Jordanhill School Chemistry Department
National 5
Unit 1 Homework Exercises
Instructions
The purpose of this booklet is to help you revise earlier work, to give you practice with past exam
questions, and to improve your knowledge and understanding of Higher chemistry. It is therefore
important that your homework exercises are your best work. As such, you should follow these
instructions:
1. Use your text book and notes to help you with the questions.
2. You will be given 1 week to complete each exercise. This is to give you time to complete
the exercise, and to seek help from your teacher if you cannot work out the answer to a
question.
Do not leave blanks! Seek help!
3. Please look after this booklet as you will have to return it at the end of the course.
If you follow these instructions, you will continue to be successful at chemistry.
Do not write on this book, all exercises should be completed in your homework jotter
Exercise 1- Reaction Rates
Int 2 2000
Int 2 2004
1. The graph below shows a variation of
concentration of a reactant with time as a
reaction proceeds.
3. The table shows the times taken for 0.5g of
magnesium to react completely with acid
under different conditions.
Concentration (mol l-1)
1.00
0.75
Temperature
(°C)
Reaction
time (s)
20
80
0.1
25
60
0.2
30
20
0.2
40
10
0.50
0.25
0
10
20
30
40
The time for 0.5g of magnesium to react
completely with 0.2 mol l-1 acid ad 25°C will
be
50
Time (s)
During the first 20s, the average reaction
rate, in mol l-1 s-1, is
A
B
C
D
0.0125
0.0180
0.0375
0.0450
Int 2 2003
2. Magnesium was reacted with dilute
hydrochloric
acid
under
different
conditions. In each experiment an excess
of magnesium was added.
Reaction 1
100 cm3 2 mol l-1
hydrochloric
acid at 20°C
Reaction 2
100 cm3 1 mol l-1
hydrochloric
acid at 20°C
magnesium
powder
magnesium
powder
Which line in the table correctly describes
Reaction 2 when compared to Reaction 1?
Rate of reaction
faster
faster
slower
slower
less than 10s
between 10s and 20s
between 20s and 60s
more than 80s
Int 2 2005
Volume of gas
produced
less
the same
less
the same
4. Graph P shows the volume of hydrogen gas
collected when 1.0g of magnesium ribbon
reacts with excess 2 mol l-1 hydrochloric
acid.
Volume of hydrogen (cm3)
A
B
C
D
A
B
C
D
Acid
concentration
(mol l-1)
0.1
1000
P
500
Q
Time (s)
Which of the following samples of
magnesium, when reacted with excess 2
mol l-1 hydrochloric acid would produce
graph Q.
A
B
C
D
0.5g of magnesium ribbon
0.5g of magnesium powder
1.0g of magnesium powder
2.0g of magnesium ribbon
Int 2 2001
5. Hydrochloric acid is a strong acid. The table shows the pH values of some hydrochloric acid
solutions.
Concentration (mol l-1)
1.0
0.1
0.01
0.001
pH
0
1
2
3
(a) Predict the concentration of hydrochloric acid solution with a pH of 5.
(1)
(b) Describe the experiment which you could carry out to compare the rate of reaction of
hydrochloric acid and ethanoic acid with magnesium.
(2)
Int 2 2001
6. Human blood contains Fe3+ ions.
To find the concentration of Fe3+ in blood, the Fe3+ ions are first converted into Fe2+ ions.
(a) Fe2+ ions are then reacted to form a purple compound.
When the solution is placed in a beam of light only some of the light is transmitted.
These results show the percentage of light transmitted for a series of solutions of known Fe 2+
concentration.
Concentration Fe2+
(mg l-1)
1.0
2.0
3.0
4.0
6.0
8.0
% Transmittance
79
65
55
44
27
18
(i)
Plot the results as a line graph
(3)
(ii)
Using your graph, estimate the concentration of Fe2+ ions present in a solution with a
transmittance of 36%.
(1)
SG C 2002/ Int 2 2005
7. The rate of reaction between zinc and dilute hydrochloric acid can be followed by measuring the
volume of gas given off during the reaction.
(a) Copy, complete and label the diagram to show how you would collect the gas given off.
(2)
zinc pieces
dilute hydrochloric acid
7. (continued)
(b) The results for the reaction are shown below.
Volume of gas (cm3)
0
20
40
58
72
80
Time (seconds)
0
10
20
30
40
50
60
Predict the volume of gas which would have been given off after 60 seconds.
(1)
(c) Calculate the average rate at which gas is given off during the first 40 seconds of the
reaction.
(2)
(d) Why would increasing the concentration of the acid increase the rate of reaction?
(1)
SG C 2010
8. A student added magnesium ribbon to an excess of dilute sulphuric acid and measured the
volume of hydrogen gas produced.
The reaction stopped when all the magnesium was used up.
Time /s
0
10
20
40
50
60
70
Volume of hydrogen
gas /cm3
0
20
32
50
52
53
53
(a) State the test for hydrogen gas.
(1)
(b) Draw a line graph of the results
use appropriate scales to fit most of the graph paper
(3)
(c) Using your graph, predict the volume of hydrogen gas produced during the first 30 seconds
(1)
(d) The student repeated the experiment using a higher concentration of acid. The same
volume of acid and the same mass of magnesium ribbon were used.
What volume of hydrogen gas would have been produced after 60 seconds?
(1)
Exercise 2- Atoms
Int 2 2007
Int 2 2006
1. Which of the following elements has
similar chemical properties to argon?
A
B
C
D
Fluorine
Krypton
Potassium
Zinc
5. The table shows information about some
atoms
Atom
W
X
Y
Z
2.
solid
A
B
C
D
W and X
X and Y
W and Y
Y and Z
Int 2 2004
Which of the following would not be
evidence of a chemical reaction when a
solid is added to the solution?
6. Which of the following elements exists as a
noble gas?
A colour change
A gas being given off
The temperature rising
The solid disappearing
A
B
C
D
Int 2 2006
Nitrogen
Fluorine
Oxygen
Neon
Int 2 2002
7. An atom has atomic number 17 and mass
number 35.
The number of neutrons in the atom is
3. Which of the following elements is an alkali
metal?
A
B
C
D
Aluminium
Calcium
Copper
Sodium
A
B
C
D
17
18
35
52
4. Which of the following is the electron
arrangement of a halogen atom?
A
B
C
D
2,5
2,6
2,7
2,8
Mass number
34
36
40
40
Which two atoms are isotopes of the same
element?
solution
A
B
C
D
Atomic number
16
18
18
20
Int 2 2013
8. Which line in the table correctly describes
a proton?
A
B
C
D
Mass
negligible
negligible
1
1
Charge
0
-1
+1
0
Location
outside nucleus
outside nucleus
in nucleus
in nucleus
Int 2 2001
9. The most common isotope of potassium is
39
.
19 K
(a) Copy and complete the table to show the number of particles in an atom of
Type of particle
39
19 K
.
Number of particles
Proton
Neutron
Electron
(1)
(b) How do isotopes of potassium differ from each other?
(1)
Int 2 2013
10. Strontium compounds have many uses.
(a) Strontium nitrate is used in warning flares.
What colour flame will strontium nitrate give?
(you may wish to use the data booklet to help you.)
(1)
(b) Strontium chloride hexahydrate can be used in toothpaste for sensitive teeth as it plugs the
holes in the tooth enamel.
This is possible because strontium has similar chemical properties to calcium.
Why does strontium have similar chemical properties to calcium?
(1)
Int 2 2009
11. Electrons are arranged in energy levels.
Complete the diagram to show how the electrons are arranged in an atom of sodium
(You may wish to use page 6 of the data booklet to help you.)
= Nucleus
X = Electron
(1)
SG C 2009
12. There are three different types of neon atom.
Type of atom
Number of protons
Number of neutrons
20
10 Ne
21
10 Ne
22
10 Ne
(a) Complete the table to show the number of protons and neutrons in each atom.
(1)
(b) What term is used to describe the different types of neon atom?
(1)
(c) A natural sample of neon has an average atomic mass of 20.2.
What is the mass number of the most common type of atom in the sample of neon?
(1)
Int 2 2013
Electronegativity
13. Electronegativity is the measure of attraction that an atom has for the bonded electrons.
The chart shows the electronegativity values for some elements in the periodic table.
Atomic number
(a) Describe what happens to the electronegativity values going across a period in the
periodic table.
(1)
(b) Give a value for the electronegativity of the element calcium, atomic number 20.
(1)
Exercise 3- Ions and Bonding
Int 2 2013
Int 2 2004
1. In a hydrogen fluoride molecule, the atoms
share electrons in order to achieve the
same electron arrangements as the atoms
in group
A
B
C
D
0
1
2
7
Int 2 2008
2. The table below show information about
an ion.
5. During electrolysis of silver(I) nitrate
solution, silver ions, Ag+(aq),
A gain electrons
electrode
B lose electrons
electrode
C gain electrons
electrode
D lose electrons
electrode.
at
the
negative
at
the
negative
at
the
positive
at
the
positive
Int 2 2009
Particle
Number
protons
19
neutrons
20
electrons
18
The charge on the ion is
A 1+
B 1C 2+
D 2Int 2 2002
6. Which of the following diagrams
represents a compound made up of
diatomic molecules?
A
B
3. Which substance does not exist as
diatomic molecules?
A
B
C
D
Nitrogen
Oxygen
Fluorine
Neon
4. Which one of the following particles
contains a different number of electrons
from the others?
(You may wish to use page 6 of the data
booklet to help you.)
A
B
C
D
ClS2Ar
Na+
C
D
SG C 2013
7. The grid shows some ions.
B
A
C
Al3+
Cl-
D
Li+
E
F
H+
Br-
OH-
(a) Identify the ion with the same electron arrangement as a helium atom.
You may wish to use the data booklet to help you.
(1)
(b) Identify the two ions which combine to form an insoluble compound.
You may wish to use the data booklet to help you.
(1)
SG C 2004*
8. The table contains some information about some substances
Substance
Melting
point/ °C
Boiling
point/ °C
A
B
C
D
E
F
455
80
1492
1407
645
98
1567
218
2897
2357
1287
890
Conducts as
a solid
a liquid
no
yes
no
no
yes
yes
no
no
no
yes
yes
yes
(a) Identify the two ionic compounds.
(1)
(b) Identify the substance which exists as a covalent network.
(1)
(c) Identify the substances which would be liquid at 1500°C
(2)
SG C 2003
9. Copy and complete the table to show the number of each type of particle in
Type of particle
Proton
Neutron
Electron
35
17
Cl- .
Number of particles
(1)
SG C 2004
10. In a hydrogen molecule the atoms share two electrons in a covalent bond.
+ = Nucleus
+
+
= Electron
(a) Explain how the covalent bond holds the two hydrogen atoms together.
(1)
(b) The hydrogen molecule can be represented more simply as
H H
Showing all outer electrons, draw a similar diagram to represent a molecule of ammonia, NH3.
(1)
Int 2 2011/ N5 2014
11. The properties of a substance depend on its type of bonding and structure.
There are four types of bonding and structure.
A
B
C
D
Discreet covalent
molecular
Covalent
network
Ionic lattice
Metallic lattice
(a) Complete the table to match up each type of bonding with its properties
Bonding and
structure type
Properties
Do not conduct electricity and have high
melting points
Have high melting points and conduct
electricity when liquid but not when solid
Conduct electricity when solid and have a wide
range of melting points
Do not conduct electricity and have low
melting points
(2)
(b) Graphene is a substance made of a single layer of carbon atoms. Graphene can conduct
electricity.
Suggest what this means about some of the electrons in graphene.
(1)
11. (Continued)
(c) A section of a covalent network compound is shown below.
Write the formula for this covalent network compound.
(1)
SG C 2013
12. Nitrogen trifluoride, NF3, is used in the manufacturing of plasma screens.
(a) Draw a diagram showing all outer electrons in a molecule of nitrogen trifluoride.
(b) The atoms in nitrogen trifluoride are held together by covalent bonds.
Copy the sentence with the correct words to give information about covalent bonds
(1)
(1)
SG C 2012
13. A student investigated how the concentration of sodium chloride in water affected the
freezing point.
(a) What type of bond is broken in sodium chloride when it is dissolved in water?
(1)
(b) The table shows information about the freezing point of different sodium chloride solutions.
Concentration of sodium
chloride solution (mol/l)
1
0.09
0.18
0.27
0.37
0.46
Freezing point (oC)
0
–0.2
–0.5
–0.8
–1.1
–1.5
Describe the relationship between the concentration and freezing point.
(1)
(c) Predict the freezing point of a 0.55 mol/l sodium chloride solution.
(1)
SG C 2011
14. A student set up the following experiment to electrolyse cobalt chloride solution.
(a) The formula for cobalt chloride is CoCl2.
What is the charge on the cobalt ion in CoCl2?
(1)
(b) Describe what would be seen at the positive electrode.
You may wish to use your data booklet to help you.
(1)
SG C 2011
15. The grid shows the formulae of some oxides.
B
A
C
ZnO
D
K2O
NO2
E
F
CO
Fe2O3
CuO
Identify the two oxides which are covalent.
(1)
Int 2 2011
16. A hydrogen fluoride molecule can be represented as:
H
X
F
Showing all outer electrons draw a similar diagram to represent a molecule of water, H 2O
(2)
Exercise 4- Formula and Shapes of Molecules
Int 2 2001
1. The charge on the iron ion in Fe2(SO4)3 is
A 2+
B 3+
C 2D 3Int 2 2002
2. The formula for magnesium sulfate is
A MgS
B MgSO3
C MgSO4
D MgS2O3
Int 2 2003
3. A metal X reacts with oxygen to form an
oxide, X2O3.
During the reaction each atom of metal X
A gains two electrons
B gains three electrons
C loses two electrons
D loses three electrons
4. The formula for potassium sulfate is
A P2SO3
B K2SO4
C P2SO4
D K2S
Int 2 2004
5. When hydrogen chloride gas is dissolved in
water a solution containing hydrogen ions
and chloride ions is formed.
Which equation correctly shows the state
symbols for this change?
A HCl(g) + H2O(l)  H+(aq) + Cl-(aq)
B HCl(l) + H2O(aq)  H+(l) + Cl-(l)
C HCl(aq) + H2O(l)  H+(aq) + Cl-(aq)
D HCl(g) + H2O(l)  H+(l) + Cl-(l)
Int 2 2005
6. Which of the following compounds
contains only two elements?
A Magnesium hydroxide
B Magnesium phosphate
C Magnesium sulfite
D Magnesium nitride
7. A substance, X, has a melting point of
996°C and a boiling point of 1704°C. It only
conducts electricity when molten or
dissolved in water.
The structure of X is likely to be
A ionic
B metallic
C covalent network
D covalent molecular
Int 2 2012
8. The shapes and names of some molecules
are shown below.
tetrahedral pyramidal
bent
linear
Phosphine is a compound of phosphorus
and hydrogen. The shape of the molecule
of phosphine is likely to be
A tetrahedral
B pyramidal
C bent
D linear
Int 2 2013
9. What is the name of the compound with
the formula VO2?
A Vanadium(V) oxide
B Vanadium(IV) oxide
C Vanadium(III) oxide
D Vanadium(II) oxide
Int 2 2009
10. Two tests were carried out for compound X.
The following results were obtained.
Test
Result
1
Limewater turns cloudy
2
Flame turns blue/green
Which of the following could be compound X?
(You may wish to use page six of the data booklet to help you)
A Barium carbonate
B Copper carbonate
C Copper sulfate
D Sodium sulfate
Int 2 2007*
11. Rust contains iron(III) oxide.
(a) Write the formula for iron(III) oxide.
(1)
(b) What type of bonding occurs in iron(III) oxide?
(1)
Int 2 2008
12. Chlorofluorocarbons (CFCs) are a family of compounds which are highly effective as refrigerants
and aerosol propellants. However, they are now known to damage the ozone layer.
One example of a CFC molecule is shown.
What term is used to describe the shape of this molecule?
(1)
Int 2 2011*
13. Information on some two-element molecules is shown in the table.
Name
Formula
Hydrogen fluoride
HF
Water
H2O
Ammonia
NH3
Methane
CH4
(a) Draw and name the shapes of each of the molecules on the table.
(4)
(b) The hydrogen fluoride molecule can be represented as:
H
X
F
Showing all outer electrons, draw a similar diagram to represent a molecule of
methane, CH4
(2)
Int 2 2012
14. Glass is made up from the chemical silica, SiO2, which is covalently bonded and has a
melting point of 1700°C
(a) What does the melting point of silica suggest about its structure?
(1)
(b) Antimony(III) oxide is added to reduce any bubbles that may appear during the
manufacturing process.
Write the chemical formula for antimony(III) oxide
(1)
(c) In the manufacture of glass, other chemicals can be added to alter the properties of
the glass. The element boron can be added to the glass to make oven proof dishes.
(i)
Information about an atom of boron is given in the table below.
Particle
Number
proton
5
electron
5
neutron
6
14. (Continued)
Use this information to complete the nuclide notation for this atom of boron.
___
___
(ii)
B
(1)
Atoms of boron exist which have the same number of protons but a different
number of neutrons from that shown in the table.
What name can be used to describe the different atoms of boron?
(1)
Int 2 2012
15. Rapid inflation of airbags in cars is caused by the production of nitrogen gas.
The graph gives information on the volume of gas produced over 30 microseconds
Volume of nitrogen produced (litres)
50
40
30
20
10
0
0
5
10
15
20
25
30
Time (microseconds)
(a) (i)
(ii)
Calculate the average rate of reaction between 2 and 10 microseconds.
(1)
At what time has half of the final volume of nitrogen gas been produced?
(1)
(b) In some types of airbags, electrical energy causes sodium azide, NaN3, to decompose
producing sodium metal and nitrogen gas.
Write a formula equation for this
(1)
(c) Potassium nitrate is also present in the airbag to remove the sodium metal by converting
it into sodium oxide.
Why is it necessary to remove the sodium metal?
(1)
Exercise 5- The mole
Int 2 2001
1. The gram formula mass of sodium
carbonate is 106g.
How many moles are present in 5.3g of
sodium carbonate?
A 0.05
B 0.5
C 2
D 20
Int 2 2002
2. What is the relative formula mass of
ammonium sulfate, (NH4)2SO4?
A 70
B 118
C 132
D 228
Int 2 2003
3. The formula mass of
carbonate, (NH4)2CO3 is?
A 52
B 64
C 96
D 110
ammonium
Int 2 2006
4. What is the correct formula for aluminium
sulfate?
A AlSO4
B Al(SO4)3
C Al2(SO4)3
D Al3(SO4)2
5. Glucose has the molecule formula C6H12O6.
How many moles are contained in 18g of
glucose?
A 0.01
B 0.1
C 1
D 10
6. 0.2 moles of gas has a mass of 12.8g.
Which of the following could be the
molecular formula for the gas?
A SO2
B CO
C CO2
D NH3
Int 2 2008
7. How many moles are present in 1.7g of
ammonia, NH3?
A 0.1
B 1.0
C 1.7
D 17
Int 2 2010
8. xAl(s) + yBr2(l)  zAlBr3(s)
The equation will be balanced when
A x = 1, y = 2, z = 1
B x = 2, y = 3, z = 2
C x = 3, y = 2, z = 3
D x = 4, y = 3, z = 4
Int 2 2013
9. 4NH3 + xO2  4NO + yH2O
The equation will be balanced when
A x = 5, y = 6
B x = 5, y = 10
C x = 3, y = 6
D x = 3, y = 10
10. Which of the following substances has the
smallest gram formula mass?
A CO
B CO2
C N2
D CH4
Int 2 2013
11. The equation below shows the breakdown of glyceryl tristearate to form glycerol and
stearic acid.
C57H110O6
+
3H2O

C3H8O3
+
3C18H36O2
glyceryl tristearate
water
glycerol
stearic acid
GFM = 890g
Calculate the mass of stearic acid produced from 8.9g of glycerol tristearate.
(3)
Int 2 2014
12. Ammonia can be used to make the fertiliser, ammonium phosphate.
3NH3 + H3PO4  (NH4)3PO4
Calculate the mass of ammonium phosphate that would be produced from 510g of
ammonia.
(3)
Int 2 2011
13. Hydrogen peroxide is a useful bleaching agent and is contained in many hair dyes.
Over time, the hair dye becomes less effective as the hydrogen peroxide decomposes
forming water and oxygen.
The equation for the decomposition of hydrogen peroxide is:
H2O2(aq)

O2(g)
+
H2O(l)
(a) Balance this equation
(1)
(b) State the test for oxygen gas
(1)
(c) When 34g of hydrogen peroxide decomposes, 12 litres of oxygen is produced.
Calculate the volume of oxygen produced when 1.7g of hydrogen peroxide decomposes
(2)
14. Ammonium sulfate is a commonly used fertiliser. It can be produced by the reaction between
ammonium carbonate and calcium sulfate.
(NH4)2CO3(aq)
+
CaSO4(aq)

(NH4)2SO4(aq)
+
CaCO3(s)
What mass of ammonium carbonate, (NH4)2CO3, would be needed to make 13.2kg of
ammonium sulfate (NH4)2SO4?
(3)
Int 2 2010
15. Gold is a very soft metal. In order to make it harder, goldsmiths mix it with silver.
The quality of gold is indicated in carats.
(a) The graph shows information about the quality of the gold.
(i)
What is the percentage of silver in an 18 carat gold ring?
(1)
(ii)
Calculate the mass of silver in an 18 carat gold ring weighing 6g.
(1)
(b) Silver tarnishes in air forming black silver sulfide, Ag2S.
The equation for the reaction is:
4Ag
+
2H2S
+ O2

2Ag2S
+
2H2O
What mass of silver sulfide would be formed from 1.08g of silver?
(3)
Int 2 2009
16. Iron is produced from iron ore in a Blast Furnace. The equation is shown:
Fe2O3(s)
+
CO(g)

Fe(l)
+
CO2(g)
(a) Balance this equation.
(1)
(b) From the balanced equation below, calculate the mass of carbon monoxide produced
when 1200kg of carbon reacts.
(3)
CO2(g)
+
C(s)

2CO(g)
Exercise 6- pH & Neutralisation
Int 2 2000
1. Which oxide, when shaken with water,
would leave the pH unchanged?
A Calcium oxide
B Carbon dioxide
C Sulfur dioxide
D Zinc oxide
Int 2 2001
2. An acidic solution contains
A Only hydrogen ions
B Equal numbers of hydrogen and
hydroxide ions
C More hydrogen ions than hydroxide
ions
D More hydroxide ions than hydrogen
ions
Int 2 2002
3. Which of the following statements
describes the concentrations of H+(aq) and
OH-(aq) ions in pure water?
A The concentrations of H+(aq) and OH(aq) ions are equal.
B The concentrations of H+(aq) and OH(aq) ions are zero.
C The concentration of H+(aq) ions is
greater than the concentration of OH(aq) ions.
D The concentration of OH-(aq) ions is
greater than the concentration of
H+(aq) ions.
4. Which of the following sodium chloride
solutions would contain the most dissolved
solute?
A 100cm3 of 4 mol l-1 solution
B 200cm3 of 3 mol l-1 solution
C 300cm3 of 1 mol l-1 solution
D 400cm3 of 0.5 mol l-1 solution
Int 2 2003
5. 0.25 mol of potassium hydroxide was
dissolved in water and the solution made
up to 500cm3.
What was the concentration, in mol l-1, of
the solution which was formed?
A 0.0005
B 0.125
C 0.5
D 2.0
6. Identify the spectator ions in the following:
Pb2+(aq) + 2NO3-(aq) + 2Na+(aq) + 2I-(aq)
Pb2+(I-)2(s) + 2Na+ (aq) + 2NO3-(aq)
A
B
C
D
Na+(aq) and NO3-(aq)
Na+(aq) and I-(aq)
Pb2+(aq) and NO3-(aq)
Pb2+(aq) and I-(aq)
Int 2 2004
7. Which of the following oxides, when
shaken with water, would leave the pH
unchanged?
(you may wish to use page 8 of the data
booklet to help you.)
A Carbon dioxide
B Copper oxide
C Sodium oxide
D Sulfur dioxide
8. Which of the following compounds is a
base?
A Magnesium carbonate
B Magnesium chloride
C Magnesium nitrate
D Magnesium sulfate
Int 2 2007
9. Which of the following increases when
hydrochloric acid is diluted with water?
A Rate of reaction with magnesium
B Concentration of H+ ions
C Electrical conductivity
D pH
Int 2 2007
10. When 100cm3 of a 1 mol l-1 solution of
sodium sulfate was evaporated to dryness,
14.2g of solid was obtained.
To obtain 14.2g of solid from a 2mol l-1
solution of sodium sulfate the volume of
the solution needed would be
A 20cm3
B 50cm3
C 100cm3
D 200cm3
11. In which of the following test tubes will a
gas be produced?
A
Int 2 2008
13. 1 mole of sodium chloride can be used to
prepare
A 250cm3 of a 0.4 mol l-1 solution
B 250cm3 of a 4 mol l-1 solution
C 200cm3 of a 0.5 mol l-1 solution
D 200cm3 of a 1 mol l-1 solution
Int 2 2010
14. In a neutralisation reaction between an
acid and an alkali, the pH
A of the acid increases
B of the acid is unchanged
C of the alkali increases
D of the alkali is unchanged
15. An alkaline solution contains
A Only hydrogen ions
B More hydrogen ions than hydroxide
ions
C More hydroxide ions than hydrogen
ions
D Equal numbers of hydrogen ions and
hydroxide ions
B
C
Int 2 2011
16. Which of the following pairs of chemicals
react to produce a gas that turns lime
water milky?
A Calcium carbonate and dilute
hydrochloric acid
B Copper oxide and dilute sulfuric acid
C Copper and dilute hydrochloric acid
D Magnesium and dilute sulphuric acid
D
Int 2 2008
12. Which of the following oxides will dissolve
in water to produce an alkaline solution?
(You may wish to use page 8 of the data
booklet)
A Carbon dioxide
B Copper(II) oxide
C Potassium oxide
D Nitrogen dioxide
17. Which line in the table describes what
happens to a dilute solution of
hydrochloric acid when water is added to
it?
H+(aq)
pH
concentration
A
increases
increases
B
increases
decreases
C
decreases
increases
D
decreases
decreases
Int 2 2011
18. Fizzy drinks contain acids.
These acids can attack the compound calcium hydroxyapatite which is found in tooth
enamel.
The equation for the reaction is:
Ca10(PO4)6(OH)2(s) + 8H+(aq)  6CaHPO4(s) + 4Ca2+(aq) + 2H2O
Calcium hydroxyapatite
What will happen to the pH as the tooth enamel is attacked by the acids?
(1)
Int 2 2012
19. A student carried out the following experiment.
(a) During the reaction a solid was formed.
Name the type of chemical reaction taking place
(1)
(b) The equation for the reaction is
Ba2+(aq) + 2Cl-(aq) + 2Na+(aq) + SO42-(aq)  Ba2+ SO42-(s) + 2Cl-(aq) + 2Na+(aq)
(i)
Rewrite the equation showing only the ions which react
(1)
(ii)
What term is used to describe the ions which do not react?
(1)
Nat 5 2014
20. Sodium carbonate solution can be added to the water in swimming pools to neutralise the
acidic effects of chlorine.
A student carried out a titration experiment to determine the concentration of a sodium
carbonate solution
(a) Using the results in the table, calculate the average volume, in cm3, of hydrochloric
acid required to neutralise the sodium carbonate solution.
(1)
(b) The equation for the reaction is
2HCl + Na2CO3  2NaCl + CO2 + H2O
Using your answer from part (a) calculate the concentration, in mol l-1, of the sodium
carbonate solution.
Show your working clearly.
(3)
SG C 2011
21. The salt copper(II) nitrate can be produced as shown.
X + 2HNO3  Cu(NO3)2 + CO2 +H2O
Name substance X
(1)