w
w
w
.s
m
ar
te
du
h
ub
.
co
m
A
C
I
D
S
126
B
A
S
E
S
&
S
A
L
T
S
126
127
A
It reacts with a carbonate to form carbon dioxide.
B
It reacts with an acid to form a salt.
C
It reacts with an ammonium salt to form ammonia.
D
It turns universal indicator paper blue.
0620/13/O/N/15
co
m
17 Which property is not characteristic of a base?
ub
.
18 Zinc sulfate is a soluble salt and can be prepared by reacting excess zinc carbonate with dilute
sulfuric acid.
Which piece of equipment would not be required in the preparation of zinc sulfate crystals?
A
beaker
B
condenser
C
evaporating dish
D
filter funnel
w
w
w
.s
m
ar
te
du
h
0620/13/O/N/15
127
128
15 Element X is in Group I of the Periodic Table.
Which row shows the type of oxide and whether element X is metallic or non-metallic?
A
acidic
metallic
B
acidic
non-metallic
C
basic
metallic
D
basic
non-metallic
0620/13/O/N/15
co
m
metallic or
non-metallic
ub
.
type of oxide
16 Three liquids, P, Q and R, are added to a mixture of hydrochloric acid and Universal Indicator
solution.
te
du
h
0620/13/O/N/15
The following observations are made.
P
the colour of the indicator turns purple.
Q
the colour of the indicator does not change.
R
there is effervescence and the indicator turns blue.
P
ar
What are P, Q and R?
Q
R
sodium carbonate
solution
water
sodium hydroxide
solution
B
sodium hydroxide
solution
water
sodium carbonate
solution
C
water
sodium carbonate
solution
sodium hydroxide
solution
water
sodium hydroxide
solution
sodium carbonate
solution
w
.s
m
A
w
w
D
128
129
16 A white solid is insoluble in water.
When it is added to hydrochloric acid, bubbles of gas are formed.
Adding aqueous ammonia to the solution formed gives a white precipitate. Adding excess
aqueous ammonia causes the precipitate to re-dissolve.
0620/11/O/N/15
aluminium nitrate
B
ammonium nitrate
C
calcium carbonate
D
zinc carbonate
17 Which property is not characteristic of a base?
It reacts with a carbonate to form carbon dioxide.
B
It reacts with an acid to form a salt.
C
It reacts with an ammonium salt to form ammonia.
D
It turns universal indicator paper blue.
0620/11/O/N/15
te
du
h
A
ub
.
A
co
m
What is the white solid?
18 Four stages in the preparation of a salt from an acid and a solid metal oxide are listed.
Add excess solid.
2
Evaporate half the solution and leave to cool.
3
Filter to remove unwanted solid.
4
Heat the acid.
0620/11/O/N/15
.s
m
ar
1
In which order should the stages be carried out?
A
B
2→1→3→4
4→1→3→2
w
C
1→3→4→2
4→2→1→3
w
w
D
129
19 Aqueous sodium hydroxide is added to two different solutions with the results shown.
0620/01/M/J/07
Y
co
m
X
green precipitate formed
light blue precipitate formed
Y
A
copper(II)
iron(II)
B
copper(II)
iron(III)
C
iron(II)
copper(II)
D
iron(III)
copper(II)
te
du
h
X
ub
.
What are the cations present in X and Y?
20 In which experiment does the limewater not turn milky?
ar
A
acid
130
.s
m
limewater
0620/01/M/J/07
B
suction
pump
limewater
ethanol
D
C
w
w
w
magnesium carbonate
acid
limewater
iron filings
limewater
130
131
21 Two indicators, bromophenol blue and Congo red, show the following colours in acidic solutions
and in alkaline solutions.
0620/01/M/J/07
acid
alkali
bromophenol blue
yellow
blue
Congo red
violet
red
co
m
indicator
A few drops of each indicator are added to separate samples of a solution of pH 2.
What are the colours of the indicators in this solution?
in a solution of pH 2
Congo red is
A
blue
red
B
blue
violet
C
yellow
red
D
yellow
te
du
h
ub
.
bromophenol blue is
violet
22 Aqueous lead(II) nitrate is added to a solution containing iodide ions. Lead(II) iodide is formed.
0620/01/M/J/07
neutralisation
B
oxidation
C
precipitation
D
reduction
.s
m
A
ar
Which type of reaction takes place?
0620/01/M/J/07
w
w
w
23 The diagram shows an outline of part of the Periodic Table.
W
X
Y
Z
Which two elements could form a covalent compound?
A
W and X
B
W and Y
C
X and Y
D
X and Z
131
24 Which substances react with aqueous potassium bromide to form bromine?
iodine
A
B
C
D
0620/01/M/J/07
co
m
chlorine
132
0620/01/M/J/07
27 The diagram shows the properties of four substances.
ub
.
Which one could be magnesium?
Does it bend or break easily?
breaks
te
du
h
bends
Does it react with dilute
hydrochloric acid?
yes
A
Does it react with dilute
hydrochloric acid?
no
yes
no
B
C
D
34 The diagram shows an experiment in which ammonia is released.
ar
0620/01/M/J/07
damp
litmus paper
.s
m
Which line in the table is correct?
ammonia
w
w
w
mixture of solution X
and
aqueous ammonium sulphate
heat
solution X
final colour of litmus paper
A
aqueous sodium hydroxide
blue
B
aqueous sodium hydroxide
red
C
dilute sulphuric acid
blue
D
dilute sulphuric acid
red
132
133
14 Why does the powdering of calcium carbonate increase the speed of its reaction with an acid?
It increases the mass of calcium carbonate.
B
It increases the surface area of the calcium carbonate.
C
The powder becomes more concentrated.
D
The powder floats on top of the acid.
15 Which process does not involve either oxidation or reduction?
burning methane in the air
B
extracting iron from hematite
C
heating copper(II) oxide with carbon
D
reacting sodium carbonate with dilute hydrochloric acid
0620/01/O/N/05
ub
.
A
co
m
0620/01/O/N/05
A
16 An excess of acid in the stomach causes indigestion that can be cured by an anti-indigestion
tablet.
te
du
h
0620/01/O/N/05
What should the tablet contain to decrease the acidity?
an acidic substance
B
an alkaline substance
C
a neutral substance
D
Universal Indicator
ar
A
0620/01/O/N/05
17 A solution is made by adding sodium oxide to water.
.s
m
Which pH change can occur?
pH change
1
→
7
B
7
→
1
w
A
7
→
12
D
12
→
7
w
C
0620/01/O/N/05
w
18 Which element has an oxide that forms a salt with an alkali?
A
N
B
Na
C
Ne
D
Ni
133
134
19 Pure zinc sulphate can be prepared by adding an excess of either zinc carbonate or an excess of
zinc hydroxide to dilute sulphuric acid.
0620/01/O/N/05
In which form are these zinc compounds used?
A
zinc hydroxide
aqueous
solution
C
aqueous
solution
ub
.
aqueous
solution
B
solid
solid
aqueous
solution
solid
solid
te
du
h
D
co
m
zinc carbonate
B
C
iodide
nitrate
sulphate
w
w
w
D
chloride
0620/01/O/N/05
.s
m
A
ar
20 Which aqueous ion causes a yellow precipitate to form when acidified aqueous lead(II) nitrate is
added to it?
134
135
19 Which property does hydrochloric acid have?
0620/01/M/J/05
It gives a pale blue precipitate with aqueous copper(II) sulphate.
B
It gives a white precipitate with aqueous barium nitrate.
C
It releases ammonia from aqueous ammonium sulphate.
D
It releases hydrogen with zinc powder.
co
m
A
20 Hydrochloric acid is used to clean a metal surface by removing the oxide layer on the metal.
ub
.
This is because hydrochloric acid has a …..X….. pH and the metal oxide is …..Y…..
What are X and Y?
A
high
B
high
C
low
D
low
0620/01/M/J/05
Y
te
du
h
X
acidic
basic
acidic
basic
18 What is the colour of liquid bromine and of the aqueous bromide ion?
red-brown
red-brown
B
red-brown
colourless
C
yellow-green
yellow-green
D
yellow-green
colourless
.s
m
A
An aqueous solution contains barium iodide.
w
3
bromide ion
0620/01/M/J/05
ar
bromine
0620/01/O/N/08
w
It is possible to obtain a solution that contains Ba2+(aq) but no I–(aq) by adding ……1…… until no
more ……2…… precipitate forms.
w
Which words correctly complete gaps 1 and 2?
1
2
A
aqueous lead(II) nitrate
white
B
aqueous lead(II) nitrate
yellow
C
dilute sulphuric acid
white
D
dilute sulphuric acid
yellow
135
136
21 The apparatus shown can be used to prepare aqueous copper(II) sulphate.
filter paper
stirrer
excess of solid X
co
m
solid X
aqueous
copper(II)
sulphate
aqueous Y
heat
What are substances X and Y?
substance Y
A
copper
iron(II) sulphate
B
copper(II) chloride
C
copper(II) oxide
D
sulphur
te
du
h
substance X
ub
.
0620/01/M/J/05
sulphuric acid
sulphuric acid
copper(II) chloride
22 In the experiment shown, the dilute sulphuric acid is run into the flask of aqueous barium
hydroxide until the reaction is complete.
0620/01/M/J/05
ar
Which processes occur in this reaction?
neutralisation
precipitation
A
B
C
D
aqueous
barium
hydroxide
w
w
w
.s
m
dilute
sulphuric
acid
136
137
17 In different experiments, 2 g of marble are added to 10 cm3 of hydrochloric acid.
0620/01/M/J/05
In which tube is the reaction fastest?
B
C
cold
hydrochloric
acid
ub
.
hot
hydrochloric
acid
powdered marble
marble chips
powdered marble
te
du
h
marble chips
D
co
m
A
20 Dilute hydrochloric acid is added to aqueous barium nityrate in a test-tube.
What happens?
0620/01/O/N/08
the pH of the liquid
in the test-tube
a precipitate forms
A
decreases
yes
B
decreases
C
increases
yes
D
increases
no
.s
m
ar
no
23 Which substances react with dilute sulphuric acid to form a salt?
w
magnesium
magnesium
carbonate
magnesium
chloride
A
B
C
D
w
w
magnesium
oxide
0620/01/O/N/08
137
138
21 A colourless liquid in an unlabelled bottle is tested as shown.
•
Litmus paper turns red.
•
Magnesium ribbon fizzed.
•
Reaction with aqueous barium nitrate produced a white precipitate.
aqueous sodium hydroxide
B
aqueous sodium sulphate
C
dilute hydrochloric acid
D
dilute sulphuric acid
ub
.
A
co
m
What is the colourless liquid?
22 The diagrams show two experiments.
red
litmus paper
.s
m
ar
blue
litmus paper
aqueous
ammonium chloride
+
aqueous
sodium hydroxide
experiment 2
te
du
h
experiment 1
blue
litmus paper
aqueous
ammonium chloride
+
dilute
sulphuric acid
heat
heat
What happens to the pieces of litmus paper?
w
experiment 1
0620/01/O/N/08
experiment 2
A
blue → red
both pieces bleached
B
blue → red
no change
C
red → blue
both pieces bleached
D
red → blue
no change
w
w
red
litmus paper
138
139
22 Salts can be prepared by reacting a dilute acid
1
with a metal;
2
with a base;
3
with a carbonate.
0620/12/O/N/09
1 and 2 only
B
1 and 3 only
C
2 and 3 only
D
1, 2 and 3
ub
.
A
co
m
Which methods could be used to prepare copper(II) chloride?
31 Compound X is heated with carbon using the apparatus shown.
reaction tube
0620/12/O/N/09
te
du
h
compound X and
carbon
limewater
.s
m
ar
heat
A brown solid is formed in the reaction tube and the limewater turns cloudy.
What is compound X?
calcium oxide
B
copper(II) oxide
C
magnesium oxide
D
sodium oxide
w
w
w
A
139
7
140
14 Calcium carbonate was reacted with hydrochloric acid in a conical flask. The flask was placed on
a balance and the mass of the flask and contents was recorded as the reaction proceeded.
During the reaction, carbon dioxide gas was given off.
The reaction was carried out at two different temperatures.
0620/12/O/N/10
temperature at which mass
changed more quickly
A
decrease
higher temperature
B
decrease
lower temperature
C
increase
higher temperature
D
increase
lower temperature
0620/12/O/N/10
te
du
h
15 Some barium iodide is dissolved in water.
ub
.
change in mass
co
m
Which row is correct?
Aqueous lead(II) nitrate is added to the solution until no more precipitate forms.
This precipitate, X, is filtered off.
Dilute sulfuric acid is added to the filtrate and another precipitate, Y, forms.
What are the colours of precipitates X and Y?
white
B
white
white
yellow
.s
m
A
Y
ar
X
C
yellow
white
D
yellow
yellow
w
37 When added in turn to four solutions, aqueous sodium carbonate gives the following results.
Which solution is acidic?
w
w
solution
0620/01/O/N/08
result
A
a blue precipitate forms
B
a white precipitate forms
C
bubbles of gas form
D
no visible reaction occurs
140
24 The oxide of element X was added to an acid. It reacted to form a salt and water.
141
0620/12/O/N/10
acid
co
m
oxide of
element X
type of element X
A
greater than 7
metal
B
greater than 7
non-metal
C
less than 7
metal
D
less than 7
te
du
h
pH
ub
.
What is the pH of the acid before the reaction and what type of element is X?
w
w
w
.s
m
ar
non-metal
141
22 The results of three tests on a solution of compound X are shown.
test
result
white precipitate formed,
soluble in excess
aqueous ammonia added
white precipitate formed,
soluble in excess
dilute hydrochloric
acid added
bubbles of gas
co
m
aqueous sodium
hydroxide added
0620/12/O/N/11
B
aluminium chloride
C
zinc carbonate
D
zinc chloride
te
du
h
aluminium carbonate
ub
.
What is compound X?
A
142
23 Which property is not characteristic of a base?
It reacts with a carbonate to form carbon dioxide.
B
It reacts with an acid to form a salt.
C
It reacts with an ammonium salt to form ammonia.
D
It turns universal indicator paper blue.
ar
A
0620/12/O/N/11
.s
m
17 Copper(II) carbonate reacts with dilute sulfuric acid.
0620/12/O/N/11
CuCO3(s) + H2SO4(aq) → CuSO4(aq) + CO2(g) + H2O(l)
The speed of the reaction can be changed by varying the conditions.
Which conditions would always increase the speed of this chemical reaction?
Increase the concentration of the reactants.
2
Increase the size of the pieces of copper(II) carbonate.
3
Increase the temperature.
4
Increase the volume of sulfuric acid.
w
w
w
1
A
1, 3 and 4
B
1 and 3 only
C
2 and 3
D
3 and 4 only
142
143
15 Element X forms an acidic, covalent oxide.
Which row shows how many electrons there could be in the outer shell of an atom of X?
2
6
7
A
B
C
D
0620/12/O/N/12
ub
.
17 Barium hydroxide is an alkali. It reacts with hydrochloric acid.
co
m
1
How does the pH of the hydrochloric acid change as an excess of aqueous barium hydroxide is
added?
The pH decreases from 14 and becomes constant at 7.
B
The pH decreases from 14 to about 1.
C
The pH increases from 1 and becomes constant at 7.
D
The pH increases from 1 to about 14.
te
du
h
A
0620/12/O/N/12
18 Which of these pairs of aqueous ions both react with dilute sulfuric acid to give a visible result?
Ba2+ and Cl −
B
Ba2+ and CO32−
C
NH4+ and Cl −
D
NH4+ and CO32−
0620/12/O/N/12
.s
m
ar
A
19 A compound is a salt if it
can neutralise an acid.
B
contains more than one element.
C
dissolves in water.
0620/12/O/N/12
w
w
A
is formed when an acid reacts with a base.
w
D
143
144
32 Carbon dioxide is produced when dilute hydrochloric acid reacts with
A
calcium sulfate.
B
carbon.
C
copper(II) carbonate.
D
limewater.
33 The diagram shows two substances, X and Y, being heated together.
co
m
0620/12/O/N/12
damp Universal Indicator
paper
heat
te
du
h
substances X and Y
ub
.
0620/12/O/N/12
The Universal Indicator paper turns blue during the experiment.
What are substances X and Y?
ammonium nitrate and hydrochloric acid
B
ammonium nitrate and sodium hydroxide
C
sodium carbonate and hydrochloric acid
D
sodium carbonate and sodium hydroxide
w
w
w
.s
m
ar
A
144
145
16 A student investigates the rate of reaction between zinc and an excess of sulfuric acid.
The graph shows the results of two experiments, X and Y.
co
m
Y
X
0
0
ub
.
volume of
hydrogen
time
0620/12/O/N/13
te
du
h
Which change explains the difference between X and Y?
A
A catalyst is added in Y.
B
A lower temperature is used in Y.
C
Larger pieces of zinc are used in Y.
D
Less concentrated acid is used in Y.
ar
21 Compound X is tested and the results are shown in the table.
result
aqueous sodium hydroxide is
added, then heated gently
gas given off which turns damp
red litmus paper blue
dilute hydrochloric acid is added
effervescence, gas given off
which turns limewater milky
.s
m
test
w
w
w
Which ions are present in compound X?
A
ammonium ions and carbonate ions
B
ammonium ions and chloride ions
C
calcium ions and carbonate ions
D
calcium ions and chloride ions
0620/12/O/N/13
145
146
1
reacts with ammonium sulfate to form ammonia
2
turns red litmus blue
1
2
A
B
C
D
property 2
A
acidic
covalent
B
acidic
C
basic
D
basic
te
du
h
property 1
0620/12/O/N/13
ub
.
18 Which of the following are properties of the oxides of non-metals?
0620/12/O/N/13
co
m
17 Which are properties of an acid?
ionic
covalent
ionic
19 The reactions shown may occur in the air during a thunder storm.
ar
N2 + O2 → 2NO
0620/12/O/N/13
2NO + O2 → 2NO2
.s
m
NO + O3 → NO2 + O2
Which row shows what happens to the reactant molecules in each of these reactions?
NO
O3
A
oxidised
oxidised
oxidised
B
oxidised
oxidised
reduced
C
reduced
reduced
oxidised
D
reduced
reduced
reduced
0620/12/O/N/13
w
w
w
N2
146
147
20 Which statement about oxides is correct?
A
A solution of magnesium oxide will have a pH less than 7.
B
A solution of sulfur dioxide will have a pH greater than 7.
C
Magnesium oxide will react with nitric acid to make a salt.
D
Sulfur dioxide will react with hydrochloric acid to make a salt.
co
m
0620/13/O/N/14
21 Which salt preparation uses a burette and a pipette?
0620/13/O/N/14
calcium nitrate from calcium carbonate and nitric acid
B
copper(II) sulfate from copper(II) hydroxide and sulfuric acid
C
potassium chloride from potassium hydroxide and hydrochloric acid
D
zinc chloride from zinc and hydrochloric acid
ub
.
A
te
du
h
22 The graph shows how the pH of soil in a field changes over time.
0620/13/O/N/14
At which point was the soil neutral?
11
9
pH of 7
soil
B
D
C
ar
5
A
.s
m
3
time
23 Which statement about the elements of Group I is correct?
A
Lithium is more dense than sodium.
w
B
0620/13/O/N/14
Potassium is less reactive than sodium.
w
C
Potassium has a higher density than lithium.
Sodium has a higher melting point than lithium.
w
D
147
148
20 An oxide of element X dissolves in water to form a solution of pH 5.
type of element
type of oxide
A
metallic
acidic
B
metallic
basic
C
non-metallic
acidic
D
non-metallic
basic
It bleaches damp litmus paper.
B
It relights a glowing splint.
C
It turns cobalt(II) chloride paper pink.
D
It turns limewater cloudy.
te
du
h
A
0620/01/M/J/08
ub
.
21 Which statement describes a test for carbon dioxide gas?
co
m
0620/01/M/J/08
Which line in the table is correct?
19 A colourless solution is tested by the following reactions.
0620/13/O/N/14
Which reaction is not characteristic of an acid?
A piece of magnesium ribbon is added. Bubbles are seen and the magnesium disappears.
B
A pungent smelling gas is produced when ammonium carbonate is added.
C
Copper oxide powder is added and the mixed is warmed. The solution turns blue.
D
The solution turns blue litmus red.
.s
m
ar
A
21 An element E is burned in air. A white solid oxide is formed.
The oxide is tested with damp red litmus paper. The paper turns blue.
w
What is element E?
w
w
A
0620/12/M/J/09
calcium
B
carbon
C
iodine
D
sulfur
148
149
22 A solution of zinc sulphate can be made by adding an excess either of zinc carbonate or of zinc
hydroxide to dilute sulphuric acid.
zinc carbonate
zinc hydroxide
A
aqueous
aqueous
B
aqueous
solid
C
solid
aqueous
D
solid
solid
0620/01/M/J/08
co
m
In which forms are these zinc compounds added to the acid?
ub
.
23 Which aqueous ion causes a white precipitate to form when acidified aqueous silver nitrate is
added to it?
chloride
B
iodide
C
nitrate
D
sulphate
te
du
h
0620/01/M/J/08
A
24 What is the colour of gaseous chlorine and of solid sodium chloride?
sodium chloride
A
colourless
B
colourless
white
C
yellow-green
yellow-green
.s
m
chlorine
0620/01/M/J/08
D
yellow-green
white
ar
yellow-green
25 The Group I elements lithium and potassium are tested.
w
Which element has the higher melting point and which element reacts more vigorously with
water?
A
lithium
lithium
B
lithium
potassium
C
potassium
lithium
D
potassium
potassium
w
w
higher melting point
more vigorous
reaction with water
0620/01/M/J/08
149
150
20 Some reactions of a substance, R, are shown in the diagram.
magnesium
reacts with
substance R
hydrogen
sodium carbonate
carbon dioxide
an acid
B
a base
C
an element
D
a salt
0620/12/M/J/09
te
du
h
A
copper(II) sulfate
ub
.
What type of substance is R?
co
m
copper(II) oxide
27 Farmers add calcium oxide (lime) and ammonium salts to their fields.
The compounds are not added at the same time because they react with each other.
Which gas is produced in this reaction?
ammonia
B
carbon dioxide
C
hydrogen
D
nitrogen
0620/12/O/N/13
w
w
w
.s
m
ar
A
150
14 Iron is extracted from iron oxide using carbon monoxide as shown in the equation.
151
iron oxide + carbon monoxide → iron + carbon dioxide
0620/13/M/J/10
A
Carbon monoxide is oxidised to carbon dioxide.
B
Carbon monoxide is reduced to carbon dioxide.
C
Iron is oxidised to iron oxide.
D
Iron oxide is oxidised to iron.
co
m
What does the equation show?
The loss in mass of the reaction flask is measured.
ub
.
15 A student investigates the rate of reaction between marble chips and hydrochloric acid.
0620/13/M/J/10
te
du
h
The graph shows the results of two experiments, P and Q.
mass of
reaction flask
P
Q
0
time
ar
Which change explains the difference between P and Q?
A catalyst is added in P.
B
A higher temperature is used in P.
C
Bigger marble chips are used in Q.
Hydrochloric acid is more concentrated in Q.
w
w
w
D
.s
m
A
151
152
22 Aqueous sodium hydroxide is added to a solid, X, and the mixture is heated.
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A green precipitate is formed and an alkaline gas is given off.
A
NH4+ and Fe2+
B
NH4+ and Fe3+
C
OH– and Fe2+
D
OH– and Fe3+
co
m
Which ions are present in X?
Which statement about methylamine is correct?
ub
.
23 An aqueous solution of the organic compound methylamine has a pH greater than 7.
It neutralises an aqueous solution of sodium hydroxide.
B
It reacts with copper(II) carbonate to give carbon dioxide.
C
It reacts with hydrochloric acid to form a salt.
D
It turns blue litmus red.
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A
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24 The positions in the Periodic Table of four elements are shown.
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A
C
D
w
w
w
.s
m
B
ar
Which element is most likely to form an acidic oxide?
152
19 Carbon dioxide is an acidic oxide that reacts with aqueous calcium hydroxide.
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decomposition
B
fermentation
C
neutralisation
D
oxidation
co
m
Which type of reaction takes place?
A
153
20 A solution contains barium ions and silver ions.
What could the anion be?
chloride only
B
nitrate only
C
sulfate only
D
chloride or nitrate or sulfate
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A
ub
.
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21 A mixture containing two anions was tested and the results are shown below.
test
result
effervescence of a gas which
turned limewater milky
dilute nitric acid added, followed
by aqueous silver nitrate
yellow precipitate formed
ar
dilute nitric acid added
A
B
C
carbonate and chloride
carbonate and iodide
sulfate and chloride
sulfate and iodide
w
D
w
22 Which is not a typical property of an acid?
w
0620/12/M/J/11
.s
m
Which anions were present?
A
They react with alkalis producing water.
B
They react with all metals producing hydrogen.
C
They react with carbonates producing carbon dioxide.
D
They turn litmus paper red.
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153
154
14 The diagram shows the reaction between zinc oxide and dilute hydrochloric acid.
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co
m
zinc oxide powder
aqueous
zinc chloride
22 °C
pH 7
dilute
hydrochloric acid
20 °C
pH 1
Which terms describe the reaction?
neutralisation
A
B
C
D
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endothermic
after
ub
.
before
w
w
w
.s
m
ar
154
7
155
15 Four different gases are passed through the apparatus shown.
gas in
gas out
damp blue
litmus paper
co
m
damp red
litmus paper
Which gas has no effect on either piece of litmus paper?
ammonia
B
carbon dioxide
C
chlorine
D
hydrogen
ub
.
A
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16 An aqueous solution of copper(II) sulfate was made by adding excess copper(II) oxide to dilute
sulfuric acid. The mixture was heated, stirred and then filtered.
copper(II) sulfate
solution
dilute
sulfuric acid
heat
ar
copper(II) oxide
.s
m
What was the pH of the acid before adding the copper(II) oxide and of the solution after filtration?
pH of solution
after filtration
A
greater than 7
7
B
greater than 7
less than 7
C
less than 7
7
D
less than 7
greater than 7
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w
w
w
pH of acid before adding
copper(II) oxide
155
156
17 Aqueous potassium iodide is added to aqueous silver nitrate.
precipitate
solution
A
brown
colourless
B
white
yellow
C
yellow
colourless
D
yellow
white
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co
m
What are the colours of the final precipitate and solution?
ub
.
18 Three gas jars contain carbon dioxide, hydrogen and oxygen, as shown.
te
du
h
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carbon dioxide
hydrogen
oxygen
Which one of the following tests could be used to discover which gas is in each jar?
a glowing splint
B
a lighted splint
C
damp blue litmus paper
D
limewater
w
w
w
.s
m
ar
A
156
157
20 The diagram shows an experiment.
red
litmus paper
co
m
blue
litmus paper
aqueous
ammonium chloride
+
aqueous
sodium hydroxide
heat
What happens to the pieces of litmus paper?
A
changes colour
B
changes colour
C
no colour change
D
no colour change
red litmus paper
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blue litmus paper
ub
.
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changes colour
no colour change
changes colour
no colour change
ar
21 Two indicators, bromophenol blue and Congo red, show the following colours in acidic solutions
and in alkaline solutions.
acid
alkali
bromophenol blue
yellow
blue
Congo red
violet
red
.s
m
indicator
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A few drops of each indicator are added to separate samples of a solution of pH 2.
w
w
w
What are the colours of the indicators in this solution?
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in a solution of pH 2
bromophenol blue is
Congo red is
A
blue
red
B
blue
violet
C
yellow
red
D
yellow
violet
157
158
19 Element X forms an oxide, XO, that neutralises sulfuric acid.
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nature of oxide, XO
A
metal
acidic
B
metal
basic
C
non-metal
acidic
D
non-metal
basic
ub
.
element X
co
m
Which row describes X and XO?
20 Copper carbonate reacts with dilute sulfuric acid to make copper sulfate.
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CuCO3(s) + H2SO4(aq) → CuSO4(aq) + CO2(g) + H2O(l)
Which row gives the correct order of steps for making copper sulfate crystals?
step 1
step 2
step 3
step 4
filter
evaporate filtrate to
point of crystallisation
leave to cool
filter
evaporate to
dryness
leave to cool
add excess acid to
the copper carbonate
B
add excess acid to
the copper carbonate
C
add excess copper
carbonate to the acid
evaporate to point
of crystallisation
leave to cool
filter
D
add excess copper
carbonate to the acid
filter
evaporate filtrate to
point of crystallisation
leave to cool
.s
m
ar
A
w
19 Which statement about the reaction of acids is correct?
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They react with ammonium salts to form a salt and ammonia only.
B
They react with metal carbonates to give a salt and carbon dioxide only.
C
They react with metal hydroxides to give a salt and water only.
D
They react with metals to give a salt, hydrogen and water only.
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w
A
158
159
21 Element X is a non-metal.
In which position of the Periodic Table could element X be found?
A
at the bottom of Group I
B
at the top of Group 0
C
at the top of Group I
D
in the transition elements
co
m
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22 Aqueous sodium hydroxide is added to solid X and the mixture is heated.
NH4+ and Fe2+
B
NH4+ and Fe3+
C
OH– and Fe2+
D
OH– and Fe3+
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w
w
.s
m
ar
A
te
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Which ions are present in X?
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ub
.
A green precipitate is formed and an alkaline gas is given off.
159
160
15 Which statement is not correct?
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When a base reacts with an ammonium salt, ammonia is given off.
B
When an acid reacts with a base, neutralisation takes place.
C
When an acid reacts with a carbonate, carbon dioxide is given off.
D
When the acidity of a solution increases, the pH increases.
co
m
A
16 Hydrochloric acid is used to clean metals.
The acid reacts with the oxide layer on the surface of the metal, forming a salt and water.
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alloy
B
base
C
element
D
indicator
te
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A
ub
.
Which word describes the metal oxide?
17 Which method is used to make the salt copper sulfate?
dilute acid + alkali
B
dilute acid + carbonate
C
dilute acid + metal
D
dilute acid + non-metal oxide
ar
A
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.s
m
18 Two tests are carried out to identify an aqueous solution of X.
test 1
Aqueous sodium hydroxide is added and a blue precipitate is produced.
test 2
Dilute nitric acid is added followed by aqueous silver nitrate and a white
precipitate is produced.
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w
What is X?
copper carbonate
B
copper chloride
C
iron(III) carbonate
D
iron(III) chloride
w
w
A
160