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Chemistry > Topic 3 > Flashcards

Topic 3 Flashcards

1
Q

sulfuric acid

A

H2SO4

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2
Q

Hydrochloric acid

A

HCl

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3
Q

Nitric acid

A

HNO3

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4
Q

Sodium Hydroxide

A

NaOH

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5
Q

Potassium Oxide

A

K2O

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6
Q

Ammonium hydroxide

A

NH4OH

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7
Q

neuteral

A

7

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8
Q

acidic

A

1-6

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9
Q

alkaline

A

8-14

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10
Q

alkali properties

A
  • slippery
  • soapy
  • burns
  • corossive
    e.g. bleach
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11
Q

acid properties

A
  • sour
  • corrosive
    e.g. lemon juice
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12
Q

universal indicator

A

acid : red, orange, yellow
alkali : blue, purple

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13
Q

Methyle orange

A

acid: red
alkaline: yellow

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14
Q

phenophelin

A

acid: colourless
alkaline: pink

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15
Q

litmus paper

A

acid: blue to red
alkaline: red to blue

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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

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17
Q

hydrogen ion

A

H+

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18
Q

Hydroxide ion

A

OH-

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19
Q

Nitrate

A

NO3 -

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20
Q

hydroxide

A

OH -

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21
Q

Carbonate

A

CO3 2-

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22
Q

Sulfate

A

SO4 2-

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23
Q

acids are

A

chemicals that when dissolve split to release hydrogen ions

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24
Q

alkalis are

A

bases that when dissolved in water split to release hydroxide ions

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25
Q

neuteral solutions

A

have an equal amount of H+ and OH- ions

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26
Q

strong acid

A

completely dissociated into H+ ions

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27
Q

weak acid

A

partially dissociated into H+ ions

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28
Q

ph scale measured by

A

how many H+ ions there are

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29
Q

ph scale H+ ions

A

PH 2 has ten times more H+ ions than PH 3

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30
Q

all alkalines…

A

alkalies are bases and are soluble in water

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31
Q

acids are always

32
Q

H+ + OH-

33
Q

hydrochloric acid

34
Q

sulfuric acid

35
Q

nitric acid

36
Q

metal oxide + acid

A

salt + water

37
Q

metal hydroxide + acid

A

salt + water

38
Q

metal + aicd

A

salt + hydrogen

39
Q

metal carbonate + acid

A

carbon dioxide
water
salt

40
Q

test for hydrogen

A

lit splint squeaky pop

41
Q

test for oxygen

A

glowing splint relights

42
Q

test for chlorine

A

blue litmus paper turns red then bleaches

43
Q

test for co2

A

blow into colourless limewater
turns cloudy/ milky

44
Q

solubility nitrates

A

all soluble

45
Q

solubility chlorides

A

all soluble apart from silver and lead

46
Q

solubility sulfates

A

all soluble apart from lead, barium and calcium

47
Q

carbonates and hydroxides

A

all insoluble except those of sodium potassium and ammonium

48
Q

precipitation reaction

A

when an insoluble solid is formed when two soluble substances react

49
Q

making copper sulfate

A

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
Q

Copper ions produce

A

clear blue solution

51
Q

Titration

A
  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
  7. leave dish in warm place like a radiator to allow water to vaporise and crystals to form
52
Q

acid + base

A

add an excess of the insoluble base to use up all the acid
filter off the left over base

53
Q

acid + alkali

A

mix the acid and alkali until the soloution is neuteral ensureing no left over acid or alkiali
check ph7

54
Q

anhydrous salt crystals

A

no water in them
boil off all the water

55
Q

hydratyed slat crytsals

A

have water in them
boil off some of the after and leave it to evaporate and crystalise

56
Q

electricity is needed to

A

needed to break down ionic compounds

57
Q

negative eletrode

A

cathode
cations

58
Q

positive eletrode

A

anode
anions - halogens

59
Q

AlO

A

cathode: aluminium
anode: oxygen

60
Q

potassium Iodide

A

cathode: potassium
anode: iodine

61
Q

electrolysis of zinc chloride

A

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
Q

at the cathode

A

if the metal is more reactive than hydrogen, hydrogen will be produced

63
Q

at the anode

A

if halogen is present it will form
if not present OH- will form

64
Q

pure copper cathode

A

gains mass

65
Q

impurites

A

from the anode dont form ions and collect bellow as sludge which is collected as it may conatin valuable metalic elements

66
Q

impure copper anode

A

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
Q

unreactive

68
Q

equation at the anode

A

Cu -> Cu 2+ + 2e-

69
Q

at the cathode

A

Cu2+ + 2e- -> Cu

70
Q

acid reacts with alkali

A

neutralisation

71
Q

how is h2 gas produced at teh cathode

A

H+ ions are attracted to the cathode , gain electrons and form hydrogen gas.

72
Q

how is O2 gas produced at teh anode

A

OH - ions are attracted to the anode , lose electrons and form oxygen gas.

73
Q

why does teh solution remain blue

A

the same amount of ions entered and left the solution

74
Q

Suggest why universal indicator must not be used in titration experiments

A

colour chge too gradual, too many colours

75
Q

Explain, in terms of the particles present, why the pH increases during the experiment.

A

H+ ions neuteralised
H+ +OH- -> H2O
less H+ ions, concentration falls

76
Q

) State two observations that would show the reaction has finished.

A

no more colour chnage
bubles stop

77
Q

Suggest a reason why the actual yield was greater than the theoretical yield

A

not all the water had evaporated

Chemistry (9 decks)

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