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National 5 Chemistry > Unit 1 - Topic 2 - Acids and Alkalis > Flashcards

Unit 1 - Topic 2 - Acids and Alkalis Flashcards

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1
Q

What are indicators?

A

Indicators are dyes which change colour when reacted with an acid or alkali. There are many kinds of indicators. The one we use most often in chemistry is Universal Indicator.

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2
Q

What does universal indicator tell us?

A

If a substance is acidic, alkaline, or neutral.

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3
Q

What does the pH scale do?

A

It measures the concentration of hydrogen ions (H+). The higher the concentration of hydrogen ions, the lower the pH.

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4
Q

What is the pH of a strong acid?

A

1-3

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5
Q

What is the pH of a weak acid?

A

4-6

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6
Q

What is the pH of a neutral solution?

A

7

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7
Q

What is the pH of a weak alkaline?

A

8-10

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8
Q

What is the pH of a strong alkaline?

A

11-14

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9
Q

What is electrolysis?

A

Electrolysis is chemical decomposition produced by passing an electric current through a liquid or solution containing ions.

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10
Q

Why is water neutral?

A

Water dissociates (breaks up) to form H+ and OH- ions.

H2O ⇌ H+ + OH-

Water is neutral because it has the same/equal numbers of H+ and OH- ions.

This ⇌ means the reaction is reversible.

Acidic and alkaline solutions contain both H+ and OH- ions.

An acid contains more hydrogen (H+) ions than hydroxide (OH-) ions.

An alkali contains more hydroxide (OH-) ions than hydrogen (H+) ions.

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11
Q

What happens when an element or compound is burned in oxygen?

A

The elements combine with oxygen to form an oxide.

Combustion is another name for burning.

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12
Q

Can metals undergo combustion?

A

Yes

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13
Q

Can non-metals undergo combustion?

A

Yes

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14
Q

Describe what happens when metals undergo combustion?

A

Metals can undergo combustion to produce metal oxides. If a metal oxide is soluble, it will dissolve in water to produce a metal hydroxide (an alkali).

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15
Q

Describe what happens when non-metals undergo combustion?

A

Non-metals undergo combustion to produce non-metal oxides. Non-metal oxides dissolve in water to produce acids.

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16
Q

What should you be able to identify in any neutralisation reaction?

A

The spectator ion(s)

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17
Q

What are spectator ions?

A

Spectator ions are ions that remain unchanged by the reaction.

Spectator ions do not take part in the reaction.

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18
Q

What does (s) mean?

A

Solid

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19
Q

What does (l) mean?

A

Liquid

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20
Q

What does (g) mean?

A

Gas

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21
Q

What does (aq) mean?

A

Aqueous (in solution)

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22
Q

When naming salt’s where does the first part of the salt’s name come from?

A

The metal part of the alkali’s or base’s name.

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23
Q

When naming salt’s where does the second part of the salt’s name come from?

A

It is determined by the acid.

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24
Q

What is the second part of the salt’s name in hydrochloric acid?

A

Chloride

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25
Q

What is the second part of the salt’s name in nitric acid?

A

Nitrate

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26
Q

What is the second part of the salt’s name in sulphuric acid?

A

Sulphate

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27
Q

What is the second part of the salt’s name in phosphoric acid?

A

Phosphate

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28
Q

How many types of bases react with acids to make water and a salt?

A

3

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29
Q

Name the 3 types of bases which react with acids to make water and a salt

A

Metal Oxide
Metal Hydroxide (Alkali)
Metal Carbonate

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30
Q

What are all the reactions an acid carries out with a base?

A

Neutralisation reactions

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31
Q

How many neutralisation reactions are there?

A

4

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32
Q

Name the neutralisation reactions

A

Base + Acid –> Salt + Water

Metal hydroxide + Acid –> Salt + Water

Metal oxide + Acid –> Salt + Water

Metal carbonate + Acid –> Salt + Water + Carbon dioxide

33
Q

What is produced when metal oxides react?

A

H2O

34
Q

What is produced when metal hydroxides react?

A

H2O

35
Q

What is produced when an aqueous metals react with carbonates?

A

H2O + CO2

36
Q

What is produced when an insoluble metal reacts with carbonates?

A

H2O + CO2

37
Q

What is a base?

A

A base is a substance which reacts with an acid to produce a salt and water.

When a base reacts with an acid, neutralisation reactions take place.

38
Q

Give 2 examples of a soluble base

A

Calcium oxide

Sodium carbonate

39
Q

Give 2 examples of an insoluble base

A

Aluminium oxide

Calcium carbonate

40
Q

Describe a precipitation reaction

A

A precipitation reaction is when two solutions are mixed together to form an insoluble salt.

41
Q

How can you find the substance that is the precipitate?

A

The metal ions “swap places.” We can identify the insoluble precipitate using the data booklet.

42
Q

What does soluble mean?

A

It dissolves in water

43
Q

What do you use to prepare a soluble salt?

A

A titration

44
Q

How can you obtain a salt from a solution?

A

By evaporating the water off so that the solid salt remains

This can be done using an evaporating dish or just evaporating off the water.

45
Q

What does insoluble mean?

A

It does not dissolve in water

46
Q

When preparing a salt using an insoluble salt, how do you know the reaction is complete?

A

When the fizzing stops and no more gas/solid is produced.

47
Q

When preparing a salt using an insoluble salt, why does the mixture need to be filterred?

A

To remove any unreacted base.

48
Q

Are alkalis soluble or insoluble bases?

A

Soluble

49
Q

How are alkali solutions formed?

A

An alkaline solution can be formed when a metal oxide is dissolved in water.

Soluble metal oxides (or metal hydroxides) produce alkaline solutions.

50
Q

How are acidic solutions formed?

A

An acidic solution can be formed when a non-metal oxide is dissolved in water.

Soluble non-metal oxides produce acidic solutions.

51
Q

What affect do insoluble oxides have on the pH of water?

A

No affect

52
Q

When acid is electrolysed , what is produced at each electrode?

A

Bubbles of gas

More gas was made in the positive electrode than the negative.

53
Q

What do all acids have?

A

Ionic bonding

54
Q

What do all acids contain?

A

Hydrogen ion (H+ ion)

55
Q

What does the negative electrode give off?

A

Hydrogen gas

56
Q

What happens when water is added to a solution of ions?

A

The same number of ions remains but the concentration decreases.
The solution is said to have been diluted.

57
Q

What happens when an acid is diluted?

A

The concentration of hydrogen ions decreases.

58
Q

What happens when an alkaline is diluted?

A

The concentration of hydroxide ions decreases.

59
Q

What happens when metal oxides from group 1 and 2 dissolve in water?

A

An alkaline is produced

60
Q

What happens when non-metal oxides dissolve in water?

A

An acid is produced.

61
Q

Are transition metals soluble or insoluble and what does this mean?

A

They are insoluble, so the pH of water remains neutral.

62
Q

What happens to the indicator’s colour when the correct volume of alkali is added to the acid?

A

Changes from red to green.

63
Q

What happens to the indicator’s colour when too much alkali is added to the acid and how can this be fixed?

A

Changes from green to blue.

You can fix this by adding more acid back in

64
Q

When reacting an acid with a metal oxide, how do you know the reaction is complete?

A

When the unreacted metal oxide sank to the bottom of the beaker.

65
Q

When reacting an acid with a metal oxide, what happened as the reaction continued?

A

The pH increased towards 7

66
Q

What colour is pH 1?

A

Red

67
Q

What colour is pH 2?

A

Dark Pink

68
Q

What colour is pH 3?

A

Pink

69
Q

What colour is pH 4?

A

Orange

70
Q

What colour is pH 5?

A

Dark Yellow

71
Q

What colour is pH 6?

A

Yellow

72
Q

What colour is pH 7?

A

Green

73
Q

What colour is pH 8?

A

Dark Green

74
Q

What colour is pH 9?

A

Green Blue

75
Q

What colour is pH 10?

A

Blue

76
Q

What colour is pH 11?

A

Dark Blue

77
Q

What colour is pH 12?

A

Blue Purple

78
Q

What colour is pH 13?

A

Light Purple

79
Q

What colour is pH 14?

A

Purple

National 5 Chemistry (15 decks)

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