Edexcel Igcse Chemistry Past Paper Questions 2013 5n113x
This document was ed by and they confirmed that they have the permission to share it. If you are author or own the copyright of this book, please report to us by using this report form. Report 3i3n4
Overview 26281t
& View Edexcel Igcse Chemistry Past Paper Questions 2013 as PDF for free.
More details 6y5l6z
- Words: 4,089
- Pages: 320
Islamia English School
Chemistry past Paper Questions First Term
2013
Guided By Sir.Sadiq Amin
Paper References Acids, Bases, Salts and Titration Calculation Year
Month
Paper
Question Number
Part
2000
January
1
1 4
c a b c d c a b d a b
2000
2001 2001 2002 2004
May
January May May January
1
6 1
1 1 1 1
8 7 13 8
2004
May
1
14 9 14
2005
May
1
15
2006 2006
January May
1 1
2007 2008 2009
May May January
1 1 1
Sub Part
I, ii, iii
a b
I, ii, ii, ii, iv
a a b c d a b
i
iii, iv
7 12 14 15 11 14 1
2009 2010 2010 2011
May January May January
1 1 1 1
2011
May
1
2012
2013
January
1
2012
May
January
1
10 13 3 7 12 3 6 10 11 3 4 1 2 3 8 3
a
I, ii
d e 1 b
Acids, Bases, Salts and Titration Calculation Year
Month
Paper
Question Number
Part
2003
May
2
3
a
2004
January
2
4
a
Sub Part
b 2005
January
2
a b
2005
May
2
6
2006
January
2
2
c
2007
January
2
6
a
I, iii 2
2007
May
2
1
2008
January
2
5
2008
May
2
7
c
7
a
8
b
2009
January
2
8
a
2009
May
2
1
a
7
d
6
a
2010
January
2
I,ii
iii
I, ii
b c 9
a b
2010
May
2
3 5
2011
January
2
3
b
2011
May
2
8
a
i
b d 2012
January
2
3 8
2012
May
2
3
a
2013
January
2
3
c
5 3
7
Halogens Year
Month
Paper
Question Number
Part
2000
January
1
6
a
Sub Part
b 2001
January
1
7
2004
January
1
11
2006
January
1
9
2008
January
1
8
b
a b c
2008
May
1
5
2011
May
1
5
a
2012
May
1
4
d
I, ii, iii
e
Halogens Year
Month
Paper
Question Number
Part
2005
January
2
6
2006
January
2
2
2007
January
2
4
2009
January
2
4
2009
May
2
9
b
2010
January
2
9
b
Sub Part
a
4
2010
May
2
7
b
Reversible Reactions Year
Month
Paper
Question Number
Part
2000
January
1
8
c
2001
January
1
5
a
2001
May
1
3
a
Sub Part
b c 2006
January
1
13
2007
January
1
7
2008
January
1
11
2010
January
1
10
2012
January
1
3
2013
January
1
8
a
I, ii, iii
c
Reversible Reactions Year
Month
Paper
Question Number
Part
2003
May
2
2
b
Sub Part
c 4
d e 5
2004
January
2
6
d
2004
May
2
4
c
I,ii
d 2005
January
2
9
a
2006
May
2
7
a
2007
January
2
5
a b
2007
May
2
7
a
2009
May
2
7
a
2012
May
2
5
d
I,ii
6
7
8
9
Paper 1 Acid, Alkali and Salts and Titration Calculation Monday 17 January 2000 Q1 (c) Describe a chemical test to distinguish between a solution of hydrogen chloride in methylbenzene and a solution of hydrogen chloride in water. Describe the result with each solution.
(3 marks) 4. The acid concentration in red wine can be determined by titration against 0.010 mol dm-3 sodium hydroxide solution. The colour of the red wine is first removed by the use of activated charcoal. One acid present is tartaric acid, which like sulphuric acid has a molecule containing two replaceable protons. (a) Name a suitable indicator for an acid-alkali titration. State the colour of this indicator in acid and alkali solutions. Indicator Color in acid Color in alkali (3 marks) (b) Why is the color of the wine removed before titration?
(1mark) (c) In a titration, 10cm3 of 0.010mol dm-3 sodium hydroxide solution were required to neutralize 25 cm3 of wine. Given that two moles of sodium hydroxide will neutralize one mole of tartaric acid calculate (i) The number of moles of sodium hydroxide used in the titration;
10
(ii) The number of moles of tartaric acid in the volume of wine used in the titration, and the concentration of tartaric acid in mol dm-3.
(3marks) (d) Even if the titration is carried out without experimental error, it gives a too high a value for the real concentration of tartaric acid in the wine. Suggest a reason for this
(1 mark) 6 (c) A sample of sea water contains 0.1g dm-3 of bromide ions. (i)
What volume of sea water produces one mole of bromine molecules?
(ii)
What volume of chlorine gas is required to produce 8g of bromine from this sea water?
(5 marks) 11
Tuesday 23 May 2000 1. This question is about four acids: Ethanoic acid
hydrochloric acid
nitric acid
sulphuric acid
(a) Which of these acids is a weak acid? Explain why this acid is regarded as weak.
(2 marks) (b) Which one of these acids can be used to prepare an acid salt? Give the name of an acid salt and write an equation for its preparation.
(3 marks) (d) In a titration, 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3 were exactly neutralized by 20.0 cm3 of dilute nitric acid. NaOH (aq) + HNO 3 (aq) → NaNO 3 (aq) + H 2 O R
(l)
(i) How many moles of sodium hydroxide are in 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3?
(ii) Calculate the concentration, in mol dm-3, of the dilute nitric acid.
(iii) What volume of this dilute nitric acid would contain exactly 1 mole of hydrogen ions?
(3 marks) 12
Tuesday 16 January 2001 8 (a) Describe how you could use a 0.10 mol dm-3 solution of sodium hydroxide to determine the concentration of a solution of sulphuric acid?
(12 marks) 13
Tuesday 22 May 2001 7 (b) Copper powders do not react with dilute sulphuric acid. Starting with copper powder and dilute sulphuric acid, describe how you would obtain pure dry sample of blue (hydrated) copper (II) sulphate.
(10 marks) 14
Tuesday 21 May 2002 13. The following equation represents the reaction between magnesium oxide and dilute sulphuric acid. MgO (s) + H 2 SO 4(aq) → MgSO 4 (aq) + H 2 O (l) R
(a) What is the relative formula mass of magnesium oxide?
(b) How many moles of sulphuric acid react with 2.0 g of magnesium oxide?
(c) What volume of 2.0mol dm-3 sulphuric acid, in cm3, would be needed to react with 2.0 g of magnesium oxide?
(d) Calculate the mass, in g, of magnesium sulphate crystals, MgSO 4 .7H 2 O, that would be formed by the reaction of 2.0g of magnesium oxide and an excess of dilute sulphuric acid.
(e) Calculate the percentage by mass of magnesium in magnesium sulphate crystals.
(7 marks)
Tuesday 13 January 2004 8 (a) Ammonia can be prepared using an ammonium salt and a strong alkali. (i) Name a suitable strong alkali.
(ii) Write an equation for a reaction that could be used to prepare ammonia gas.
(iii) Concentrated sulphuric acid is a common drying agent for gases. Why it is it not used to dry ammonia?
(iv) Name a suitable drying agent for ammonia. 15
(b) The reaction between ammonia and nitric acid is represented by the equation NH 3 (g) +HNO 3 (aq) → NH 4 NO 3 (aq) R
Calculate the mass of ammonia, in grams that would be required to neutralize 50 cm3 of nitric acid of concentration of 2 mol dm-3. (i) Number of moles of nitric acid in 50 cm3 =
(ii) Mass of ammonia =
14. A student was asked to find the relative molecular mass of a solid acid. She weighed out accurately a sample of the acid and then made 250 cm3 of solution in a graduated flask. She took 25.0 cm3 portions of the solution and titrated them against aqueous sodium hydroxide of concentration 0.20 mol dm-3 which was contained in a burette. Phenolphthalein was used as the indicator. (a) (i) What would have been the colour change for phenolphthalein at the end – point?
(ii) Why was phenolphthalein used rather than universal indicator?
(iii) Give the name of the piece of apparatus that the student would have used to accurately transfer 25.0 cm3 of acid from the graduated flask.
(b) The following results were recorded:
Table 1 Mass of weighing bottle + sample of acid Mass of weighing bottle empty Mass of sample acid Final burette reading/ cm3 Initial burette reading/ cm3 Volume of NaOH added/cm3
23.45 0.00
= = =
Table 2 23.75 1.20
23.10 0.65
16
(i) Complete Tables 1 and 2 to show the mass of acid used and the volume of sodium hydroxide in each titration. (ii) Decide which titration figures should be used to calculate the most accurate mean value for the volume sodium hydroxide added and then perform the calculation.
Titration figures used to calculate the mean:
Mean Value:
(c) Using A to represent the anion of the acid, the equation for the reaction is H 2 A + 2NaOH → Na 2 A + 2H 2 O
(i) The concentration of sodium hydroxide was 0.20 mol dm-3. How many moles of sodium hydroxide were present in the mean volume?
(ii) Use the mole ratio from the equation to determine how many moles of acids reacted with this number of sodium hydroxide. The value obtained is equal to the number of moles of acid in 25.0 cm3 of solution.
(iii) How many moles of acids were present in 250 cm3 of solution?
(iv) Use the number moles of acid in 250 cm3 of solution and the mass of the acid to calculate the relative formula mass.
(12 marks)
17
Tuesday 18 May 2004 9 (b) Two solutions of hydrogen chloride were prepared. Solution X was a solution in methylbenzene, an organic solvent. Solution Y was a solution in water. (i) Solid sodium chloride was added to a sample of each solution. No reaction was observed with solution X but effervescence occurred with solution Y. Explain the difference in behavior of the two solutions.
14.In an experiment, two plugs of cotton wool soaked respectively in concentrated aqueous ammonia and concentrated hydrochloric acid was placed at either end of a long glass tube. After a short time, white ‘smoke’ was observed in the tube.
(a) Ammonia gas is produced at the plug of cotton wool soaked in concentrated aqueous ammonia. Name the gas produced at the plug of cotton wool soaked in concentrated hydrochloric acid.
(b) Name the process by which the gases move through the tube.
(c) Write a sentence comparing the relative speeds with which the gases move along the tube.
(d) Give the formula of the chemical responsible for the white smoke.
18
Tuesday 18 January 2005 (No questions related to Acids, bases, salts and titration calculation.)
Tuesday 17 May 2005 15 (a) Magnesium react with dilute sulphuric acid to produce hydrogen gas. Write an equation for this reaction.
(b) In an experiment, x g of magnesium was added to excess dilute sulphuric acid of concentration 1moldm-3. The reaction stopped after 100 s and produced 120 cm3 of hydrogen gas measured at room temperature and normal atmospheric pressure. (iii) Calculate the value of x.
(iv) Calculate the volume of dilute sulphuric acid of concentration 1 mol dm-3 that reacted with x g of magnesium in the experiment.
Tuesday 17 January 2006 7. Sulphamic acid, NH 2 SO 3 H, is a weak acid that is used to remove lime scale, calcium carbonate from shower heads. The equation for the reaction is: CaCO 3 (s) + 2NH 2 SO 3 H (aq) → Ca(NH 2 SO 3 ) 2 (aq) + CO 2 (g) + H 2 O (l) R
(a) Describe a test to show that the Sulphamic acid is a weak acid.
(b) Describe a test to show that the gas evolved is carbon dioxide.
(c) Calculate the relative atomic mass of Sulphamic acid. 19
(d) Calculate the mass of Sulphamic acid needed to remove 1.0g of lime scale.
(Total 7 marks)
Tuesday 16 May 2006 12. A group two metal carbonate, MCO 3 reacts with dilute hydrochloric acid according to the following equation. MCO 3 + 2HCl → MCl 2 + H 2 O + CO 2
When 2.5 g of the metal carbonate was added to an excess of dilute hydrochloric acid, 600 cm3 of carbon dioxide gas was produced, measured at room temperature and atmospheric pressure. (a) How many moles of carbon dioxide were formed?
(b) Use your answer to (a) and the equation to deduce how many moles of the metal carbonate are equivalent to 2.5 g.
(c) Calculate the mass of one mole of MCO 3.
(d) Find the relative atomic mass of M and identify the metal.
(e) Give details of simple test you would carry out to confirm the identity of metal M.
(Total 8 marks)
20
14. When hydrated zinc sulphate is heated, it loses water to become anhydrous zinc sulphate. ZnSO 4 .xH 2 O → ZnSO 4 + xH 2 O
A sample of hydrated zinc sulphate was placed in an evaporating basin and heated until all the water had been lost. The following masses were recorded. Mass of evaporating dish when empty = 34.63 g Mass of evaporating basin +hydrated zinc sulphate = 40.37 Mass of evaporating basin + anhydrous zinc sulphate = 37.85 g (a) Calculate the relative formula mass of anhydrous zinc sulphate, ZnSO 4.
(b) (i) What mass of anhydrous zinc sulphate was formed?
(ii) What mass of water was lost?
(iii) Calculate the value of x in the formula ZnSO 4 .xH 2 O.
(Total 6 marks)
Tuesday 18 January 2007 (No questions related to Acids, bases, salts and titration calculation.)
21
Tuesday 15 May 2007
22
23
Monday 14 January 2008 (No questions related to Acids, bases, salts and titration calculation.)
Tuesday 13 May 2008
24
Wednesday 14 January 2009
25
Wednesday 20 May 2009
26
Wednesday 13 January 2010
27
28
Tuesday 25 May 2010
Wednesday 12 January 2011
29
30
31
32
Wednesday 25 May 2011
33
34
35
36
37
38
39
Friday 13 January 2012
40
41
42
Monday 21 May 2012
43
44
45
46
47
48
Monday 14 January 2013
49
50
Paper 2 Acid, Alkali and Salts and Titration Calculation Thursday 22 May 2003 3. Silver nitrate solution is used as a reagent in the laboratory. (a) Starting with solid silver nitrate, describe how you would prepare exactly 100 cm3 of silver nitrate solution of concentration 0.01 mol dm-3. You should give sufficient detail to allow another chemist to repeat your method.
(5 marks)
Thursday 15 January 2004 4. Nickel, Ni, is a transition metal in the same row of the Periodic Table as copper. (a) Describe, giving essential details, how you could prepare crystals of nickel (II) sulphate, NiSO 4 .6H 2 O, starting from nickel (II) oxide and dilute sulphuric acid. (Diagrams not required) Method
51
(5 marks) (b) The overall equation for the preparation is: NiO (s) + H 2 SO 4 (aq) 5H 2 O (l) → NiSO 4 .6H 2 O (s) R
Use the equation to calculate the maximum mass, in grams, of nickel (II) sulphate crystals that could be obtained from 3.75g of nickel (II) oxide.
(3 marks)
Thursday 20 May 2004 (No questions related to Acids, bases, salts and titration calculation.)
Thursday 20 January 2005 8 (a) (i) Describe, giving essential practical details, how you would perform a titration to find the concentration, in mol dm-3, of a solution of sulphuric acid. You are provided with aqueous sodium hydroxide of concentration 0.50 mol dm-3 and phenolphthalein indicator.
52
(ii) The equation for the reaction between sodium hydroxide and sulphuric acid is H 2 SO 4 + 2NaOH → Na 2 SO 4 + 2H 2 O
In a titration, 25.0 cm3 of H 2 SO 4 required 26.5 cm3 of 0.50 mol dm-3 NaOH for neutralization. Calculate the concentration of H 2 SO 4 in mol dm-3.
(iii) Sodium sulphate forms crystals of formula Na 2 SO 4 .x2H 2 O. Describe briefly how a sample of the pure, dry crystals can be obtained (use the information given in (ii) above).
(16 marks) (b) 6.44g of Na 2 SO 4. x2H 2 O was heated to remove the water of crystallization and a loss in mass of 3.60g was recorded. Use these figures to calculate the number of moles of water of crystallization, x, in 1 mole of Na 2 SO 4. x2H 2 O.
53
(4 marks)
Thursday May 2005
54
55
Thursday 19 January 2006 2.
56
Thursday 18 May 2006 (No questions related to Acids, bases, salts and titration calculation.)
Monday 22 January 2007
57
Thursday 17 May 2007
58
Thursday 17 January 2008 59
60
61
7.
62
Thursday 15 May 2008
63
8.
64
Monday 19 January 2009 8.
Friday 22 May 2009
65
7.
66
Monday 18 January 2010
67
68
69
Friday 28 May 2010
70
71
72
Monday 17 January 2011 3.
73
Wednesday 15 June 2011
74
75
76
Friday 20 January 2012
77
78
Tuesday 29 May 2012
79
Wednesday 16 January 2013 3.
80
81
82
83
84
85
Paper 1 Halogens Monday 17 January 2000
(5 marks)
Tuesday 23 May 2000 (No questions related to Halogens.)
86
Tuesday 16 January 2001 7.
Tuesday 22 May 2001 (No questions related to Halogens.)
Tuesday 21 May 2002 (No questions related to Halogens.)
Tuesday 20 May 2003 (No questions related to Halogens.)
Tuesday 13 January 2004
87
Tuesday 18 May 2004 (No questions related to Halogens.)
Tuesday 18 January 2005 (No questions related to Halogens.)
Tuesday 17 January 2006
(Total 5 marks)
Tuesday 16 May 2006 (No questions related to Halogens.)
88
Thursday 18 January 2007 (No questions related to Halogens.)
Tuesday 15 May 2007 (No questions related to Halogens.)
Monday 14 January 2008
89
Tuesday 13 May 2008
90
Wednesday 14 January 2009 (No questions related to Halogens.)
Wednesday 20 May 2009 (No questions related to Halogens.)
Wednesday 13 January 2010 (No questions related to Halogens.)
Tuesday 25 May 2010 (No questions related to Halogens.)
Wednesday 12 January 2011 (No questions related to Halogens.)
Wednesday 25 May 2011
91
Friday 13 January 2012 (No questions related to Halogens.)
Monday 21 May 2012 4.
Monday 14 January 2013 (No questions related to Halogens.)
92
Paper 2 Halogens
Thursday 22 May 2003 (No questions related to Halogens.)
Thursday 15 January 2004 (No questions related to Halogens.)
Thursday 20 May 2004 (No questions related to Halogens.)
Thursday 20 January 2005
93
94
(25 MARKS)
Thursday 19 May 2005 (No questions related to Halogens.)
Thursday 19 January 2006
Thursday May 2006 (No questions related to Halogens.)
95
Monday 22 January 2007
96
Thursday 17 May 2007 (No questions related to Halogens.)
Thursday 17 January 2008 (No questions related to Halogens.)
Thursday 15 May 2008 (No questions related to Halogens.)
Monday 19 January 2009
97
Friday 22 May 2009
98
Monday 18 January 2010
99
Friday 18 May 2010 7.
Monday 17 January 2011 (No questions related to Halogens.)
Wednesday 15 June 2011 (No questions related to Halogens.)
Friday 20 January 2012 (No questions related to Halogens.)
Tuesday 29 May 2012 (No questions related to Halogens.)
Wednesday 16 January 2013 (No questions related to Halogens.)
100
Paper 1 Reversible Reactions
Monday 17 January 2000 8.
Tuesday 23 May 2000 (No questions related to Reversible Reactions.)
Tuesday 16 January 2001
101
Tuesday 22 May 2001
102
Tuesday 21 May 2002 (No questions related to Reversible Reactions.)
Tuesday 20 May 2003 (No questions related to Reversible Reactions.)
Tuesday 13 January 2004 (No questions related to Reversible Reactions.)
Tuesday 18 January 2003 (No questions related to Reversible Reactions.)
Tuesday 17 May 2005 (No questions related to Reversible Reactions.)
Tuesday 17 January 2006
103
(Total 10 Marks)
Tuesday 16 May 2006 (No questions related to Reversible Reactions.)
Thursday 18 January 2007
104
Tuesday 15 May 2007 (No questions related to Reversible Reactions.)
Monday 14 January 2008
105
Tuesday 13 May 2008 (No questions related to Reversible Reactions.)
Wednesday 14 January 2009 (No questions related to Reversible Reactions.)
Wednesday 20 May 2009 (No questions related to Reversible Reactions.)
Wednesday 13 January 2010
106
Tuesday 25 May 2010 (No questions related to Reversible Reactions.)
Wednesday 12 January 2011 (No questions related to Reversible Reactions.) 107
Wednesday 25 May 2011 (No questions related to Reversible Reactions.)
Friday 13 January 2012 3.
Monday 21 May 2012 (No questions related to Reversible Reactions.)
Monday 14 January 2013
108
109
Paper 2 Reversible Reactions
Thursday 22 May 2003 2.
110
111
Thursday 15 January 2004 6.
Thursday 20 May 2004 4.
112
Thursday 20 January 2005
113
Thursday 19 May 2005 (No questions related to Reversible Reactions.)
Thursday 19 January 2006 (No questions related to Reversible Reactions.)
Thursday 18 May 2006
114
Monday 22 January 2007
115
116
Thursday 17 May 2007
Thursday 17 January 2008 (No questions related to Reversible Reactions.)
Monday 19 January 2009 (No questions related to Reversible Reactions.)
117
Friday 22 May 2009
Monday 18 January 2010 (No questions related to Reversible Reactions.)
118
Friday 28 May 2010 (No questions related to Reversible Reactions.)
Monday 17 January 2011 (No questions related to Reversible Reactions.)
Wednesday 15 June 2011 (No questions related to Reversible Reactions.)
Friday 20 January 2012 (No questions related to Reversible Reactions.)
Tuesday 29 May 2012 5.
119
Wednesday 16 January 2013 (No questions related to Reversible Reactions.)
120
Group Information
Group Leader: Abdullah Al Abid Mohammad Tofazzal Hossain Bhuyian
Also In the Group
Abdul Haleem Abdul Kareem Ikramullah Arifulla Haider Ali Baqwi Mohammad Zain Shakeel Mohammad Anas Kareem Ahmed Bin Rashid Irshad Mohammad Rehan Sandhu
121
CHEMISTRY PAST PAPER QEUSTIONS AND REFERENCES FOR TERM 3 Topics from term 3 Reactivity series Test for ions and gases
Extraction for metals
Project Done By Hudais khan, Hamid Hasan, Hamza Shams, Ahmed Ifthikar, Israr Ahmed, Saleem Khan, Shabbir Hossain and Abdul Khaleel Talha
REACTIVITY SERIES Paper
Month
Year
Question
Sub Part
1
May
2000
5
1
May
2001
9
(b)
1
May
2004
17
(a)(b)
1
May
2005
5
1
May
2007
5
1
May
2010
6
1
May
2012
2
1
January
2013
6
2
May
2008
7
2
June
2011
1
(a)(i)(ii)(iii)
(b)
rusting of iron Paper
Month
Year
Question
Sub Part
1
May
2004
17
( c)
1
May
2006
16
1
January
2007
3
1
January
2009
9
1
May
2009
7
1
May
2011
7
1
January
2012
2
1
January
2013
4
2
January
2011
6
(b)
Oxidation & reduction Paper
Month
Year
Question
1
January
2006
9
1
January
2008
8
1
May
2008
5
1
January
2011
8
Sub Part
(a)(b)(i)(ii)
Extraction of metals Paper
Month
Year
Question
Sub Part
1
January
2000
7
(a)
1
May
2001
6
(a)(b)( c )
1
January
2001
9
(a)
1
May
2002
7
1
May
2002
14
1
January
2005
7
1
January
2007
12
1
January
2008
8
1
May
2008
12
1
May
2011
9
1
May
2012
12
(a)(b)
1
January
2013
7
(a)
2
May
2005
7
(a)
2
January
2006
6
(a)
2
May
2006
6
(a)
2
May
2007
9
(a)
2
May
2008
6
(a)
2
May
2009
6
(a)(i)(iii)
2
January
2010
8
(a)
2
May
2010
7
(a)(iii)
2
January
2011
6
(a)
2
May
2012
2
(d)
test for ions & Preparation and test for gases
Paper
Month
Year
Question
Sub Part
1
May
2000
8
(e)
1
January
2001
3
1
May
2001
2
1
May
2001
6
1
May
2003
8
1
May
2003
10
1
May
2005
13
1
May
2006
7
1
January
2008
12
1
January
2012
3
1
May
2012
11
2
May
2007
1
2
January
2009
1
2
May
2010
9
(d)(ii)
(a)(b)
(a)(b)
Chemistry past Paper Questions First Term
2013
Guided By Sir.Sadiq Amin
Paper References Acids, Bases, Salts and Titration Calculation Year
Month
Paper
Question Number
Part
2000
January
1
1 4
c a b c d c a b d a b
2000
2001 2001 2002 2004
May
January May May January
1
6 1
1 1 1 1
8 7 13 8
2004
May
1
14 9 14
2005
May
1
15
2006 2006
January May
1 1
2007 2008 2009
May May January
1 1 1
Sub Part
I, ii, iii
a b
I, ii, ii, ii, iv
a a b c d a b
i
iii, iv
7 12 14 15 11 14 1
2009 2010 2010 2011
May January May January
1 1 1 1
2011
May
1
2012
2013
January
1
2012
May
January
1
10 13 3 7 12 3 6 10 11 3 4 1 2 3 8 3
a
I, ii
d e 1 b
Acids, Bases, Salts and Titration Calculation Year
Month
Paper
Question Number
Part
2003
May
2
3
a
2004
January
2
4
a
Sub Part
b 2005
January
2
a b
2005
May
2
6
2006
January
2
2
c
2007
January
2
6
a
I, iii 2
2007
May
2
1
2008
January
2
5
2008
May
2
7
c
7
a
8
b
2009
January
2
8
a
2009
May
2
1
a
7
d
6
a
2010
January
2
I,ii
iii
I, ii
b c 9
a b
2010
May
2
3 5
2011
January
2
3
b
2011
May
2
8
a
i
b d 2012
January
2
3 8
2012
May
2
3
a
2013
January
2
3
c
5 3
7
Halogens Year
Month
Paper
Question Number
Part
2000
January
1
6
a
Sub Part
b 2001
January
1
7
2004
January
1
11
2006
January
1
9
2008
January
1
8
b
a b c
2008
May
1
5
2011
May
1
5
a
2012
May
1
4
d
I, ii, iii
e
Halogens Year
Month
Paper
Question Number
Part
2005
January
2
6
2006
January
2
2
2007
January
2
4
2009
January
2
4
2009
May
2
9
b
2010
January
2
9
b
Sub Part
a
4
2010
May
2
7
b
Reversible Reactions Year
Month
Paper
Question Number
Part
2000
January
1
8
c
2001
January
1
5
a
2001
May
1
3
a
Sub Part
b c 2006
January
1
13
2007
January
1
7
2008
January
1
11
2010
January
1
10
2012
January
1
3
2013
January
1
8
a
I, ii, iii
c
Reversible Reactions Year
Month
Paper
Question Number
Part
2003
May
2
2
b
Sub Part
c 4
d e 5
2004
January
2
6
d
2004
May
2
4
c
I,ii
d 2005
January
2
9
a
2006
May
2
7
a
2007
January
2
5
a b
2007
May
2
7
a
2009
May
2
7
a
2012
May
2
5
d
I,ii
6
7
8
9
Paper 1 Acid, Alkali and Salts and Titration Calculation Monday 17 January 2000 Q1 (c) Describe a chemical test to distinguish between a solution of hydrogen chloride in methylbenzene and a solution of hydrogen chloride in water. Describe the result with each solution.
(3 marks) 4. The acid concentration in red wine can be determined by titration against 0.010 mol dm-3 sodium hydroxide solution. The colour of the red wine is first removed by the use of activated charcoal. One acid present is tartaric acid, which like sulphuric acid has a molecule containing two replaceable protons. (a) Name a suitable indicator for an acid-alkali titration. State the colour of this indicator in acid and alkali solutions. Indicator Color in acid Color in alkali (3 marks) (b) Why is the color of the wine removed before titration?
(1mark) (c) In a titration, 10cm3 of 0.010mol dm-3 sodium hydroxide solution were required to neutralize 25 cm3 of wine. Given that two moles of sodium hydroxide will neutralize one mole of tartaric acid calculate (i) The number of moles of sodium hydroxide used in the titration;
10
(ii) The number of moles of tartaric acid in the volume of wine used in the titration, and the concentration of tartaric acid in mol dm-3.
(3marks) (d) Even if the titration is carried out without experimental error, it gives a too high a value for the real concentration of tartaric acid in the wine. Suggest a reason for this
(1 mark) 6 (c) A sample of sea water contains 0.1g dm-3 of bromide ions. (i)
What volume of sea water produces one mole of bromine molecules?
(ii)
What volume of chlorine gas is required to produce 8g of bromine from this sea water?
(5 marks) 11
Tuesday 23 May 2000 1. This question is about four acids: Ethanoic acid
hydrochloric acid
nitric acid
sulphuric acid
(a) Which of these acids is a weak acid? Explain why this acid is regarded as weak.
(2 marks) (b) Which one of these acids can be used to prepare an acid salt? Give the name of an acid salt and write an equation for its preparation.
(3 marks) (d) In a titration, 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3 were exactly neutralized by 20.0 cm3 of dilute nitric acid. NaOH (aq) + HNO 3 (aq) → NaNO 3 (aq) + H 2 O R
(l)
(i) How many moles of sodium hydroxide are in 25.0 cm3 of sodium hydroxide solution of concentration 1.0 mol dm-3?
(ii) Calculate the concentration, in mol dm-3, of the dilute nitric acid.
(iii) What volume of this dilute nitric acid would contain exactly 1 mole of hydrogen ions?
(3 marks) 12
Tuesday 16 January 2001 8 (a) Describe how you could use a 0.10 mol dm-3 solution of sodium hydroxide to determine the concentration of a solution of sulphuric acid?
(12 marks) 13
Tuesday 22 May 2001 7 (b) Copper powders do not react with dilute sulphuric acid. Starting with copper powder and dilute sulphuric acid, describe how you would obtain pure dry sample of blue (hydrated) copper (II) sulphate.
(10 marks) 14
Tuesday 21 May 2002 13. The following equation represents the reaction between magnesium oxide and dilute sulphuric acid. MgO (s) + H 2 SO 4(aq) → MgSO 4 (aq) + H 2 O (l) R
(a) What is the relative formula mass of magnesium oxide?
(b) How many moles of sulphuric acid react with 2.0 g of magnesium oxide?
(c) What volume of 2.0mol dm-3 sulphuric acid, in cm3, would be needed to react with 2.0 g of magnesium oxide?
(d) Calculate the mass, in g, of magnesium sulphate crystals, MgSO 4 .7H 2 O, that would be formed by the reaction of 2.0g of magnesium oxide and an excess of dilute sulphuric acid.
(e) Calculate the percentage by mass of magnesium in magnesium sulphate crystals.
(7 marks)
Tuesday 13 January 2004 8 (a) Ammonia can be prepared using an ammonium salt and a strong alkali. (i) Name a suitable strong alkali.
(ii) Write an equation for a reaction that could be used to prepare ammonia gas.
(iii) Concentrated sulphuric acid is a common drying agent for gases. Why it is it not used to dry ammonia?
(iv) Name a suitable drying agent for ammonia. 15
(b) The reaction between ammonia and nitric acid is represented by the equation NH 3 (g) +HNO 3 (aq) → NH 4 NO 3 (aq) R
Calculate the mass of ammonia, in grams that would be required to neutralize 50 cm3 of nitric acid of concentration of 2 mol dm-3. (i) Number of moles of nitric acid in 50 cm3 =
(ii) Mass of ammonia =
14. A student was asked to find the relative molecular mass of a solid acid. She weighed out accurately a sample of the acid and then made 250 cm3 of solution in a graduated flask. She took 25.0 cm3 portions of the solution and titrated them against aqueous sodium hydroxide of concentration 0.20 mol dm-3 which was contained in a burette. Phenolphthalein was used as the indicator. (a) (i) What would have been the colour change for phenolphthalein at the end – point?
(ii) Why was phenolphthalein used rather than universal indicator?
(iii) Give the name of the piece of apparatus that the student would have used to accurately transfer 25.0 cm3 of acid from the graduated flask.
(b) The following results were recorded:
Table 1 Mass of weighing bottle + sample of acid Mass of weighing bottle empty Mass of sample acid Final burette reading/ cm3 Initial burette reading/ cm3 Volume of NaOH added/cm3
23.45 0.00
= = =
Table 2 23.75 1.20
23.10 0.65
16
(i) Complete Tables 1 and 2 to show the mass of acid used and the volume of sodium hydroxide in each titration. (ii) Decide which titration figures should be used to calculate the most accurate mean value for the volume sodium hydroxide added and then perform the calculation.
Titration figures used to calculate the mean:
Mean Value:
(c) Using A to represent the anion of the acid, the equation for the reaction is H 2 A + 2NaOH → Na 2 A + 2H 2 O
(i) The concentration of sodium hydroxide was 0.20 mol dm-3. How many moles of sodium hydroxide were present in the mean volume?
(ii) Use the mole ratio from the equation to determine how many moles of acids reacted with this number of sodium hydroxide. The value obtained is equal to the number of moles of acid in 25.0 cm3 of solution.
(iii) How many moles of acids were present in 250 cm3 of solution?
(iv) Use the number moles of acid in 250 cm3 of solution and the mass of the acid to calculate the relative formula mass.
(12 marks)
17
Tuesday 18 May 2004 9 (b) Two solutions of hydrogen chloride were prepared. Solution X was a solution in methylbenzene, an organic solvent. Solution Y was a solution in water. (i) Solid sodium chloride was added to a sample of each solution. No reaction was observed with solution X but effervescence occurred with solution Y. Explain the difference in behavior of the two solutions.
14.In an experiment, two plugs of cotton wool soaked respectively in concentrated aqueous ammonia and concentrated hydrochloric acid was placed at either end of a long glass tube. After a short time, white ‘smoke’ was observed in the tube.
(a) Ammonia gas is produced at the plug of cotton wool soaked in concentrated aqueous ammonia. Name the gas produced at the plug of cotton wool soaked in concentrated hydrochloric acid.
(b) Name the process by which the gases move through the tube.
(c) Write a sentence comparing the relative speeds with which the gases move along the tube.
(d) Give the formula of the chemical responsible for the white smoke.
18
Tuesday 18 January 2005 (No questions related to Acids, bases, salts and titration calculation.)
Tuesday 17 May 2005 15 (a) Magnesium react with dilute sulphuric acid to produce hydrogen gas. Write an equation for this reaction.
(b) In an experiment, x g of magnesium was added to excess dilute sulphuric acid of concentration 1moldm-3. The reaction stopped after 100 s and produced 120 cm3 of hydrogen gas measured at room temperature and normal atmospheric pressure. (iii) Calculate the value of x.
(iv) Calculate the volume of dilute sulphuric acid of concentration 1 mol dm-3 that reacted with x g of magnesium in the experiment.
Tuesday 17 January 2006 7. Sulphamic acid, NH 2 SO 3 H, is a weak acid that is used to remove lime scale, calcium carbonate from shower heads. The equation for the reaction is: CaCO 3 (s) + 2NH 2 SO 3 H (aq) → Ca(NH 2 SO 3 ) 2 (aq) + CO 2 (g) + H 2 O (l) R
(a) Describe a test to show that the Sulphamic acid is a weak acid.
(b) Describe a test to show that the gas evolved is carbon dioxide.
(c) Calculate the relative atomic mass of Sulphamic acid. 19
(d) Calculate the mass of Sulphamic acid needed to remove 1.0g of lime scale.
(Total 7 marks)
Tuesday 16 May 2006 12. A group two metal carbonate, MCO 3 reacts with dilute hydrochloric acid according to the following equation. MCO 3 + 2HCl → MCl 2 + H 2 O + CO 2
When 2.5 g of the metal carbonate was added to an excess of dilute hydrochloric acid, 600 cm3 of carbon dioxide gas was produced, measured at room temperature and atmospheric pressure. (a) How many moles of carbon dioxide were formed?
(b) Use your answer to (a) and the equation to deduce how many moles of the metal carbonate are equivalent to 2.5 g.
(c) Calculate the mass of one mole of MCO 3.
(d) Find the relative atomic mass of M and identify the metal.
(e) Give details of simple test you would carry out to confirm the identity of metal M.
(Total 8 marks)
20
14. When hydrated zinc sulphate is heated, it loses water to become anhydrous zinc sulphate. ZnSO 4 .xH 2 O → ZnSO 4 + xH 2 O
A sample of hydrated zinc sulphate was placed in an evaporating basin and heated until all the water had been lost. The following masses were recorded. Mass of evaporating dish when empty = 34.63 g Mass of evaporating basin +hydrated zinc sulphate = 40.37 Mass of evaporating basin + anhydrous zinc sulphate = 37.85 g (a) Calculate the relative formula mass of anhydrous zinc sulphate, ZnSO 4.
(b) (i) What mass of anhydrous zinc sulphate was formed?
(ii) What mass of water was lost?
(iii) Calculate the value of x in the formula ZnSO 4 .xH 2 O.
(Total 6 marks)
Tuesday 18 January 2007 (No questions related to Acids, bases, salts and titration calculation.)
21
Tuesday 15 May 2007
22
23
Monday 14 January 2008 (No questions related to Acids, bases, salts and titration calculation.)
Tuesday 13 May 2008
24
Wednesday 14 January 2009
25
Wednesday 20 May 2009
26
Wednesday 13 January 2010
27
28
Tuesday 25 May 2010
Wednesday 12 January 2011
29
30
31
32
Wednesday 25 May 2011
33
34
35
36
37
38
39
Friday 13 January 2012
40
41
42
Monday 21 May 2012
43
44
45
46
47
48
Monday 14 January 2013
49
50
Paper 2 Acid, Alkali and Salts and Titration Calculation Thursday 22 May 2003 3. Silver nitrate solution is used as a reagent in the laboratory. (a) Starting with solid silver nitrate, describe how you would prepare exactly 100 cm3 of silver nitrate solution of concentration 0.01 mol dm-3. You should give sufficient detail to allow another chemist to repeat your method.
(5 marks)
Thursday 15 January 2004 4. Nickel, Ni, is a transition metal in the same row of the Periodic Table as copper. (a) Describe, giving essential details, how you could prepare crystals of nickel (II) sulphate, NiSO 4 .6H 2 O, starting from nickel (II) oxide and dilute sulphuric acid. (Diagrams not required) Method
51
(5 marks) (b) The overall equation for the preparation is: NiO (s) + H 2 SO 4 (aq) 5H 2 O (l) → NiSO 4 .6H 2 O (s) R
Use the equation to calculate the maximum mass, in grams, of nickel (II) sulphate crystals that could be obtained from 3.75g of nickel (II) oxide.
(3 marks)
Thursday 20 May 2004 (No questions related to Acids, bases, salts and titration calculation.)
Thursday 20 January 2005 8 (a) (i) Describe, giving essential practical details, how you would perform a titration to find the concentration, in mol dm-3, of a solution of sulphuric acid. You are provided with aqueous sodium hydroxide of concentration 0.50 mol dm-3 and phenolphthalein indicator.
52
(ii) The equation for the reaction between sodium hydroxide and sulphuric acid is H 2 SO 4 + 2NaOH → Na 2 SO 4 + 2H 2 O
In a titration, 25.0 cm3 of H 2 SO 4 required 26.5 cm3 of 0.50 mol dm-3 NaOH for neutralization. Calculate the concentration of H 2 SO 4 in mol dm-3.
(iii) Sodium sulphate forms crystals of formula Na 2 SO 4 .x2H 2 O. Describe briefly how a sample of the pure, dry crystals can be obtained (use the information given in (ii) above).
(16 marks) (b) 6.44g of Na 2 SO 4. x2H 2 O was heated to remove the water of crystallization and a loss in mass of 3.60g was recorded. Use these figures to calculate the number of moles of water of crystallization, x, in 1 mole of Na 2 SO 4. x2H 2 O.
53
(4 marks)
Thursday May 2005
54
55
Thursday 19 January 2006 2.
56
Thursday 18 May 2006 (No questions related to Acids, bases, salts and titration calculation.)
Monday 22 January 2007
57
Thursday 17 May 2007
58
Thursday 17 January 2008 59
60
61
7.
62
Thursday 15 May 2008
63
8.
64
Monday 19 January 2009 8.
Friday 22 May 2009
65
7.
66
Monday 18 January 2010
67
68
69
Friday 28 May 2010
70
71
72
Monday 17 January 2011 3.
73
Wednesday 15 June 2011
74
75
76
Friday 20 January 2012
77
78
Tuesday 29 May 2012
79
Wednesday 16 January 2013 3.
80
81
82
83
84
85
Paper 1 Halogens Monday 17 January 2000
(5 marks)
Tuesday 23 May 2000 (No questions related to Halogens.)
86
Tuesday 16 January 2001 7.
Tuesday 22 May 2001 (No questions related to Halogens.)
Tuesday 21 May 2002 (No questions related to Halogens.)
Tuesday 20 May 2003 (No questions related to Halogens.)
Tuesday 13 January 2004
87
Tuesday 18 May 2004 (No questions related to Halogens.)
Tuesday 18 January 2005 (No questions related to Halogens.)
Tuesday 17 January 2006
(Total 5 marks)
Tuesday 16 May 2006 (No questions related to Halogens.)
88
Thursday 18 January 2007 (No questions related to Halogens.)
Tuesday 15 May 2007 (No questions related to Halogens.)
Monday 14 January 2008
89
Tuesday 13 May 2008
90
Wednesday 14 January 2009 (No questions related to Halogens.)
Wednesday 20 May 2009 (No questions related to Halogens.)
Wednesday 13 January 2010 (No questions related to Halogens.)
Tuesday 25 May 2010 (No questions related to Halogens.)
Wednesday 12 January 2011 (No questions related to Halogens.)
Wednesday 25 May 2011
91
Friday 13 January 2012 (No questions related to Halogens.)
Monday 21 May 2012 4.
Monday 14 January 2013 (No questions related to Halogens.)
92
Paper 2 Halogens
Thursday 22 May 2003 (No questions related to Halogens.)
Thursday 15 January 2004 (No questions related to Halogens.)
Thursday 20 May 2004 (No questions related to Halogens.)
Thursday 20 January 2005
93
94
(25 MARKS)
Thursday 19 May 2005 (No questions related to Halogens.)
Thursday 19 January 2006
Thursday May 2006 (No questions related to Halogens.)
95
Monday 22 January 2007
96
Thursday 17 May 2007 (No questions related to Halogens.)
Thursday 17 January 2008 (No questions related to Halogens.)
Thursday 15 May 2008 (No questions related to Halogens.)
Monday 19 January 2009
97
Friday 22 May 2009
98
Monday 18 January 2010
99
Friday 18 May 2010 7.
Monday 17 January 2011 (No questions related to Halogens.)
Wednesday 15 June 2011 (No questions related to Halogens.)
Friday 20 January 2012 (No questions related to Halogens.)
Tuesday 29 May 2012 (No questions related to Halogens.)
Wednesday 16 January 2013 (No questions related to Halogens.)
100
Paper 1 Reversible Reactions
Monday 17 January 2000 8.
Tuesday 23 May 2000 (No questions related to Reversible Reactions.)
Tuesday 16 January 2001
101
Tuesday 22 May 2001
102
Tuesday 21 May 2002 (No questions related to Reversible Reactions.)
Tuesday 20 May 2003 (No questions related to Reversible Reactions.)
Tuesday 13 January 2004 (No questions related to Reversible Reactions.)
Tuesday 18 January 2003 (No questions related to Reversible Reactions.)
Tuesday 17 May 2005 (No questions related to Reversible Reactions.)
Tuesday 17 January 2006
103
(Total 10 Marks)
Tuesday 16 May 2006 (No questions related to Reversible Reactions.)
Thursday 18 January 2007
104
Tuesday 15 May 2007 (No questions related to Reversible Reactions.)
Monday 14 January 2008
105
Tuesday 13 May 2008 (No questions related to Reversible Reactions.)
Wednesday 14 January 2009 (No questions related to Reversible Reactions.)
Wednesday 20 May 2009 (No questions related to Reversible Reactions.)
Wednesday 13 January 2010
106
Tuesday 25 May 2010 (No questions related to Reversible Reactions.)
Wednesday 12 January 2011 (No questions related to Reversible Reactions.) 107
Wednesday 25 May 2011 (No questions related to Reversible Reactions.)
Friday 13 January 2012 3.
Monday 21 May 2012 (No questions related to Reversible Reactions.)
Monday 14 January 2013
108
109
Paper 2 Reversible Reactions
Thursday 22 May 2003 2.
110
111
Thursday 15 January 2004 6.
Thursday 20 May 2004 4.
112
Thursday 20 January 2005
113
Thursday 19 May 2005 (No questions related to Reversible Reactions.)
Thursday 19 January 2006 (No questions related to Reversible Reactions.)
Thursday 18 May 2006
114
Monday 22 January 2007
115
116
Thursday 17 May 2007
Thursday 17 January 2008 (No questions related to Reversible Reactions.)
Monday 19 January 2009 (No questions related to Reversible Reactions.)
117
Friday 22 May 2009
Monday 18 January 2010 (No questions related to Reversible Reactions.)
118
Friday 28 May 2010 (No questions related to Reversible Reactions.)
Monday 17 January 2011 (No questions related to Reversible Reactions.)
Wednesday 15 June 2011 (No questions related to Reversible Reactions.)
Friday 20 January 2012 (No questions related to Reversible Reactions.)
Tuesday 29 May 2012 5.
119
Wednesday 16 January 2013 (No questions related to Reversible Reactions.)
120
Group Information
Group Leader: Abdullah Al Abid Mohammad Tofazzal Hossain Bhuyian
Also In the Group
Abdul Haleem Abdul Kareem Ikramullah Arifulla Haider Ali Baqwi Mohammad Zain Shakeel Mohammad Anas Kareem Ahmed Bin Rashid Irshad Mohammad Rehan Sandhu
121
CHEMISTRY PAST PAPER QEUSTIONS AND REFERENCES FOR TERM 3 Topics from term 3 Reactivity series Test for ions and gases
Extraction for metals
Project Done By Hudais khan, Hamid Hasan, Hamza Shams, Ahmed Ifthikar, Israr Ahmed, Saleem Khan, Shabbir Hossain and Abdul Khaleel Talha
REACTIVITY SERIES Paper
Month
Year
Question
Sub Part
1
May
2000
5
1
May
2001
9
(b)
1
May
2004
17
(a)(b)
1
May
2005
5
1
May
2007
5
1
May
2010
6
1
May
2012
2
1
January
2013
6
2
May
2008
7
2
June
2011
1
(a)(i)(ii)(iii)
(b)
rusting of iron Paper
Month
Year
Question
Sub Part
1
May
2004
17
( c)
1
May
2006
16
1
January
2007
3
1
January
2009
9
1
May
2009
7
1
May
2011
7
1
January
2012
2
1
January
2013
4
2
January
2011
6
(b)
Oxidation & reduction Paper
Month
Year
Question
1
January
2006
9
1
January
2008
8
1
May
2008
5
1
January
2011
8
Sub Part
(a)(b)(i)(ii)
Extraction of metals Paper
Month
Year
Question
Sub Part
1
January
2000
7
(a)
1
May
2001
6
(a)(b)( c )
1
January
2001
9
(a)
1
May
2002
7
1
May
2002
14
1
January
2005
7
1
January
2007
12
1
January
2008
8
1
May
2008
12
1
May
2011
9
1
May
2012
12
(a)(b)
1
January
2013
7
(a)
2
May
2005
7
(a)
2
January
2006
6
(a)
2
May
2006
6
(a)
2
May
2007
9
(a)
2
May
2008
6
(a)
2
May
2009
6
(a)(i)(iii)
2
January
2010
8
(a)
2
May
2010
7
(a)(iii)
2
January
2011
6
(a)
2
May
2012
2
(d)
test for ions & Preparation and test for gases
Paper
Month
Year
Question
Sub Part
1
May
2000
8
(e)
1
January
2001
3
1
May
2001
2
1
May
2001
6
1
May
2003
8
1
May
2003
10
1
May
2005
13
1
May
2006
7
1
January
2008
12
1
January
2012
3
1
May
2012
11
2
May
2007
1
2
January
2009
1
2
May
2010
9
(d)(ii)
(a)(b)
(a)(b)
Related Documents 3h463d
Edexcel Igcse Chemistry Past Paper Questions 2013 5n113x
November 2019 62
Physics Igcse Past Paper Questions 6d2j1e
December 2021 0
Edexcel Igcse Chemistry Answers 263p4h
November 2019 89
Edexcel Igcse May 2012 Chemistry Paper- 2 5q3r1b
December 2019 83
Edexcel Igcse Chemistry Revision Guide y6u13
October 2019 96
Edexcel Chemistry Igcse Student Book 92e1
October 2019 240More Documents from "Sadiq Amin" 5s1i
Edexcel Igcse Chemistry Past Paper Questions 2013 5n113x
November 2019 62
Uop375wmky5801 22601s
November 2019 111
Fuel_oil_piping_installation_instructions_h14694m_8-10-11.pdf 4v3h3j
December 2019 76
F 5ei5n
September 2021 0
Pooleh-khoon_www-azadieiran2-wordpress-com.pdf 133w6p
February 2022 0