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Chemistry > 2 Acids, bases and salt preparations > Flashcards

2 Acids, bases and salt preparations Flashcards

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1
Q

What is a salt?

A

It is a compound formed when a hydrogen is replaced by a metal or ammonium in an acid.

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2
Q

What are three examples of salts?

A
  • Magnesium sulfate.
  • Zinc chloride.
  • Potassium nitrate.
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3
Q

What is hydrochloric acid?

A

An acid.

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4
Q

What is the formula for hydrochloric acid?

A

HCI.

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5
Q

What is an example of a salt with hydrochloric acid?

A

NaCI

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6
Q

What are the names of salts stemmed from hydrochloric acid?

A

Chlorides.

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7
Q

What is nitric acid?

A

An acid.

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8
Q

What is the formula for nitric acid?

A

HNO3

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9
Q

What is an example of a salt with nitric acid?

A

KNO3

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10
Q

What are the names of salts stemmed from nitric acid?

A

Nitrates.

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11
Q

What is sulfuric acid?

A

An acid.

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12
Q

What is the formula for sulfuric acid?

A

H2SO4

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13
Q

What is an example of a salt with sulfuric acid?

A

CuSO4

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14
Q

What are the names of salts stemmed from sulfuric acid?

A

Sulfates.

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15
Q

What is ethanoic acid?

A

An acid.

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16
Q

What is the formula for ethanoic acid?

A

CH3COOH

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17
Q

What is an example of a salt with ethanoic acid?

A

CH3COONa

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18
Q

What are the names of salts stemmed from ethanoic acid?

A

Ethanoates.

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19
Q

What is phosphoric acid?

A

An acid.

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20
Q

What is the formula for phosphoric acid?

A

H3PO4

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21
Q

What is an example of a salt with phosphoric acid?

A

K3PO4.

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22
Q

What is the name of salts stemmed from phosphoric acid?

A

Phosphates.

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23
Q

What is so special about sulfuric acid?

A

It can be thought of as the parent acid of all the sulfates.

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24
Q

What is the parent acid?

A

The acid from which a salt is formed, for example the sulfuric acid is the parent acid of all sulfates.

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25
Q

What happens if the replacement of the hydrogen can’t be done directly?

A

It doesn’t matter.

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26
Q

What is an example of this?

A

You can’t make copper sulfate from copper and dilute sulfuric acid because they don’t react. There are, however, other ways of making it from sulfuric acid - copper sulfate is still a salt.

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27
Q

When are salts also formed?

A

When the hydrogen in an acid is replaced with NH4.

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28
Q

What is it called when the hydrogen in an acid is replaced with NH4?

A

Ammonium salts.
- NH4CI (ammonium chloride)
- (NH4)2SO4 (ammonium sulfate)

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29
Q

What are the different types of reactions of acids?

A
  • Reacting acids with metals.
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30
Q

How do dilute acids react with metals?

A

Depending on their positions in the reactivity series.

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31
Q

What are the ways that dilute acids react?

A
  • Metals below hydrogen in the series don’t react with dilute acids.
  • Metals above hydrogen in the series react to produce hydrogen gas.
  • The higher the metal is in the reactivity series, the more vigorous the reaction.
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32
Q

Why would you never mix metals such as sodium or potassium with acids?

A

Because their reactions are too violent.

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33
Q

What is a summary equation for metals above hydrogen in the reactivity series?

A

Metal + Acid —> Salt + Hydrogen

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34
Q

What are the types of reactions involving magnesium and acids?

A
  • With dilute sulfuric acid.
  • With dilute hydrochloric acid.
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35
Q

What are the reactions with dilute sulfuric acid?

A

There is a rapid fizzing and a colourless gas is evolved, which pops with a lighted sprint (the test for hydrogen).

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36
Q

What happens during this reaction?

A

The reaction mixture becomes very warm as heat is produced.

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37
Q

What does the magnesium gradually disappear to leave?

A

A colourless solution of magnesium sulfate.

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38
Q

What is an equation to show magnesium reacting with dilute sulfuric acid?

A

Mg + H2SO4 —> MgSO4 + H2

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39
Q

What kind of reaction is it between magnesium and dilute sulfuric acid?

A

This is a displacement reaction. The more reactive magnesium has displaced the less reactive hydrogen.

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40
Q

What happens during the reaction of magnesium with dilute hydrochloric acid?

A

The reaction looks exactly the same. The only difference is that this time a solution of magnesium chloride is formed.

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41
Q

What is the equation to show the reaction between magnesium and dilute hydrochloric acid?

A

Mg + 2HCI —> MgCI + H2

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42
Q

What happens to MgSO4?

A

Ionic compounds are present as separate ions in solution so in MgSO4, Mg2+ and the SO42- ions are separated from eachother.

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43
Q

What are the reactions involving zinc and acids?

A

The reactions between zinc and two acids look exactly the same.

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44
Q

Why are the reactions of zinc slower than those of magnesium?

A

The reactions are slower because zinc is lower down the reactivity series that magnesium.

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45
Q

What is the equation for the reaction between zinc and sulfuric acid?

A

Zn + H2SO4 —> ZnSO4 + H2

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46
Q

What is the equation for the reaction between zinc and dilute hydrochloric acid?

A

Zn + 2HCI —> ZnCI2 + H2

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47
Q

What is reacting acids with bases?

A

Metal oxides, such as copper oxide and magnesium oxide, are bases.

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48
Q

What is the reaction between dilute sulfuric acid and copper oxide?

A

The copper oxide (black powder) reacts with dilute sulfuric acid to produce a blue solution of copper sulfate.

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49
Q

What is the equation of reacting dilute sulfuric acid with copper oxide?

A

CuO + H2SO4 —> CuSO4 + H2O

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50
Q

What do all the metal oxide and acid combinations behave like?

A

In the same way as the reaction between copper oxide and sulfuric acid. They produce a salt and a water.

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51
Q

What needs to be present for most of these reactions?

A

Heat.

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52
Q

What is an explanation of the equation above?

A

Coper (II) oxide is an ionic compound containing the O2- ion. What has happened in this reaction is that the H+ ions from the acid have combined with the O2- ions to form water (H2O).

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53
Q

What is the general equation for the reaction of a metal oxide with an acid?

A

Metal oxide + acid —> Salt + Water

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54
Q

What kind of reaction is this?

A

A neutralisation reaction.

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55
Q

How do we know that this is a neutralisation reaction?

A

Because the base neutralises the reaction (water is formed).

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56
Q

What do metal oxides that are soluble in water react and react with it to form?

A

Solutions of metal hydroxides.

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57
Q

What is an example of this reaction?

A

Na2O + H2O —> 2NaOH

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58
Q

Which substances do this reaction?

A

All the group 1 oxides do this reaction, so for potassium oxide.

59
Q

What is the formula to represent this reaction?

A

K2O + H2O —> 2KOH

60
Q

So, which metal oxides are soluble in water?

A
  • Sodium oxide.
  • Potassium oxide.
61
Q

What is said about metal oxides?

A

Most other metal oxides are not soluble in water.

62
Q

How does calcium oxide react with water?

A

It dissolves slightly to form calcium hydroxide.

63
Q

What is the equation to show calcium and oxygen reacting?

A

CaO + H2O —> Ca(OH)2

64
Q

What is another alkali that reacts with water?

A

A solution of ammonia.

65
Q

How does ammonia react with water?

A

To form ammonium ions and hydroxide ions.

66
Q

What is the equation for the reaction with ammonia and water?

A

NH3 + H2O ⇌ NH4+ + OH-

67
Q

What is similar about all of these solutions?

A

All of these solutions contain hydroxide ions.

68
Q

How do we know that these are alkali solutions?

A

Since we can define alkalis as solutions that are a source of hydroxide ions, so all of these solutions are alkalis.

69
Q

In what reactions do metal hydroxides react with acids?

A

Neutralisation reactions.

70
Q

What is the structure of a neutralisation reaction?

A

Metal hydroxide + acid —> Salt + water

71
Q

What does mixing sodium hydroxide and dilute hydrochloric acid form?

A

It produces a colourless solution so not much seems to have happened.

72
Q

How can we tell that something has happened in the reaction?

A

If you repeat the reaction with a thermometer in the beaker, the temperature rises several degrees, showing that there has been a chemical change.

73
Q

What is an equation for this reaction?

A

NaOH + HCI —> NACI + H2O

74
Q

What is the ionic equation for this reaction?

A

OH- + H+ —> H2O

75
Q

How do we know that this is the ionic equation?

A

All neutralisation reactions for an acid reacting with an alkali have the same ionic equation: they all involve the hydroxide ions from the alkali reacting with the H+ ions from the acid to form water.

76
Q

How do carbonates react with cold dilute acids?

A

To produce carbon dioxide gas.

77
Q

What is the equation for acids and carbonates?

A

Carbonate + acid —> Salt + Carbon dioxide + water

78
Q

How does green copper carbonate react with common dilute acids?

A

To give a blue or blue-green solution of copper sulfate, copper nitrate or copper chloride. Carbon dioxide gas is given off.

79
Q

How can you recognise that carbon dioxide has been given off?

A

Because it turns limewater milky.

80
Q

What is special about al of these equations in this reaction?

A

They all have the same form.

81
Q

What is an example of the form that these equations have?

A

CuCO3+H2SO4–>CuSO4 + CO2+H2O
CuCO3+2HNO3–>Cu(No3)2+CO2+H2O
CuCO3+2HCI–>CuCI2+CO2+H2O

82
Q

What is a property of sodium carbonate?

A

Sodium carbonate is soluble in water.

83
Q

What is the equation for the reaction of sodium carbonate with hydrochloric acid?

A

Na2CO3+2HCI–>2NaCI+CO2+H2O

84
Q

What compounds are soluble?

A

All sodium, potassium and ammonium compounds are soluble.

85
Q

What else is soluble?

A

All nitrates.

86
Q

Are most common chlorides soluble?

A

Yes.

87
Q

Which common chlorides aren’t soluble?

A

Lead(II) chloride and silver chloride.

88
Q

Are most common sulfates soluble?

A

Yes.

89
Q

Which common sulfates aren’t soluble?

A
  • Lead(II) sulfate.
  • Barium sulfate.
  • Silver sulfate.
  • Calcium sulfate.
90
Q

Are common carbonates soluble?

A

No, they are insoluble.

91
Q

Which common carbonates are soluble?

A
  • Sodium carbonate.
  • Potassium carbonate.
  • Ammonium carbonate.
92
Q

Are most metal hydroxides soluble?

A

No, they are insoluble or almost insoluble.

93
Q

Which metal hydroxides are soluble?

A
  • Sodium hydroxide.
  • Potassium hydroxide.
  • Ammonium hydroxide.
  • Calcium hydroxide.
94
Q

What are the ways that you could make a soluble salt?

A
  • Acid + metal.
  • Acid + metal oxide or hydroxide.
  • Acid + carbonate.
95
Q

When using the acid + metal method, what do you have to bear in mind?

A

You can only use metals from the moderately reactive metals - from magnesium to iron in the reactivity series.

96
Q

What is the method followed with these mixtures?

A

Whatever mixture you use, the method is basically the same.

97
Q

What is the first step when making copper (II) sulfate crystals?

A

Measure 50cm^3 of dilute sulfuric acid into a beaker and heat it on a tripod and gauze using a bunsen burner.

98
Q

What is the first second when making copper (II) sulfate crystals?

A

Add a spatula full of black copper oxide and continue heating. If the copper oxide disappears add more copper oxide until there is some left in the beaker. Stir the mixture well to make sure that no more will react. At this stage, we have added excess copper oxide.

99
Q

What do we mean by excess copper oxide?

A

There is more than enough copper oxide present to react with all the acid present.

100
Q

How do we know that all the acid has been neutralised?

A

When there is no copper oxide left.

101
Q

What is the third step when making copper (II) sulfate crystals?

A

Filter off the excess copper oxide and transfer the filtrate, which is blue, to an evaporating basin.

102
Q

What is the solution that we have now?

A

Copper sulfate.

103
Q

What is a picture of the apparatus used to make copper sulfate crystals?

A
104
Q

What is the equation for the formation of the solution?

A

CuO + H2SO4 —> CuSO4 + H2O

105
Q

What is the fourth step when making copper (II) sulfate crystals?

A

Heat the solution of copper sulfate over a bunsen burner.

106
Q

Why do we heat the solution?

A

To boil off some of the water and concentrate the solution.

107
Q

What is the fifth step when making copper (II) sulfate crystals?

A

Keep heating until a saturated solution is formed.

108
Q

How do we know if a saturated solution is formed?

A

We can test this by dipping a glass rod into the solution. If crystals form on the glass rod when we remove it we know that the solution is very close to saturated and crystals will also begin to form in the solution.

109
Q

What is the sixth step when making copper (II) sulfate crystals?

A

Stop heating the reaction mixture and allow it to cool slowly at room temperature.

110
Q

Why do we stop heating the reaction mixture and allow it to cool slowly at room temperature?

A

So that larger crystals can form.

111
Q

What is the seventh step when making copper (II) sulfate crystals?

A

Remove the blue crystals from the reaction mixture.

112
Q

How would we remove the blue crystals from the reaction mixture?

A

By filtration, or just pouring off the remaining solution.

113
Q

What is the eighth step when making copper (II) sulfate crystals?

A

The crystals can be dried by blotting them with a paper towel, or they can be left to dry in a warm place.

114
Q

What is a safety precaution that needs to be taken when heating in this reaction?

A

Heating must be very gentle to avoid ‘spitting’ of hot particles.

115
Q

Why can’t we just evaporate the solution to dryness?

A

Evaporating the solution to dryness wouldn’t give you blue copper sulfate crystals. Instead, you would produce a white powder of anhydrous copper sulfate.

116
Q

What happens when many salts form their crystals?

A

Water from the solution becomes chemically bound up with the salt.

117
Q

What is this called?

A

Water of crystallisation.

118
Q

What is a salt which contains water of crystallisation called?

A

Hydrated.

119
Q

What equation shows the crystallisation part of the reaction?

A

CuSO4+5H2O–>CuSO4.5H2O.

120
Q

How can we make magnesium sulfate crystals?

A

We can add excess magnesium to sulfuric acid. This time the acid does not have to be heated.

121
Q

What is the procedure we follow during this reaction?

A

When we add the magnesium the reaction mixture will fizz (hydrogen is given off). We keep adding magnesium until the fizzing stops and there is magnesium left in the beaker. This means that all the acid has reacted.

122
Q

What is the equation for the formation of the solution of magnesium sulfate?

A

Mg+H2SO4–>MgSO4+H2

123
Q

How is the solution concentrated?

A

By heating it and allowing it to crystallise.

124
Q

What is the equation for the crystallisation reaction?

A

MgSO4+7H2O–>MgSO4.7H2O

125
Q

How do you know whether you need to heat the mixture or not?

A

Carbonates react with dilute acids in the cold, and so does magnesium. Most other things that you are likely to come across need to be heated.

126
Q

What do the mixtures need to contain in order to be kept cold?

A
  • Carbonates.
  • Magnesium.
127
Q

What do mixtures need to contain in order to be kept hot?

A

Most other substances.

128
Q

What is an acid in terms of protons?

A

A proton donor.

129
Q

What is a base in terms of protons?

A

A proton acceptor

130
Q

How can this be shown in a formula?

A

H2O+HCI—>H3O + CI

131
Q

What is an explanation of the formula?

A

The HCI donates a proton (H+) to a H2O molecule. So, according to our definition, the HCI is an acid and H2O is a base because it accepts the proton.

132
Q

What substances can act as bases?

A

Metal oxides, metal hydroxides and ammonia can act as bases, and alkalis are bases that are soluble in water.

133
Q

What are examples of soluble metal hydroxides?

A
  • KOH
  • NaOH
  • LiOH
  • RbOH
  • Ba(OH)2
  • NH3
134
Q

What are examples of metal oxides?

A
  • CaO
  • MgO
  • CuO
  • FeO
135
Q

What are examples of metal carbonates?

A
  • Cu(CO3)
  • Ca(CO3)
  • Mg(CO3)
  • Fe(CO3)
136
Q

What are examples of insoluble metal hydroxides?

A
  • CuOH2 [Cu(II)]
  • FeOH2
  • CaOH2
  • MgOH2
137
Q

What is the word equation between an acid and an alkali?

A

Acid + Alkali —> Salt + water

138
Q

What is the word equation between an acid and an insoluble hydroxide?

A

Acid+insoluble hydroxide ->Salt + water

139
Q

What is the word equation between an acid and a metal oxide?

A

Acid + metal oxide —> Salt + water

140
Q

What is the word equation between an acid and metal carbonates?

A

Acid + metal carbonate —> Salt + CO2

141
Q

What is the word equation between an acid and reactive metals?

A

Acid + reactive metals —> Salt + water

142
Q

How do you find the products produced by reactants with acids?

A

The first element goes with the last element. The second element goes with the first element.

143
Q
A

Chemistry (22 decks)

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