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Chemistry Flashcards > 7. Acids, bases and salts > Flashcards

7. Acids, bases and salts Flashcards

1
Q

What pH value do acids have?

A

Acids have pH values of below 7

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2
Q

What property do acids have which makes them dangerous?

A

They’re corrosive

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3
Q

What colour does blue litmus paper turn in acidic conditions?

A

Blue litmus paper turns red

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4
Q

What colour does methyl orange indicator turn in acidic conditions?

A

methyl orange indicator turns red

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5
Q

What can acids do to bases?

A

Acids are substances that can neutralise a base, forming a salt and water

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6
Q

When acids react, what will they form? (in terms of ions)

A

When acids react, they will lose electrons to form positively charged hydrogen ions (H+)

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7
Q

What makes a solution acidic?

A

The presence of H+ ions is what makes a solution acidic

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8
Q

What metals react with dilute acids?

A

Only metals above hydrogen in the reactivity series will react with dilute acids.

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9
Q

What is formed when metals react with acid?

A

When acids react with metals they form a salt and hydrogen gas:
Acid + Metal → Salt + Hydrogen

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10
Q

What type of oxides are metal oxides and metal hydroxides?

A

Metal oxides and metal hydroxides can act as bases

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11
Q

What happens when metal oxides/hydroxides react with acid?

A

When they react with acid, a neutralisation reaction occurs

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12
Q

What is produced by a neutralisation reaction?

A

In all acid-base neutralisation reactions, salt and water are produced
Acid + Base → Salt + Water

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13
Q

What happens when an acid reacts with a metal carbonate? products?

A

Acids will react with metal carbonates to form the corresponding metal salt, carbon dioxide and water:
Acid + Metal Carbonate → Salt + Carbon Dioxide + Water

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14
Q

What pH do bases have?

A

Bases have pH values of above 7

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15
Q

What is an alkali?

A

A base which is water-soluble is referred to as an alkali

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16
Q

What colour does red litmus paper turn in alkaline conditions?

A

In basic (alkaline) conditions red litmus paper turns blue

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17
Q

What colour does methyl orange indicator turn in alkaline conditions?

A

methyl orange indicator turns yellow

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18
Q

In what ways can bases react with acids?

A

Bases are substances which can neutralise an acid, forming a salt and water

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19
Q

In what forms do bases usually appear?

A

Bases are usually oxides or hydroxides of metals

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20
Q

What happens to alkalis when they react? (in terms of ions)

A

When alkalis react, they gain electrons to form negative hydroxide ions (OH–)

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21
Q

What makes a solution alkaline

A

The presence of the OH– ions is what makes the aqueous solution an alkali

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22
Q

What happens to ammonium salts when warmed with an alkali?

A

Ammonium salts undergo decomposition when warmed with an alkali

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23
Q

What makes ammonia dangerous? How can this problem be fixed?

A

Even though ammonia is itself a weak base, it is very volatile and can easily be displaced from the salt by another alkali

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24
Q

What is produced in the reaction between alkalis and ammonium salts?

Give an example equation between ammonium chloride and sodium hydroxide

A

A salt, water and ammonia are produced
Example:

NH4Cl + NaOH →NaCl + H2O + NH3

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25
Q

What is the reaction between ammonium chloride and sodium hydroxide used for?

A

This reaction is used as a chemical test to confirm the presence of the ammonium ion (NH4+)

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26
Q

How does the test for ammonia work?

A

Alkali is added to the substance with gentle warming followed by the test for ammonia gas using damp red litmus paper

The litmus paper will turn from red to blue if ammonia is present

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27
Q

What is the pH scale?

A

The pH scale is a numerical scale which is used to show how acidic or alkaline a solution is

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28
Q

From what scale does the pH scale range?

A

0-14

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29
Q

What does it mean if the pH value of an acid is very low?

A

The lower the pH then the more acidic the solution is

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30
Q

What does it mean if the pH value of an alkali is very high?

A

The higher the pH then the more alkaline the solution is

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31
Q

What does it mean if a substance has a pH of 7?

A

A solution of pH 7 is describe as being neutral e.g. water

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32
Q

What type of indicator can be used to measure pH?

A

Universal indicator is a mixture of different indicators which is used to measure the pH

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33
Q

How is universal indicator used?

A

A drop is added to the solution and the colour is matched with a colour chart which indicates the pH which matches specific colours

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34
Q

Why is soil pH analysed?

A

Soil pH is analysed to indicate the acidity or alkalinity of soil

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35
Q

What PH’s do most plants favour?

A

Most plants favour a pH value of between 5 and 8

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36
Q

What happens if the soil pH is not ideal for the plant?

A

Changes in soil which cause a pH to be outside this range adversely affect plant processes resulting in reduced growth and crop yield

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37
Q

How may soils become acidic?

A

Soils may become acid from acid rain, overuse of fertilisers which contain ammonium salts or by the excessive breakdown of organic matter by bacteria

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38
Q

How can soil be neutralised?

A

Crushed or powdered limestone (calcium carbonate) or lime (calcium oxide) or slaked lime (calcium hydroxide) is added to neutralise the excess acidity in the soil

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39
Q

Why must the process in which soil is neutralised be monitored?

A

The addition process must be carefully monitored though, as if added in excess, further damage could be done if the pH goes too high

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40
Q

What are acids? (in terms of protons) Why?

A

Acids are proton donors as they ionize in solution producing protons, H+ ions

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41
Q

What are alkalis? (in terms of protons) Why?

A

Bases (alkalis) are proton acceptors as they ionize in solution producing OH– ions which can accept protons

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42
Q

What determines whether an acid or base is strong or weak?

A

Acids and alkalis can be either strong or weak, depending on how many ions they produce when dissolved in water

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43
Q

What determines a strong acid or alkali?

A

Strong acids and bases ionize completely in water, producing solutions of very low pH for an acid or very high pH for a base

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44
Q

What are examples of strong acids and bases?

A

Strong acids include HCl and H2SO4 and strong bases include the Group I hydroxides

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45
Q

What determines a weak acid or base?

A

Weak acids and bases partially ionize in water and produce pH values which are closer to the middle of the pH scale

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46
Q

What are examples of weak acids?

A

Weak acids include organic acids such as ethanoic acid, CH3COOH

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47
Q

What are examples of weak bases?

A

weak bases include aqueous ammonia

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48
Q

What is usually set-up for both weak acids and bases once they’re added to water?

A

For both weak acids and bases, there is usually an equilibrium set-up between the molecules and their ions once they have been added to water

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49
Q

Give an example for the ions forming aqueous ammonia

A

NH3 + H2O ⇌ NH4+ + OH-

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50
Q

In the example for aqueous ammonia and its ions, to which direction does the equilibrium lie and why?

A

In both cases the equilibrium lies to the left, indicating a high concentration of intact acid / base molecules, with a low concentration of ions in solution

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51
Q

What determines if a solution of an acid or base is concentrated?

A

A concentrated solution of either an acid or a base is one that contains a high number of acid or base molecules per dm3 of solution

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52
Q

Is a concentrated acid strong?

A

NO
It does not necessarily mean that the acid or base is strong though, as it may be made from a weak acid or base which does not dissociate completely

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53
Q

Do acidic and basic oxides have the same properties?

A

NO

Acidic and basic oxides have different properties and values of pH

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54
Q

What determines the pH of an oxide?

A

The difference in their pH stems from whether they are bonded to a metal or a nonmetal element

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55
Q

What does the metallic character influence? (oxides)

A

The metallic character of the element influences the acidic or alkaline behaviour of the molecule

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56
Q

When are acidic oxides formed?

A

Acidic oxides are formed when a nonmetal element combines with oxygen

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57
Q

What happens when an acidic oxide is dissolved in water?

A

When dissolved in water they produce an acidic solution with a low pH

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58
Q

What happens when an acidic oxide reacts with a base?

A

They react with bases to form a salt and water

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59
Q

What are common examples of acidic oxides?

A

Common examples include SO2 and SiO2

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60
Q

When are basic oxides formed?

A

Basic oxides are formed when a metal element combines with oxygen

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61
Q

What happens when a basic oxide is dissolved in water?

A

When dissolved in water they produce a basic solution with a high pH

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62
Q

What happens when a basic oxide reacts with an acid?

A

They react with acids to form a salt and water

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63
Q

What are common examples of basic oxides?

A

Common examples include NaOH, KOH and Ca(OH)2

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64
Q

What are neutral oxides?

A

Some oxides do not react with either acids or bases and thus are said to be neutral

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65
Q

What are examples of neutral oxides?

A

Examples include N2O, NO and CO

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66
Q

What are amphoteric oxides?

A

Amphoteric oxides are a curious group of oxides that can behave as both acidic and basic, depending on whether the other reactant is an acid or a base

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67
Q

What is formed when an amphoteric oxide reacts with an acid or a base?

A

In both cases a salt and water is formed

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68
Q

What are examples of amphoteric oxides?

A

Two most common amphoteric oxides are zinc oxide and aluminum oxide

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69
Q

Do the hydroxides of zinc and aluminium also react amphoterically?

A

YES

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70
Q

What is a salt?

A

A salt is a compound that is formed when the hydrogen atom in an acid is replaced by a metal

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71
Q

How can salts be used?

A

These uses include fertilisers, batteries, cleaning products, healthcare products and fungicides

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72
Q

How many parts does the name of a salt have?

A

The name of a salt has two parts

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73
Q

Where does the first part of a salt name come from?

A

The first part comes from the metal, metal oxide or metal carbonate used in the reaction

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74
Q

Where does the second part of the salt name come from?

A

The second part comes from the acid

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75
Q

how can the name of a salt be determined?

A

The name of the salt can be determined by looking at the reactants

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76
Q

What are two key things to consider when preparing salts?

A

Is the salt being formed soluble or insoluble in water?
- Is there water of crystallisation present in the salt crystals?

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77
Q

Are sodium, potassium and ammonium salts soluble?

A

Yes, all of them are

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78
Q

Are nitrates soluble?

A

Yes, all of them are

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79
Q

Are ethanoates soluble?

A

Yes, all of them are

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80
Q

Are chlorides soluble?

A

Most of them,
Exceptions include:
Silver and Lead(II)

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81
Q

Are sulfates soluble?

A

Most of them,
Exceptions include:
Barium, Calcium and Lead (II)

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82
Q

Are carbonates soluble?

A

Most of them are INSOLUBLE,
Exceptions include:
Sodium, potassium and ammonium

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83
Q

Are hydroxides soluble?

A

Most of them are INSOLUBLE,
Exceptions include:
Sodium, potassium and calcium (calcium hydroxide is slightly soluble)

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84
Q

8.2.1 look at methods of salt preparation

A

:)

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85
Q

Alkali ions

A

OH-

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86
Q

Acid ions

A

H+

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87
Q

pH of pure water

A

pH 7

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88
Q

Salt

A

A compound formed when some or all of the hydrogen in an acid is replaced by a metal.

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89
Q

Acid + Metal ->

A

Salt + Hydrogen

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90
Q

Acid + Base ->

A

Salt + Water

Neutralisation reaction

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91
Q

Acid + Base ->

A

Salt + Water

Neutralisation reaction

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92
Q

Acid + Alkali ->

A

Salt + Water

Neutralisation reaction

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93
Q

Precipitate

A

An insoluble solid formed by a reaction taking place in a solution.

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94
Q

How are precipitation reactions used?

A

To remove pollutants from the waste water produced by factories.
To remove metal ions from industrial waste water.
Remove unwanted ions from drinking water.

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95
Q

Acid + Metal Carbonate ->

A

Salt + Water + CO2

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96
Q

Test for CO2

A

Limewater solution.

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97
Q

How to carry out a Titration

A

Measure a known volume of alkali into a flask using a volumetric pipette. Measure from the bottom of the Meniscus.
Add a few drops of indicator (thymolphthalein- Blue in alkali, colourless in acid)
Pour acid into a Burette. Drop into alkali until alkali changes colour.
Measure how much acid it took, an repeat until you get two identical results.

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98
Q

Where does the alkali go in a Titration?

A

The flask.

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99
Q

sums to remember

A

conc = mol/ vol and mol = mass/ Mr

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100
Q

All salts of group I

A

soluble

101
Q

All ammonium salts

A

soluble

102
Q

All nitrates

A

soluble

103
Q

All nitrates

A

soluble

104
Q

Most halides

A

soluble

105
Q

Silver and lead halides

A

insoluble

106
Q

Group I hydroxides/carbonates

A

soluble

107
Q

Most hydroxides/carbonates

A

insoluble

108
Q

Group I & II oxides in water

A

soluble

109
Q

Most metal oxides

A

insoluble

110
Q

What is the role of the pH scale?

A

pH scale is used to show the acidity or alkalinity of a solution

111
Q

What is an acid? (2)

A

Substance that form hydrogen ions when dissolved in water

proton donor

112
Q

metal + acid →

A

salt + hydrogen

113
Q

alkali + acid →

A

salt + water

114
Q

What type of reaction is an metal + acid reaction?

A

redox reaction

115
Q

metal hydroxide + acid →

A

salt + water

116
Q

metal carbonate + acid →

A

salt + water + carbon dioxide

117
Q

What is a base that is soluble in water?

A

Alkali

118
Q

acid + base →

A

salt + water

119
Q

Ammonia salts are much more _ than metal salts

A

volatile

120
Q

alkali + ammonium salt →

A

metal salt + ammonia + water

121
Q

What happens when acids react with a metal oxides?

A

When acids react with metals they form a salt and hydrogen gas:
Acid + Metal oxides → Salt + Hydrogen.

122
Q

What happens when acids react with bases?

A

In all acid-base neutralisation reactions, salt and water are produced:

Acid + Base → Salt + Water.

123
Q

What happens when acids react with metal carbonates?

A

Acids will react with metal carbonates to form the corresponding metal salt, carbon dioxide and water:

Acid + Metal Carbonate → Salt + Carbon Dioxide + Water.

124
Q

Describe the effect on litmus, thymolphthalein and methyl orange in acidic conditions.

A

In acidic conditions, blue litmus paper turns red, thymolphthalein turns colourless and methyl orange indicator turns red.

125
Q

What are the three important properties of acids?

A

Acids have pH values of below 7, have a sour taste (when edible) and are corrosive.

126
Q

What are acids?

A

Acids are substances that will lose electrons to form positively charged hydrogen ions (H+ also called protons) when dissolved in water.

127
Q

What is an indicator?

A

A substance which changes color when added to acidic or alkaline solutions.

128
Q

What is a base?

A

Bases are substances which can neutralise an acid, forming a salt and water.

129
Q

What is an alkali?

A

An alkali is a soluble base.

130
Q

Describe the effect on litmus, thymolphthalein and methyl orange in basic (alkaline) conditions?

A

In basic (alkaline) conditions red litmus paper turns blue, thymolphthalein turns blue and methyl orange indicator turns yellow.

131
Q

What four substances can bases be?

A

Bases can be metal oxides, metal hydroxides, ammonia or carbonates of metals.

132
Q

What is a neutralisation reaction?

A

When a base reacts with an acid to form a salt we call the reaction a neutralization reaction.

133
Q

What do acids and alkalis produce in aqueous solutions?

A

Acids produce H+ ions in aqueous solutions.
Alkalis produce OH- ions in aqueous solutions.

134
Q

What does the pH scale measure and describe neutrality, acidity, and alkalinity through whole numbers?

A

The pH scale (0 to 14) measures the acidity or alkalinity of a solution, and can be measured using a universal indicator:

The lower the pH then the more acidic the solution is.
A solution with a pH of 7, such as water, is described as being neutral.
The higher the pH then the more basic the solution is.

135
Q

Soil may become acidic after a number of years. This can be due to:
Give three examples.

A

Acid rain.
Bacteria and fungi rotting the vegetation so that it releases acids.
Use of fertilizers containing ammonium salts.

136
Q

What is used to neutralize excess acidity in soil?

A

Crushed limestone (calcium carbonate) or lime (calcium oxide) are added to neutralise excess acidity in the soil.

137
Q

Describe the importance of controlling acidity in soil?

A

If the pH of the soil is too acidic or too basic this would mean that crops would be unable to grow well.

138
Q

What are acids in terms of proton transfer?

A

Acids are proton donors as they ionise in solution producing protons, which are H+ ions.

NOTE - These H+ ions make the aqueous solution acidic.

139
Q

What are bases in terms of proton transfer?

A

Bases (alkalis) are proton acceptors as they ionise in solution producing OH- ions which can accept protons.

NOTE - These OH- ions make the aqueous solution alkaline.

140
Q

Describe the meaning of strong acids.

A

Strong acids ionise completely in water, producing solutions of very low pH for an acid.

141
Q

Describe the meaning of strong bases.

A

Strong bases ionise completely in water producing solutions of very high pH for a base.

142
Q

Describe the meaning of weak acids.

A

Weak acids partially ionise in water and produce pH values which are closer to the middle of the pH scale.

143
Q

Describe the meaning of weak bases.

A

Weak bases partially ionise in water and produce pH values which are closer to the middle of the pH scale.

144
Q

We can tell if an acid is strong or weak by measuring its electrical conductivity, pH and rate of reaction with metals or metal carbonates:

A

A strong acid conducts much better than a weak acid of the same concentration.
A strong acid has a lower pH than weak acid of the same concentration.
A strong acid reacts faster than a weak acid.

145
Q

We can tell is an acid is strong or weak by measuring its electrical conductivity, pH and rate of reaction with metals or metal carbonates.
What are the reasons for these differences?

A

This is because there is a greater concentration of hydrogen ions in the strong acid compared with the weak acid.

146
Q

Compared with strong bases, weak bases have:

A

A lower electrical conductivity.
A less alkaline (lower) pH.
A slower rate of reaction.

147
Q

What is a universal indicator?

A

A universal indicator is a mixture of different indicators which is used to measure the pH.

148
Q

What are oxides?

A

Oxides are compounds of metal or non-metals.

149
Q

What are the four types of oxides?

A

Acidic oxides.
Neutral oxides.
Amphoteric oxides.
Basic oxides.

150
Q

When are basic oxides formed?

A

Basic oxides are formed when a metal element combines with oxygen

151
Q

What happens when a metal reacts with oxygen (basic oxide reaction)?

A

Metal + oxygen → salt.

152
Q

What happens when basic oxides are dissolved in water?

A

When dissolved in water they produce a basic solution with a high pH.

153
Q

Give three examples of basic oxides.

A

CuO - Copper oxide.
CaO - Calcium oxide.
BaO - Barium oxide.
MgO - Magnesium oxide.
Fe₂O₃ - Iron (III) oxide.

154
Q

When are acidic oxides formed?

A

Acidic oxides are formed when a non-metal element combines with oxygen.

155
Q

What happens when basic oxides react with acid?
What happens when acidic oxides react with bases?

A

Basic oxides + acid → salt + water.
Acidic oxides + base → salt + water.

156
Q

What happens when acidic oxides are dissolved in water?

A

When dissolved in water they produce an acidic solution with a low pH.

157
Q

Give three examples of acidic oxides.

A

SO₂ - Sulfur dioxide.
CO₂ - Carbon dioxide.
P₂O5 - Phosphorus pentoxide.
SO₃ - Sulfur trioxide.
NO₂ - Nitrogen dioxide.

158
Q

What are neutral oxides?

A

Neutral oxides do not react with acids or bases.

159
Q

Give three examples of neutral oxides.

A

N₂0 - Nitrous Oxide.
NO - Nitrogen monoxide.
CO - Carbon monoxide.

160
Q

What are amphoteric oxides?

A

Amphoteric oxides are a curious group of oxides that can behave as both acidic and basic, depending on whether the other reactant is an acid or a base.

NOTE - In both cases, a salt and water is formed.

161
Q

Give two examples of amphoteric oxides.

A

ZnO - Zinc oxide.
Al2O3 - Aluminium oxide.

162
Q

What are the four common laboratory acids?

A

Hydrochloric acid - HCl.
Sulfuric acid - H₂SO₄.
Nitric acid - HNO₃.
Phosphoric acid - H₃PO₄

163
Q

What makes an acidic solution acidic?

A

All acids form hydrogen ions (H+) when dissolved in water, it is the hydrogen ions that make a solution acidic.

164
Q

What are three common laboratory bases?

A

Sodium hydroxide - NaOH.
Calcium hydroxide - Ca(OH)₂.
Ammonia - NH₃.

165
Q

What do alkalis form when dissolved in water?

A

Alkalis form hydroxide ions (OH-) when they dissolve in water.

166
Q

What is a salt?

A

A salt is a compound that is formed when the hydrogen atom in an acid is replaced by a metal/an ammonium group (NH₄).

167
Q

What happens when an acid reacts with a metal hydroxide?

A

Metal hydroxide + acids → salt + water.

168
Q

When is a hydrogen ion formed?

A

A
A hydrogen ion is formed by the removal of the single electron from a hydrogen atom.

169
Q

What are the four ways of making salts?

A

Reacting a metal with an acid.
Reacting an insoluble base with an acid.
Neutralising an alkali with an acid by the titration method.
By precipitation.

170
Q

How do you make a salt from an insoluble base (3)?

A

add excess base to the acid.
filter to remove any unreacted base that’s been added.
heat the solution to evaporate the water, allowing crystals of the salt to form.

171
Q

How do you make a salt from an soluble base (titration is the making of a soluble salt from a soluble base and acid) (7)?

A

Measure the alkali into the titration flask using a volumetric pipette.
Add a few drops of indicator solution to the alkali in the flask.
Fill a clean burette with acid.
Record the burette reading.
Open the burette tap and let the acid flow into the flask.
Keep adding acid slowly until the indicator changes color.
Record the reading on the burette.

172
Q

How do we make a salt from metals (6)?

A

Add the metal to the acid in the flask so that the metal is in excess.
Warm the flask gently to complete the reaction.
Filter off the excess metal.
Put the filtrate into an evaporating basin and evaporate the water until the crystalisation point is reached.
Filter off the crystals and wash them with distilled water.
Dry the crystals between sheets of filter paper.

173
Q

What is a titration?

A

A titration is used to make a soluble salt from an acid.

To conduct a titration both acid and alkali must be soluble.

174
Q

What are the salts made by the titration method included in?

A

Salts made by the titration method include salts of Group 1 elements and ammonium salts.

175
Q

What is a precipitate?

A

The solid obtained when solutions of two soluble compounds are mixed is called a precipitate.

176
Q

What are the 7 soluble compounds?

A

All salts of Group 1 elements.
All nitrates.
All ammonium salts.
Most chlorides, bromides and iodides (halides).
Most sulfates.
Group I hydroxide and carbonates are soluble.
Group I and II oxides react with water.

177
Q

What are the 4 insoluble compounds (precipitation)?

A

Chlorides, bromides and iodides of silver and lead.
Sulfates of calcium, barium and lead.
Most hydroxide and carbonates.
Most metal oxides.

178
Q

How do we make an insoluble salt (precipitation)?

A

making insoluble salts:
- mix the two solutions that will form the salt.
- filter to remove the solid insoluble salt.
- wash salt with distilled water.
- leave salt to dry on filter paper.

179
Q

What are spectator ions?

A

The ions that do not take part in the reaction are called spectator ions.

180
Q

Decribe the test for ammonia.

A

Turns damp red litmus paper blue.

181
Q

Describe the test for carbon dioxide.

A

Bubble the gas through the limewater and it will turn milky (cloudy)

182
Q

Describe the test for chlorine gas?

A

When damp litmus paper is put into chlorine gas the litmus paper is bleached and turns white.

183
Q

Describe the test for hydrogen gas.

A

Use a burning splint held at the open end of a test tube of the gas.
▪ Creates a ‘squeaky pop’ sound.

184
Q

Describe the test for oxygen gas.

A

Uses a glowing splint inserted into a test tube of the gas.
▪ Splint relights in oxygen.

185
Q

Describe the test for sulfur dioxide.

A

Use aqueous potassium manganate(VII) and there will be a colour change from purple to colourless.

186
Q

What is the formula for percentage composition?

A

% composition = Ar (X) ÷ Mr (XY) x 100.

187
Q

What is a saturated solution?

A

A solution in which no more solute will dissolve.

188
Q

What is an acid?

A

Proton donor

HCl dissociates (breaks apart) in water to give H+ ions

189
Q

What is a base?

A

A proton acceptor

190
Q

What is an alkali?

A

An alkali is a soluble base which dissociates in water making an OH- ion

Example NaOH is a soluble base, it dissociates into Na+ and OH- in water

191
Q

Name three common acids

A

Hydrochloric acid

HCl

Sulphuric acid

H2SO4

Nitric acid

HNO3

192
Q

Name three common alkali.

A

sodium hydroxide

NaOH

Potassium hydroxide

KOH

Ammonium hydroxide

NH4OH

193
Q

What is the chemical formula for hydrochloric acid?

A

HCl

194
Q

What is the chemical formula for sulphuric acid?

A

H2SO4

195
Q

What is the chemical formula for nitric acid?

A

HNO3

196
Q

What is the chemical formula for carbonic acid?

A

H2CO3

197
Q

Complete the general equation

Acid + Alkali –>

A

Acid + Alkali –> Salt + Water

198
Q

Explain how an alkali can neutralise an acid.

A

You need to add an indicator such as thymolphthalein to a sample of the alkali. It will turn blue.

Add small drops of the acid using a pipette until one drop turn the solution from pink to colourless.

You now have equal numbers of H+ ions and OH- ions making H2O or water

199
Q

Name three bases

A

Copper oxide

CuO

Aluminium oxide

Al2O3

Copper hydroxide

Cu(OH)2

200
Q

What colour is methyl orange in acid and alkali?

A

https://www.google.co.uk/search?sa=G&hl=en-GB&q=methyl+orange+in+alkali&tbm=isch&tbs=simg:CAQSlgEJWz3N6x9eNpoaigELEKjU2AQaBAgICAoMCxCwjKcIGmEKXwgDEifvBq0ChgGHAawCqgKdAZIB5wMKyTSOJ58o5zS1KO02zSGrJ8g0nSAaMI2JhdVCfe4ww-KXkTV2fPsc3WJmrVKc5ng0PtdEvmoXgq–OHHrQIs3KbCDynaetyAEDAsQjq7-CBoKCggIARIEtLIVuQw&ved=0ahUKEwiy_Z7ohpvUAhXKLcAKHWm4B7oQwg4IIygA

acid - red

alkali- yellow

201
Q

Finish the general equation

Acid + metal carbonate –>

A

Spot the carbonate!

Think neutralisation + carbon dioxide

Acid + metal carbonate –> Salt + water + carbon dioxide

202
Q

Finish the general equation

Acid + metal carbonate –>

A

Spot the carbonate!

Think neutralisation + carbon dioxide

Acid + metal carbonate –> Salt + water + carbon dioxide

203
Q

What colour is thymolphthalein in acid and alkali?

A

Acid - colourless

Alkali- blue

204
Q

What colour is litmus in acid and alkali?

A

Acid- red

Alkali- blue

205
Q

What colour is univeral indicator in strong acid, weak acid, neutral, weak alkali and strong alkali?

A

strong acid- red

weak acid- yellow

neutral- green

weak alkali- blue

strong alkali- purple

206
Q

Name a strong acid and strong alkali

A

strong acid- HCl - stomach acid pH 2

strong alkali - NaOH - pH 14

207
Q

Name a weak acid and alkali

A

weak acid - carbonic acid

weak alkali - ammonia

208
Q

Name a neutral substance

A

water- universal indicator turns green

209
Q

Finish the reaction

HCl + NaOH –>

A

This is an acid + alkali - think neutralisation!

Salt + water!

HCl + NaOH –> NaCl + H2O

210
Q

Finish the reaction

H2SO4 + KOH –>

A

This is an acid + alkali - think neutralisation

salt + water

remember a salt is metal/non-metal or cation/anion

H2SO4 (aq) + 2KOH(aq) –> K2SO4 (aq) + 2H2O (l)

don’t forget to balance it!

211
Q

Finish the general reaction

Acid + base –>

A

acid + base –> salt + water

212
Q

How do you spot an acid from its chemical formulae?

A

All acids have a hydrogen atom at the front of the chemical formula

HCl

H2SO4

H2CO3

HNO3

213
Q

How do you spot a base from its chemical formulae?

A

The chemical formula would end with an oxide, hydroxide or carbonate

CuO

Mg(OH)2

Na2CO3

214
Q

What will the products be in this reaction?

HNO3 + CuO –>

A

This is an acid + base- think neutralisation

salt + water

2HNO3(aq) + CuO(s) –> Cu(NO3)2 (aq) + H2O(l)

Think of your solubility rules to help figure out the state symbols

All oxides are insoluble except for Na, K or NH4+ - therefore CuO (s)

All nitrate salts are soluble- therefore Cu(NO3)2 (aq)

215
Q

What will the products be?

HNO3 + CaCO3 –>

A

Spot the carbonate!

carbonate + acid - fizzing and carbon dioxide made!

2HNO3(aq) + CaCO<strong>3</strong>(s) –> Ca(NO3)2(aq) + H2O(l) + CO<strong>2</strong>(g)

Ca(NO3)2 is soluble - all nitrates are soluble

CaCO3 is insoluble- all carbonates are insoluble except for Na, K and NH4+

216
Q

What are the products?

H2SO4 + MgCO3 –>

A

Spot the carbonate + acid?

Think neutralisation with carbon dioxide

H2SO4(aq) + MgCO3(s) –>MgSO4(aq) + H2O(l) + CO2(g)

MgCO3 is insoluble

All Carbonates are insoluble except for Na, K and NH4+

MgSO4 is soluble (aq)

All sulfates are soluble except for Pb and Ba

217
Q

Complete the general equation

Metal + Acid –>

A

Think fizzing

Metal + acid –> salt + hydrogen

The metal must be more reactive than hydrogen in the reactivitiy series (copper, silver, gold and platinum will not react with acid)

218
Q

What products will form?

Mg + HCl –>

A

Think fizzing and spot the hydrogen in the acid- what is left is a salt

Mg(s) +2 HCl(aq) –> MgCl2(aq) + H2(g)

HCl is aqueous- all acids are aqueous

MgCl2 is aqueous- all halides are soluble except for Pb & Ag

219
Q

Name the products

Ca + H2SO4 –>

A

A
Think fizzing and spot hydrogen

Ca(s) + H2SO4(aq) –>CaSO4(aq) + H2(g)

Hydrogen is diatomic- H2

220
Q

Name all the diatomic elements

A

H2 , N2 , O2, Cl2, Br2, I2, F2

221
Q

Name the three oxides formed when petrol is burnt in a car engine

A

Sulfur in fuel reacts with oxygen to form SO2

Nitrogen in air reacts with oxygen to form NO2

Carbon in fuel reacts with air to for CO2

222
Q

State two environmental impact of acid rain?

A

Acid rain lowers the pH of lakes and streams and aquatic life dies

Acid rain leaches minerals from the soil and trees die

223
Q

The following occurs in a car engine

Sulfur in fuel reacts with oxygen to form SO2

Nitrogen in air reacts with oxygen to form NO2

Carbon in fuel reacts with air to for CO2

What happens with all these non-metal oxides dissolve in the rain?

A

Non-metal oxide form acidic solution in water

SO2 –> H2SO4

NO2 –> HNO3

CO2 –> H2CO3

224
Q

What is an acid a source of?

A

Hydrogen ions

225
Q

When dissolved in water, acids always produce…

A

H+ ions

226
Q

Acids always contain… in their formula

A

H

227
Q

Bases are known as an ….. if they are soluble in water

A

alkali

228
Q

A base is a …… source

A

hydroxide ion

229
Q

bases are metal ……., metal…….. and metal……

A

oxides, hydroxides, carbonates

230
Q

When dissolved in water bases always produce…

A

OH- ions

231
Q

What is neutralisation?

A

H+ + OH- -> H2O

232
Q

acid + metal ->

A

salt

233
Q

acid + metal oxide ->

A

salt + water

234
Q

acid + metal carbonate ->

A

salt + water + carbon dioxide

235
Q

SNAP =

A

All sodium, nitrate, ammonium and potassium salts are soluble

236
Q

Cl(a)SPbAg =

A

Chlorides are soluble except for lead and silver

237
Q

SolSul CaBaL =

A

Soluble sulfates except calcium, barium and lead

238
Q

InCH =

A

insoluble carbonates and hydroxides (except for snap salts)

239
Q

What is the range of the Ph scale?

A

0-14

240
Q

What is the colour change of the Ph scale from acidic to alkali?

A

red - orange - green - blue - purple

241
Q

What colour does red litmus turn in the presence of acids and bases?

A

acid - red

base - blue

242
Q

What colour change can you observe in thymolphthalein?

A

acid - colourless

base - blue

243
Q

What colour change can you observe in methyl orange?

A

acid - red

base - yellow

244
Q

Define an acid and an alkali

A

ACID = A proton or hydrogen donor

ALKALI = A proton or hydrogen accepter

245
Q

Difference between an alkali and a base?

A

Alkali is a base that is soluble in water

246
Q

Example of:

1 - Strong acid
2 - Weak acid
3 - Strong alkali
4 - Weak alkali

A

1 - Stomach acid = HCl (pH 1)
2 - Ethanoic acid (CH3COOH)
3 - Bile (from the gall bladder)
4 - Ammonia, tooth paste

247
Q

Weak acid reactions are often what?

Give an example.

A

They’re reversible.

Ethanoic acid Ethanoate ion + Hydrogen ion
CH3COOH -> CH3COO^- + H^+

248
Q
A

Chemistry Flashcards (11 decks)

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