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Edexcel GCSE Chemistry > Topic 4 Acids and alkalis > Flashcards

Topic 4 Acids and alkalis Flashcards

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1
Q
  1. What term describes a substance that attacks metals, stonework and skin?
A

corrosive

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2
Q
  1. Name an acidic solution found in the kitchen.
A

vinegar or fruit juice, etc.

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3
Q
  1. Name an alkaline solution used in the kitchen.
A

bleach or oven cleaner or soap, etc.

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4
Q
  1. What type of substance turns litmus paper red?
A

acid

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5
Q
  1. How does an indicator show the acidity or alkalinity of solutions?
A

by changing colour

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6
Q
  1. What pH values represent alkaline solutions?
A

above 7 or 8 to 14

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7
Q
  1. What happens in all chemical reactions?
A

new substances are formed

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8
Q
  1. What kind of reaction occurs between an acid and an alkali?
A

neutralisation

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9
Q
  1. What do you call a solution that is neither acidic nor alkaline.
A

neutral

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10
Q
  1. Give the name and formula of a common laboratory acid.
A

hydrochloric acid (HCl) or nitric acid (HNO3) or sulfuric acid (H2SO4), etc.

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11
Q
  1. Which ion is in excess in all acidic solutions?
A

hydrogen ions or H+ ions

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12
Q
  1. Which ion is in excess in all alkaline solutions?
A

hydroxide ions or OH– ions

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13
Q
  1. What scale is used for measuring acidic and alkaline properties?
A

the pH scale

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14
Q
  1. Name three examples of acid/alkali indicators apart from universal indicator.
A

litmus, methyl orange and phenolphthalein

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15
Q
  1. What would you use to measure pH to one decimal place?
A

a pH meter

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16
Q
  1. What pH values are acidic?
A

below 7

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17
Q
  1. What colour is phenolphthalein in a solution with a pH of 2?
A

colourless

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18
Q
  1. What happens to the pH as the H+ ion concentration increases?
A

it decreases

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19
Q
  1. If a solution has the same concentration of hydrogen ions as hydroxide ions, how is it described?
A

neutral or pH = 7

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20
Q
  1. If 2 g of salt is dissolved in 250 cm3 of solution, what is its concentration in g dm–3?
A

8 g dm–3

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21
Q
  1. What word describes a solution that contains a large amount of solute in a small volume of solvent?
A

concentrated

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22
Q
  1. How can a solution be made more dilute?
A

by adding solvent/water

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23
Q
  1. If 24 g of acid is dissolved in 600 cm3 of solution, what is its concentration in g dm–3?
A

40 g dm–3

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24
Q
  1. What happens when strong acid molecules dissolve in water?
A

they dissociate completely into ions

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25
Q
  1. What kind of reaction occurs between an acid and a base?
A

neutralisation

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26
Q
  1. What happens to the pH of an acid as it reacts with a neutraliser?
A

pH increases

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27
Q
  1. What is formed when an acid reacts with a base like a metal oxide?
A

salt + water

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28
Q
  1. What acid would be used to make zinc sulfate from zinc oxide?
A

sulfuric acid (sulphuric acid makes sulphates!)

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29
Q
  1. What process can be used to separate an insoluble solid from a liquid?
A

filtration

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30
Q
  1. How can a sample of a dissolved salt be obtained from a salt solution?
A

evaporation of the water

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31
Q
  1. In general, what is the pH of an alkaline solution?
A

greater than 7

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32
Q
  1. Which ions, hydrogen ions or hydroxide ions, are released by alkalis in solution?
A

hydroxide ions (OH-)

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33
Q
  1. What colour is litmus solution in acidic solutions?
A

red

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34
Q
  1. What name is given to substances that react with acids to form a salt and water only?
A

bases (bases are metal oxides and hydroxides, soluble bases are alkalis)

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35
Q
  1. Which salt is formed when copper oxide reacts with sulfuric acid?
A

copper sulfate

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36
Q
  1. What type of reaction happens between an acid and a base?
A

neutralisation

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37
Q
  1. What type of solution has a pH of 7?
A

neutral

38
Q
  1. Name the acid that has the formula HCl.
A

hydrochloric acid

39
Q
  1. What colour is phenolphthalein in alkaline solutions?
A

pink (it is colourless in acid conditions)

40
Q
  1. What is the formula for sulfuric acid?
A

H2SO4

41
Q
  1. Name the salt produced when sodium hydroxide reacts with hydrochloric acid.
A

sodium chloride

42
Q
  1. Which ions, hydrogen ions or hydroxide ions, are released by acids in solution?
A

hydrogen ions (H+)

43
Q
  1. What substance, other than a salt, is produced when an alkali neutralises an acid?
A

water

44
Q
  1. What name is given to substances that are soluble bases?
A

alkalis

45
Q
  1. What is the formula for hydrochloric acid?
A

HCl

46
Q
  1. What type of solution has a pH above 7?
A

alkaline

47
Q
  1. What colour is phenolphthalein in acidic solutions?
A

colourless – not ‘clear’

48
Q
  1. Name a piece of apparatus used to measure volumes of liquid.
A

measuring cylinder/pipette/burette

49
Q
  1. Name the separation method used to produce crystals from a solution.
A

crystallisation

50
Q
  1. Name the acid needed to make ammonium nitrate.
A

nitric acid

51
Q
  1. Which acid can be used to make copper sulfate?
A

sulfuric acid

52
Q
  1. Which base can be used to make copper sulfate?
A

copper oxide

53
Q
  1. Which substance is needed to complete the general equation: acid + base makes salt + …?
A

water (BASHO)

54
Q
  1. What is the formula of nitric acid?
A

HNO3

55
Q
  1. What is the name of the salt formed from zinc oxide and hydrochloric acid?
A

zinc chloride

56
Q
  1. What is the formula of the salt formed from calcium oxide and hydrochloric acid?
A

CaCl2

57
Q
  1. Which ions are present in large quantities in aqueous solutions of all acids?
A

H+ Hydrogen ions

58
Q
  1. Which ions are present in large quantities in aqueous solutions of all alkalis?
A

OH– Hydroxide ions

59
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium?
A

hydrogen (MASH)

60
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium carbonate?
A

carbon dioxide (CASHOCO)

61
Q
  1. What acid can be used to make copper chloride?
A

hydrochloric acid (hydrochloric acid makes chlorides)

62
Q
  1. What gas is given off when magnesium reacts with dilute sulfuric acid?
A

hydrogen (MASH)

63
Q
  1. How do you identify Hydrogen gas?
A

gives a squeaky pop with a lighted splint

64
Q
  1. What is seen when magnesium is added to dilute sulfuric acid?
A

effervescence/fizzing/bubbles (yes you know this is hydrogen, but you can not see that!!)

65
Q
  1. What is the formula of magnesium sulfate?
A

MgSO4

66
Q
  1. What gas is produced when copper carbonate is added to dilute nitric acid?
A

carbon dioxide (CASHOCO)

67
Q
  1. How do you test for Carbon Dioxide?
A

it turns limewater milky

68
Q
  1. What is the formula of the salt produced when copper carbonate reacts with nitric acid?
A

(Cu(NO3)2)

69
Q
  1. Sodium chloride dissolves in water to form a solution. Which is the solute?
A

sodium chloride

70
Q
  1. What do we call the liquid that dissolves a solute to form a solution.
A

solvent

71
Q
  1. What does methyl orange turn in acids and in alkalis
A

Red in acids Yellow in alkalis

72
Q

If a pH 5 has 10 H+ ions how many H+ ions are in a pH of 4?

A

100 H+ Times by 10 when the pH gets lower Divide by 10 when the pH gets higher

73
Q

What is the rate of reaction calculation?

A

1/time

74
Q
  1. What is BASHO?
A

base + acid = salt + water

75
Q
  1. What is MASH?
A

Metal + Acid = salt + hydrogen

76
Q
  1. What is CASHOCO?
A

Metal carbonate + acid = salt + water + carbon dioxide

77
Q

How do you prepare an insoluble salt from a precipitation reaction?

A

Simply mix the two solutions together, filter off the precipitate (salt) and dry.

78
Q
  1. What is the precipitate in this reaction? Lead nitrate + potassium iodide
A

= lead iodide + potassium nitrate Lead iodide is the precipitate as potassium nitrate is soluble

79
Q

The lower the pH the..

A

Stronger the acid.

80
Q

The higher the pH the…

A

Weaker the acid.

81
Q

What happens to the molecules of strong acids in water?

A

Their molecules dissociate (break up) completely into ions when they dissolve in water and produce high concentrations of H+ ions.

82
Q

What happens to the molecules of weak acids in water?

A

They don’t dissociate (break up) completely into ions in solution.

83
Q

Write the balanced ionic equation for neutralisation?

A

H+ (aq) + OH- (aq) = H20 (l)

84
Q
  1. Explain titration experiments, how you would go about them?
A
85
Q

What is used to place a fixed volume of a solution into a conical flask in titration?

A

A pipette.

A buiret is used to add variable amount of solution volume.

86
Q

Learn the solubility rules. What are they?
Used in precipitation reactions to find out the precipitate.

A
87
Q

In an ionic equation what are the spectator ions?

A

Ions that don’t change during the reaction.

88
Q

When writing ionic equations what is oxidised at what is reduced. (OILRIG)

A

Oxidation is loss of electrons

Reduction is gaining of electrons

89
Q

what is the difference in concentration oh H+ in different pH’s?

A
90
Q

A concentrated solution contains…

A

A lot of dissolved solute per unit volume.

91
Q

A dilute solution contains…

A

Only a small amount of solute.

92
Q

What is the concentration calculation?

A

Concentration (grams per decimetre cubed, g dm^-3) = amount of dissolved (in grams)/volume of solution(dm^-3)

Edexcel GCSE Chemistry (13 decks)

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