO3 -> LiNO3 + AgCl
double ionic replacement
45
C3H8 + O2 -> CO2 + H2O
combustion of a hydrocarbon
46
Mg + O2 -> MgO
combustion of a metal
47
what reaction is NOT a double replacement rxn
redox rxns
48
gas to liquid
condensation
49
liquid to gas
vaporization
50
solid to liquid
fusion(melting)
51
liquid to solid
freezing
52
solid to gas
sublimation
53
gas to solid
deposition
54
7 diatomic elements
H2 N2 O2 F2 Cl2 Br2
55
dissolution example w ionic and strong acids and bases
| NaCl(s)->NaCl(aq)
NaCl(s)-> Na+(aq) + Cl-(aq)
56
dissolution example: non ionic and weak acids/bases
| C6H12O6(s) -> C6H12O6(aq)
no change
C6H12O6(s) -> C6H12O6(aq)
57
the theoretical yield is also the
limiting reactant
58
acid base titration
either acid or base is titrant, pH meters cna determine equivalence point
59
redox titration
a color change is produced when oxidation state of a metal ion in the rxn changes
60
precipitation titration
when the titrant reacts w ions in the analyze a precipitation can occur
61
how will a strong acid or base act in water
it will completely ionize or be soluble
62
how will a weak aoc dot base act in water
it will have less than 100% ionization
63
strong acids
HClO3 HBr HCl HI HNO3 HClO4 H2SO4
64
strong bases
LiOH NaOH KOH RbOH Ca(OH)2 Sr(OH)2 Ba(OH)2
65
a strong acid forms a
a weak conjugate base and vice versa
66
a weak acid forms a
strong conjugate base and vice versa
67
What happens to the IMF
melting
weakening
68
What happens to the IMF
| boiling
breaking
69
What happens to the IMF
| condensing
forming
70
What happens to the IMF
| sublimation
breaking
71
What happens to the IMF
| deposition
forming
72
What happens to the IMF
| freezing
forming
73
metal and strong acid form a
| Mg+2HCl ->
salt and gas(usually H2)
| MgCl2 + H2
74
carbonate and strong acid form a
| MgCO3 + HCl ->
combustion reaction is an ion in addition to water and carbon dioxide
MgCl2+H2O +CO2
75
weak electrolyte have
partial dissociation
76
strong electrolytes have
complete dissociation
77
completing the following equations for an ionic compound place in water means
do the mismatching compound thing and find the solubility of the products(should be aqueous)
usually decomposition or double replacement
78
is the LR bigger or smaller than the ER
the LR is smaller
79
what do you use to find the excess reactant
the limiting reactant
80
what type of compounds are non electrolytes
polar covalen
81
what types of compounds are weak electrolytes
weak acids
82
what type of compounds are strong electrolytes
ionic compounds
83
If acid/ base is stronger than CA/CB which direction does the reaction proceed
To the right
84
If CA/CB is stronger than the acid/ base which direction does the reaction proceed
To the left
85
What is a neutralization reaction
Acid reacting with a base
86
What are the products of a neutralization reaction
Salt and water
87
What si the net ionic reaction for any strong acid/strong base rxn
H+ +OH- -> H2O
88
What is a salt
A compound with no net charge, the opposing charges balance out
89
What elements tend to be good oxidizing agents
No metals
90
What elements tend to be good reducing agents
Metals
91
What does acid base titration do
It determines how much volume acid or base is in a solution
| That will completely react with it
92
As we add base what happens to the pH
As the volum of the base increases the pH slowly rise then sharply increases at the equivalence point
93
What’s the titrant
The known concentration
94
What’s the analyte/titrand
The unknown solution your want to known the concentration of
95
What’s the point of a titration
Determine concentration of unknown solution by adding a concentration of a known solution
96
What does an indicator do
Mark the endpoint of a titration
97
As the volume of the titrant increases what happens to the color of the indicator
It appears then disappears as you swirl and infills it becomes a colored solution
98
Typically titrations are formed how many times
3 times and average volume is used
99
If a molecule is a weak acid what happens to it in a net ionic equation
Like HC2H3O2
You do not break it up for net charge because weak acids(or electrolytes) don’t fully dissociate or ionize
100
If HCl is an acid what is it’s conjugate
| And why
Cl-
1 less H and 1 less charge
101
If H2O is a base what is its conjugate
H3O+
One extra H and one extra positive charge
102
Amohoteric
Substances that are able to act as an acid or base (water?)
103
What can MV = MV be used for
Determining molarity of unknown solution that reacts with known sokution(titration)
M is moles and v is volume in L
104
What does a non electrolyte do
Not dissociate at all
105
What does a weak electrolyte do
Some molecules dissociate some do not
106
What does a strong electrolyte do
Everything completely dissociates
107
What is the driving force in the net equation
Something that isn’t (aq) aka something that can’t be ionized and broken up in the net equation
108
When does M1V1=M2V2 work
In neutralization reaction
When there is one OH in one equation and one H in the other
1:1 ratio
109
What is a neutralization reaction
Moles of acid must equal moles of base
110
For solution equations first
Find the products side and balance the equation to use for mol ratio!
111
What product should you always try to get in a neutralization reaction
Water H2O
112
when u add base to a strong acid to a strong base solution what happens to the pH
it increases
113
when you add acid to a strong base to a a strong acid solution what happens to the pH
it decreases
114
in pH titration curve the volume corresponds to what
the titration in the left of the solution
115
the equivalence point occurs when the slope is
vertical
116
when calculating charges for redox rxns consider
the coefficient multiply the eco efficient by the charge!!
