Topic 3 Flashcards
(77 cards)
1
Q
sulfuric acid
A
H2SO4
2
Q
Hydrochloric acid
A
HCl
3
Q
Nitric acid
A
HNO3
4
Q
Sodium Hydroxide
A
NaOH
5
Q
Potassium Oxide
A
K2O
6
Q
Ammonium hydroxide
A
NH4OH
7
Q
neuteral
A
7
8
Q
acidic
A
1-6
9
Q
alkaline
A
8-14
10
Q
alkali properties
A
- slippery
- soapy
- burns
- corossive
e.g. bleach
11
Q
acid properties
A
- sour
- corrosive
e.g. lemon juice
12
Q
universal indicator
A
acid : red, orange, yellow
alkali : blue, purple
13
Q
Methyle orange
A
acid: red
alkaline: yellow
14
Q
phenophelin
A
acid: colourless
alkaline: pink
15
Q
litmus paper
A
acid: blue to red
alkaline: red to blue
16
Q
whats the best indicator
A
ph pro/ metre as it doenst ruin the solution and tells you how strong or weak the substance is
17
Q
hydrogen ion
A
H+
18
Q
Hydroxide ion
A
OH-
19
Q
Nitrate
A
NO3 -
20
Q
hydroxide
A
OH -
21
Q
Carbonate
A
CO3 2-
22
Q
Sulfate
A
SO4 2-
23
Q
acids are
A
chemicals that when dissolve split to release hydrogen ions
24
Q
alkalis are
A
bases that when dissolved in water split to release hydroxide ions
25
neuteral solutions
have an equal amount of H+ and OH- ions
26
strong acid
completely dissociated into H+ ions
27
weak acid
partially dissociated into H+ ions
28
ph scale measured by
how many H+ ions there are
29
ph scale H+ ions
PH 2 has ten times more H+ ions than PH 3
30
all alkalines...
alkalies are bases and are soluble in water
31
acids are always
aq
32
H+ + OH-
H2O
33
hydrochloric acid
chloride
34
sulfuric acid
sulfate
35
nitric acid
nitrate
36
metal oxide + acid
salt + water
37
metal hydroxide + acid
salt + water
38
metal + aicd
salt + hydrogen
39
metal carbonate + acid
carbon dioxide
water
salt
40
test for hydrogen
lit splint squeaky pop
41
test for oxygen
glowing splint relights
42
test for chlorine
blue litmus paper turns red then bleaches
43
test for co2
blow into colourless limewater
turns cloudy/ milky
44
solubility nitrates
all soluble
45
solubility chlorides
all soluble apart from silver and lead
46
solubility sulfates
all soluble apart from lead, barium and calcium
47
carbonates and hydroxides
all insoluble except those of sodium potassium and ammonium
48
precipitation reaction
when an insoluble solid is formed when two soluble substances react
49
making copper sulfate
1 add excess copper oxide
2 gently warm mixture to speed up the reaction
3 filter to remove unreacted solid from solution
4 heat to evaporate water and concentrate the salt solution
5 leave to evaporate water slowly for crystallisation to occur
50
Copper ions produce
clear blue solution
51
Titration
1. mesure teh alkali using a pipette
2. add a few drops of indicator phenothiazine
3. add acid from teh burette
4. continue adding acid until there's a colour change and end point recorded
5. repeat without indicator
6. add salt solution to evaporating dish and heat until the water has evaporated to concentrate
6. leave dish in warm place like a radiator to allow water to vaporise and crystals to form
52
acid + base
add an excess of the insoluble base to use up all the acid
filter off the left over base
53
acid + alkali
mix the acid and alkali until the soloution is neuteral ensureing no left over acid or alkiali
check ph7
54
anhydrous salt crystals
no water in them
boil off all the water
55
hydratyed slat crytsals
have water in them
boil off some of the after and leave it to evaporate and crystalise
56
electricity is needed to
needed to break down ionic compounds
57
negative eletrode
cathode
cations
58
positive eletrode
anode
anions - halogens
59
AlO
cathode: aluminium
anode: oxygen
60
potassium Iodide
cathode: potassium
anode: iodine
61
electrolysis of zinc chloride
zinc ions gain 2 electrons to become zinc atoms
each chloride atom looses one electron to become chloride atom
2 chlorine atoms bond to form a molecule
62
at the cathode
if the metal is more reactive than hydrogen, hydrogen will be produced
63
at the anode
if halogen is present it will form
if not present OH- will form
64
pure copper cathode
gains mass
65
impurites
from the anode dont form ions and collect bellow as sludge which is collected as it may conatin valuable metalic elements
66
impure copper anode
coppper atoms loose two electrons to become copper ions
loose mass
these ions dissolve into teh solution and migrate to the pure copper cathode where they gain electrons to become copper atoms
looses mass
67
unreactive
inert
68
equation at the anode
Cu -> Cu 2+ + 2e-
69
at the cathode
Cu2+ + 2e- -> Cu
70
acid reacts with alkali
neutralisation
71
how is h2 gas produced at teh cathode
H+ ions are attracted to the cathode , gain electrons and form hydrogen gas.
72
how is O2 gas produced at teh anode
OH - ions are attracted to the anode , lose electrons and form oxygen gas.
73
why does teh solution remain blue
the same amount of ions entered and left the solution
74
Suggest why universal indicator must not be used in titration experiments
colour chge too gradual, too many colours
75
Explain, in terms of the particles present, why the pH increases during the experiment.
H+ ions neuteralised
H+ +OH- -> H2O
less H+ ions, concentration falls
76
) State two observations that would show the reaction has finished.
no more colour chnage
bubles stop
77
Suggest a reason why the actual yield was greater than the theoretical yield
not all the water had evaporated
