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AQA Chemistry GCSE > Chemical Changes > Flashcards

Chemical Changes Flashcards

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1
Q

What does the pH scale go from?

A

0 to 14

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2
Q

True or false : The lower the pH of a solution, the more alkaline it is.

A

False - the lower the pH, the more acidic

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3
Q

What is the pH of a neutral substance?

A

7

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4
Q

How can you measure the pH of a solution?

A

An indicator (dye that changes colour)
A pH probe attached to a pH meter

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5
Q

What do acids and bases do to each other?

A

neutralise each other

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6
Q

What is an acid?

A

A substance that forms an aqueous solution with a pH of less than 7.

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7
Q

What ions do acids form in water?

A

H+ ions

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8
Q

What is a base?

A

Any substance that will react with an acid to form a salt.

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9
Q

What is an alkaline?

A

A base that dissolves in water to form a solution with a pH greater than 7.

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10
Q

What ions do alkalis form in water?

A

OH-

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11
Q

What is the word equation for neutralisation?

A

acid + base —> salt + water

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12
Q

What is the ionic equation for neutralisation?

A

H+ + OH- —> H2O

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13
Q

What are titrations used for?

A

To find out exactly what volume of acid is needed to neutralise a measured volume of alkali - or vice versa.

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14
Q

How would you measure the alkali?

A

Using a pipette and pipette filler

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15
Q

What do you add to the alkali?

A

An indicator

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16
Q

Give two examples of indicators in titrations.

A

Phenolphthalein and methyl orange

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17
Q

What colour is phenophthalein in acids?

A

Colourless

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18
Q

What colour is phenolphthalein in alkalis?

A

pink

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19
Q

What colour does methyl orange in an acid turn when an alkali is added?

A

From red to yellow

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20
Q

What is the acid stored in, in a titration?

A

A burette with an unknown concentration

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21
Q

Give the method for titrations. RP

A
  1. Use a pipette and pipette filler to add a set volume of alkali to a conical flask. Add two drops of indicator.
  2. Use a funnel to fill a burette with an unknown concentration of acid. Record the initial volume.
  3. Use the burette to add the acid a bit at a time, whilst swirling the conical flask. Go slowly when you think the endpoint is about to be reached.
  4. When the indicator has changed colour, the alkali has been neutralised.
  5. Record the final volume of thr acid in the burette and use it to calculate the volume used to neutralise the alkali.
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22
Q

Name the 4 apparatus used in titrations.

A

Pipette, Burette, Scale, Conical flask

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23
Q

What could you do to calculate a mean volume of acid in titrations?

A

Repeat

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24
Q

What do acids produce in water?

A

protons or H+ ions

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25
Q

What do acids do in aqueous solutions?

A

ionise, they produce H+ ions

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26
Q

What is meant by a strong acid?

A

They ionise completely in water, all particles dissociate to release H+ ions.

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27
Q

What is meant by a weak acid?

A

They do not fully ionise in a solution, only a small proportion of particles dissociate to release H+ ions.

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28
Q

What type of reaction is the ionisation of a weak acid?

A

reversible reaction

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29
Q

What is meant by the pH of an acid or alkali?

A

The concentration of H+ ions.

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30
Q

Complete the sentence: For every decrease of 1 on the pH scale, the concentration of H+ ions ___________ by a factor of ___.

A

increases, 10

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31
Q

What is meant by a concentrated acid?

A

A large amount of acid in a certain volume of liquid.

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32
Q

What is meant by a dilute acid?

A

A small amount of acid in a certain volume of liquid.

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33
Q

What are metal oxides and metal hydroxides?

A

Bases

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34
Q

What does an acid + a metal oxide/hydroxide produce?

A

Salt + Water

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35
Q

What does an acid + a metal carbonate produce?

A

Salt + Water + Carbon dioxide

36
Q

How can you make soluble salts using an insoluble base? RP

A
  1. Gently warm the acid using a bunsen burner then remove from the heat.
  2. Add the insoluble base in excess to the acid.
  3. Filter out the excess solid to get the salt solution.
  4. Gently heat the solution in an evaporating basin over a bunsen burner until about half has evaporated and crystals have begun to form.
  5. Stop heating and leave the solution to cool or pat dry.
37
Q

List the reactivity series?

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminuim
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold

38
Q

What is the most reactive element in the reactivity series?

A

Potassium

39
Q

What is meant by reactivity?

A

How easily an element loses electrons

40
Q

What does an acid + metal produce?

A

Salt + hydrogen

41
Q

What does a metal + water produce?

A

Metal hydroxide + hydrogen

42
Q

What metals don’t react with water?

A

zinc, iron, copper

43
Q

What are ores?

A

Compounds that contain an element due to its reactivity.

44
Q

What is oxidation?

A

The gain of oxygen

45
Q

What is reduction?

A

The loss of oxygen

46
Q

What is an oxide?

A

A metal compound that contains oxygen

47
Q

How can metals be extracted by reduction?

A

Using carbon

48
Q

What metals can be extracted by carbon?

A

Metals below carbon in the reactivity series

49
Q

What does OILRIG stand for?

A

Oxidation
Is
Loss (of electrons)
Reduction
Is
Gain (of electrons)

50
Q

What is a redox reaction?

A

When reduction and oxidation happen at the same time.

51
Q

What are three examples of redox reactions?

A

Metals reacting with acids
Halogen displacement reactions
Metal displacement reactions

52
Q

What happens when metals react with acids?

A

Metal atoms become oxidised (lose electrons)
The hydrogen ions are reduced (gain electrons)

53
Q

Complete the sentence: A ________ reactive halogen can displace a ________ reactive halogen from a salt solution.

A

More, less

54
Q

Which ion becomes reduced when copper sulphate is reacted with iron?

A

Copper gains electrons

55
Q

What is meant by electrolysis?

A

Splitting up with electricity

56
Q

During electrolysis, what is passed through the electrolyte?

A

An electric current.

57
Q

What is an electrolyte?

A

A molten or dissolved ionic compound

58
Q

What charge does the cathode have?

A

Negative

59
Q

What charged ions does the cathode attract?

A

Positive

60
Q

What happens to the ions at the cathode?

A

They become reduced/gain electrons

61
Q

What is the positive electrode called?

A

The anode

62
Q

What charged ions does the anode attract?

A

negative

63
Q

What happens to the ions at the anode?

A

They become oxidised/lose electrons

64
Q

What does electrolysis of molten ionic solids form?

A

elements

65
Q

Why can’t ionic solids be electrolysed?

A

The ions are in fixed positions and can’t move

66
Q

In electrolysis of molten ionic solids, what type of ion is reduced at the cathode?

A

metal ions

67
Q

In electrolysis of molten ionic solids, what type of ion is oxidised at the anode?

A

non-metal ions

68
Q

What are electrodes made of?

A

An inert material, often graphite

69
Q

What metals are extracted by electrolysis?

A

Metals more reactive than carbon

70
Q

What are the disadvantages of electrolysis?

A

Very expensive and requires lots of energy

71
Q

What ore is aluminium extracted from?

A

bauxite

72
Q

What does bauxite contain?

A

Aluminium oxide

73
Q

True or false : Aluminium oxide has a low melting point.

A

False - it has a very high melting point

74
Q

What is aluminium oxide mixed with to lower its melting point?

A

cryolite

75
Q

In electrolysis of aluminium oxide, what ions are attracted to the negative electrode?

A

Positive Al3+ ions are attracted to the cathode where it gains electrons to produce aluminium atoms.

76
Q

In electrolysis of aluminium oxide, what ions are attracted to the positive electrode?

A

Negative O2- ions are attracted to the anode where they lose two electrons. They then combine to form O2 molecules.

77
Q

What happens at the negative electrode during electrolysis of molten ionic solides?

A

Metals form positive ions. The metal is produced

78
Q

What happens at the positive electrode during electrolysis of molten ionic solides?

A

Non-metals form negative ions.
Oxygen is produced

79
Q

What happens at the cathode during the electrolysis of aqueous solutions?

A

If the metal is less reactive tham hydrogen, the metal is produced.
If the metal is more reactive than hydrogen, hydrogen is produced.

80
Q

What happens at the anode during the electrolysis of aqueous solutions?

A

If no halide ions are present, oxygen and water is produced.
If halide ions are present then molecules of the halogen is produced.

81
Q

What is formed at the cathode and anode in the electrolysis of copper sulfate solution?

A

Cathode: Copper
Anode: Oxygen

82
Q

What is formed at the cathode and anode in the electrolysis of sodium chloride solution?

A

Cathode: Hydrogen
Anode: Chlorine

83
Q

What are half equations?

A

Equations that show the reactions at the electrodes

84
Q

If no halide ions are present, give the half equation for the anode.

A

4OH- — 4e- —> O2 + 2H2O

85
Q

What is the half equation at the cathode if the metal is more reactive than hydrogen?

A

2H+ + 2e- —> H2

AQA Chemistry GCSE (9 decks)

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