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UK GCSE Chemistry > Acids and Bases (C4) > Flashcards

Acids and Bases (C4) Flashcards

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1
Q

What does pH measure?

A

Acidity or Alkalinity

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2
Q

What is indicator?

A

A dye that changes colour depending on its pH

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3
Q

Is pH 7 acid or alkali?

A

Neutral

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4
Q

Is pH 5 acid or alkali?

A

Acid

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5
Q

Is pH 9 acid or alkali?

A

Alkali

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6
Q

Is pH 14 acid or alkali?

A

Strong Alkali

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7
Q

Is pH 1 acid or alkali?

A

Strong Acid

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8
Q

What can we use to judge pH?

A

pH probe or indicator

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9
Q

Define Acid

A

Substances that form aqueous solutions with a pH below 7

They form H+ ions in water

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10
Q

Define Base

A

A substance with a pH greater than 7

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11
Q

Define Alkali

A

A base dissolved in water to form a solution greater than 7

Alkalis form OH- ions in water

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12
Q

Neutralisation Reaction

A

Base + Acid = Water + Salt

BAWS

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13
Q

Neutralisation Reaction in terms of ions

A

H+(aq) + OH- = H2O(l)

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14
Q

What is titration for?

A

They allow you to find exactly how much acid is needed to neutralise an alkali or vie versa.

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15
Q

What is the first step of a titrartion?

when you are finding the concentration of an alkali needed for the neutralisation of an acid

A

Use a pippette and pippette filler, add a set volume (25cm^3) of the alkali to a conical flask. Add a few drops of indicator.

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16
Q

What is the second step of a titrartion?

when you are finding the concentration of an alkali needed for the neutralisation of an acid

A

Use a funnel to fill a burette with acid. Make sure you do this below eye level. Record the initial volume of the acid in the burette.

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17
Q

What is the third step of a titrartion?

when you are finding the concentration of an alkali needed for the neutralisation of an acid

A

Add acid slowly from the burette into the conical flask, swirlig constantly until you see the end-point. This is visible when the colour changes.

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18
Q

What is the fourth step of a titrartion?

when you are finding the concentration of an alkali needed for the neutralisation of an acid

A

Record the final volume of the acid in the burette and use it to calculate the volume of acid needed to neutralise the alkali.

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19
Q

What should you do to increase the accuracy of your titration?

A

You should take several consstent results. Take only answers within 0.1cm^3 of each other and ignore any anomalous results.

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20
Q

Why is universal indicator not ideal for titrations?

A

It changes colour gradually

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21
Q

What indicators are best for titrations?

A

Single indicators

litmus, phenolphthalein, methyl organge

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22
Q

What colour does litmus paper turn?

A

Blue in alkalis and red in acids.

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23
Q

What colour does phenolphthalein turn?

A

Pink in alkalis and colourless in acids and neutral

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24
Q

What colour does methyl orange turn?

A

Yellow in alkalis and red in acids

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25
Q

What is a strong acid?

A

Fully ionising in an aqueous solution

They produce H+ hydrogen ions

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26
Q

What is a weak acid?

A

Weak acids do not fully ionise in aqueous solutions. Only a small proportion of acid particles dissociate to release H+ ions.

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27
Q

Examples of strong acids

A

Sulphuric Acid
Hydrochloric Acid
Nitric Acid

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28
Q

Examples of weak acids

A

Ethanoic Acid
Citroc Acid
Carbonic Acid

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29
Q

The ionisation of which acids is reversible?

A

Weak Acids

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30
Q

What is pH?

A

Concentration of H+ ions

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31
Q

If the concentration of H+ ions in an acid that was pH 4 is increased by a factor of 10, what is the pH now?

A

pH5

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32
Q

Which has a higher pH, strong acid or weak acid?

A

Weak acid has a higher pH than strong acid

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33
Q

Reaction between acid and metal oxide

A 
Metal Oxide (Base) + Acid = Water + Salt
BAWS
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34
Q

Reaction between acid and metal hydoxide

A 
Metal Hydroxide (Base) + Acid = Water + Salt
BAWS
35
Q

What is salt produced in a reaction between hydrochloric acid and a metal?

A

Metal chloride

36
Q

What is salt produced in a reaction between sulphuric acid and a metal?

A

Metal sulphate

37
Q

What is salt produced in a reaction between nitric acid and a metal?

A

Metal nitrate

38
Q

Reaction between acid and metal carbonate

A

Metal Carbonate + Acid = Water + Carbon Dioxide + Salt

CAWCS

39
Q

Name 3 types of bases

A

Metal oxides
Metal hydroxides
Metal carbonates

40
Q

Which base does not form a BAWS reaction?

A

Metal Carbonates form a CAWCS reaction (with carbon dioxide)

41
Q

How do you make a soluble salt from an insoluble base?

A
  • Gently warm the dilute acid on a bunson burner, then switch off
  • Add the base, stirring until it sinks to the bottom (it will be in excess at this point)
  • Filter out excess base
  • Gently heat the solution in a water bath or electric heater to evaporate water
  • Stop heating and allow to cool
  • Filter and dry the crystals
42
Q

What process seperates an insoluble?

A

Crystallisation

43
Q

What is the reactivity series?

A

Order of metal reactivity

44
Q

Which non-metals are in the reactivity series?

A

Hydrogen and Copper

45
Q

How reactive is Potassium (K)

A

Very

46
Q

How reactive is Copper (Cu)

A

Not very

47
Q

How reactive is Carbon (C)

A

Fairly

48
Q

How reactive is Lithium (Li)

A

Very

49
Q

How reactive is Hydrogen (H)

A

Not very

50
Q

How reactive is Sodium (Na)

A

Very

51
Q

How reactive is Magnesium (Mg)

A

Fairly

52
Q

How reactive is Iron (Fe)

A

Fairly

53
Q

How reactive is Calcium (Ca)

A

Very

54
Q

How reactive is Gold (Au)

A

Not - It’s a native metal

55
Q

How reactive is Zinc (Zn)

A

Fairly

56
Q

Define Native Metal

A

Usually found in their pure form, pretty much unreactive

57
Q

What forms if an acid reacts with a metal?

A

Acid + Metal = Salt + Hydrogen

58
Q

Test for Hydrogen

A

Squeaky Pop test

Place a lit splint near it, you should hear a ‘squeaky-pop-

59
Q

Which metals will readily undergo a reaction with acids?

A

Anything more reactive than hydrogen

60
Q

What forms if water reacts with a metal?

A

Metal + Water = Metal Hydroxide + Hydrogen

61
Q

Which metals will readily undergo a reaction with water?

A

Potassium (K)
Sodium (Na)
Lithium (Li)
Calcium (Ca)

62
Q

Define Oxidation

A

(Gain of oxygen)

Loss of electrons

63
Q

Define Reduction

A

(Loss of oxygen)

Gain of electrons

64
Q

How do we extract metals with low reactivity from their ores?

A

Reduction using carbon

anything less reactive than carbon

65
Q

How do we extract metals with high reactivity from their ores?

A

Electrolysis

anything more reactive than carbon

66
Q

Why can highly reactive metals not be extracted with carbon?

A

This reduction is a displacement reaction, more reactive metals will not be displaced by carbon

67
Q

What type of reaction is reduction using carbon?

A

Displacement Reaction

68
Q

What is a displacement reation?

A

When a more reactive element takes the place of a less reactive one in a compound

69
Q

What is a redox reaction?

A

A reaction where electrons are transferred

70
Q

Oxygen is essential to an oxidation or reduction reaction. True or False?

A

False

Any electron loss or gain classifies as a reduction or oxidation

71
Q

What do we call an ion which does not change in a reaction?

A

Spectator ions

72
Q

Define Electrolysis

A

Using an electrical current to ‘split’ a metal compound into its elements

73
Q

Why must a metal compound be molten or aqueous during electrolysis?

A

So that the ions can move freely

74
Q

Where does the positive ion go during electrolysis?

A

Cathode (negative electrode)

75
Q

Where does the negative ion go during electrolysis?

A

Anode (positive electrode)

76
Q

What do we call the molten or aqueous solution during electrolysis?

A

Electrolyte

77
Q

What happens during electrolysis of a molten solution?

A

Two rods (electrodes) with electrical current are placed in the electolyte
Metals (positive ions) are attracted to the negative electrode
Non - metals (negative ions) are attracted to the positive electrode
These can then be collected in their pure form

78
Q

What is used to lower the melting point of metal compounds such as aluminium oxide, to make a molten solution?

A

Cryolite

79
Q

What is aluminum ore called?

A

Bauxite

80
Q

What happens at the negative elctrode?

A

The positive metal ion is attracted to the negative electrode. Here it gains electrons (reduction) and becomes its element.

81
Q

What happens at the positive elctrode?

A

The negative non-metal ion is attracted to the positive electrode. Here it looses electrons (oxidation) and becomes its element.

82
Q

What additional ions are involved in the electrolysis of an aqueous solution?

A

H+ and OH-

83
Q

When does hydrogen form at the cathode?

A

Electrolysis of an aqueous solution if hydrogen is less reactive than the metal

84
Q

When does oxygen form at the annode?

A

Electrolysis of an aqueous solution if no halide ions are present (Cl2, Br2 etc..)

UK GCSE Chemistry (9 decks)

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