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SULIT4541/1Chemistry2 jam 30 minit

CHEMISTRY DEPARTMENT

PRA-PEPERIKSAAN AKHIR TAHUNTINGKATAN 4 TAHUN 2011

CHEMISTRY

Dua jam tiga puluh minit

1 A B C D 16 A B C D Soalan Markah penuh Markah

2 A B C D 17 A B C D A 1-30 30

3 A B C D 18 A B C D B1 8

4 A B C D 19 A B C D 2 10

5 A B C D 20 A B C D 3 15

C4 20

6 A B C D 21 A B C D 5 17

7 A B C D 22 A B C D Jumlah: [100]

8 A B C D 23 A B C D

9 A B C D 24 A B C D

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11 A B C D 26 A B C D

12 A B C D 27 A B C D

13 A B C D 28 A B C D

14 A B C D 29 A B C D

15 A B C D 30 A B C D

1 The following word equation shows a chemical reaction.

X + magnesium oxide magnesium chloride + water

What is acid X?A Hydrochloric acid C Phosphoric acidB Sulphuric acid D Nitric acid

2 Hydrogen chloride in methylbenzene does not show any acidic property. Which of the followings explain the observation?

A Hydrogen choride is a covalent compoundB Hydrogen choride molecules ionises in the solution.C This solution does not contain hydrogen ions.D This solution show the electrical conductivity

3 Which of the following reactions does not show the role of benzoic acids as an acid?A The burning of benzoic acid to produce carbon dioxide and waterB The reaction that occurs between benzoic acid and sodium hydroxide to produce salt and waterC The reaction that occurs between benzoic acid and limestone to produce carbon dioxideD The reaction that occurs between benzoic acid and magnesium ribbon to produce hydrogen

4 Which of the following statements are true for both dilute ethanoic acid and dilute hydrochloric acid of the same concentration?

I They have different concentration of hydrogen ions.II Their degree of ionisation in water is the same.III They have different pH value.IV They neutralise equal amount of sodium hydroxide.

A I and II only C II and IV onlyB I and III only D III and IV only

5 Which of the following is a synthetic polymer?

A Rubber C ProteinB PVC D Starch

6 What is the type of glass used to make laboratory glass wares?

A Lead glass C Borosilicate glassB Fused glass D Soda glass

7 Which of the following substances used by a farmer to neutralize an acidic soil?

A Calcium oxide C Sodium hydroxideB Sulphuric acid D Ammonium hydroxide

8 Which of the following are insoluble salts?

I Silver chlorideII Magnesium nitrateIII Barium sulphateIV Zinc carbonate

A I and III only C I, II and III onlyB II and IV only D I, III and IV only

9 If 150 cm3 of a 4 mol dm–3 solution Y is added to 250 cm3 of water, what is the molarity of the diluted solution?A 1.50 mol dm–3 C 2.80 mol dm–3

B 2.40 mol dm–3 D 3.00 mol dm–3

10 Which of the following shows a precipitation reaction?

A K2CO3 + Pb(NO3)2 2KNO3 + PbCO3

B 2HCl + PbO PbCl2 + H2OC Na2SO4 + Mg(NO3)2 MgSO4 + 2NaNO3

D NaOH + K2CO3 Na2CO3 + 2KOH

11 The pie chart in Diagram 11 shows the composition of stainless steel.

Diagram 11What is element X?

A Tin C IronB Copper D Aluminium

12 Which of the following statement describes the property of hydrochloric acid?

A It reacts with any metal to give hydrogenB It liberates ammonia from ammonium saltsC It causes colour of litmus paper to change from red to blueD It reacts with any bases to produce a salt.

13 Table 1 shows some of the steps for preparing a standard solution but they are not in order.

Table 3Which of the following sequence of steps is correct?A P Q R S C R P Q SB R P S Q D R Q P S

14 Diagram 10 shows the industrial preparation of sulphuric acid through the Process I.

I II III IV S SO2 SO3 H2S2O7 H2SO4 oxygen oxygen concentrated H2SO4 water

Diagram 10

Which stage involves the use of a catalyst?A IB IIC IIID IV

15 Diagram 6 shows the pH values of four different solutions.

Diagram 13

Which of the solutions has the highest concentration of hydrogen ions?

A VB W C X D Y

P - Dissolve the solute in distilled water

S - Transfer the solution into a volumetric flask

Q - Add distilled water until the mark of the flask

R - Weigh the mass of the solute needed

WV YX

pH = 12pH = 8pH = 4pH = 1

16 Which pairs of substances are suitable to prepare copper(II) sulphate in the laboratory?

I Copper and dilute suphuric acidII Copper(II) carbonate and dilute sulphuric acidIII Aqueous copper(II) nitrate solution and dilute sulphuric acidIV Copper(II) hydroxide and sulphuric acid

A I and II only C II and IV onlyB I and III only D I, II and III only

17 Lead (II) Iodide can be prepared through

A Precipitation ReactionB Neutralization ReactionC CrystallizationD Recrystallization

18 Diagram 15 shows the set–up of apparatus for the titration of potassium hydroxide solution with sulphuric acid.

Diagram 15

What is the volume of sulphuric acid at the end point of the titration?

A 12.5 cm3 C 50 cm3

B 25 cm3 D 100 cm3

19 Sulphuric acid is a diprotic acid because

A sulphuric acid has the properties of acid and also a dehydrating agent.B one mole of sulphuric acid can neutralise two moles of bases.C one molecule of sulphuric acid contains two moles OH- ions.D one molecule of sulphuric acid produces two H+ ions in water.

25 cm3 of potassium hydroxide solution 1.0 mol dm-3 and phenolphthalein as an indicator

Sulphuric acid 1.0 mol dm-3

20 Process II can be represented by the following equation:

N2 (g) + 3H2 (g) → 2NH3 (g)What is the catalyst, temperature and pressure used in this process?

Catalyst Temperature(˚C) Pressure (atm)A Iron 450 200B Platinum 900 150C Platinum 800 10D Iron 200 1050

21 Table 2 shows the pairs of polymer and monomer.

Polymer MonomerI Carbohydrate GlucoseII Polyvinyl chloride ChloroetheneIII Protein Amino acidIV Natural rubber Neoprene

Table 2Which of the following pairs of polymer and monomer are correct ?

A I and II only C II, III and IV onlyB I, II and III only D I, II, III and IV

22 Neutralization reaction between nitric acid and calcium hydroxide is shown in the chemical equation below.

2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O

What is the minimum volume of nitric acid of 0.2 mol dm-3 needed to completely neutralise 50 cm3 calcium hydroxide solution 0.05 mol dm-3.

A 12.5 cm3

B 25.0 cm3

C 37.5 cm3

D 50.0 cm3

23 When sodium hydroxide is added dropwise until in excess to a solution, a white precipitate which is soluble in excess is formed. The ions that could be present in the solution are

I Al3+

II Zn2+

III Mg2+

IV Pb2+

A I and II onlyB III and IV onlyC I, II, and IV onlyD I, II, III and IV

24 A green solid is heated up strongly and the residue is black in colour. The solid is

A Sodium carbonateB Lead(II) nitrateC Iron(II) carbonateD Copper(II) carbonate

25 The table below shows the results of qualitative analysis of a salt.

Qualitative analysis Observation

Sodium hydroxide solution added until excess into salt solution

White precipitate formed and dissolve in excess.

2 cm3 of dilute nitric acid is added and followed by 2 cm3 silver nitrate solution. White precipitate is formed.

Among the following ions, which may be present in the salt?

A Zn2+ and Cl-

B Mg2+ and Cl-

C Zn2+ and SO42-

D Mg2+ and SO42-

26 The table below shows the observation of the reaction between calcium carbonate and ethanoic acid in two different solvents.

Beaker Reaction Observation

X calcium carbonate + ethanoic acid in distilled water.

Effervescence occurs

Y calcium carbonate + ethanoic acid in benzene

No visible change

Which of the following statements are true about the observation in beaker X and beaker Y?

I Water ionizes ethanoic acid in beaker XII Benzene ionizes ethanoic acid in beakerIII Water reacts with calcium carbonate in beaker X.IV Ethanoic acid remains as molecule in beaker Y.

A I and II onlyB I and IV onlyC II and III onlyD III and IV only

Alloy T

27 The body of the car shown in the diagram below is made of alloy T.

What is alloy T?

A SteelB BrassC BronzeD Duralumin

28 Ammonium nitrate fertilizer is obtained through the reaction between ammonia solutions with

A sodium nitrate solution B nitrogen dioxide gas C dilute sulphuric acid D dilute nitric acid

29 Ammonium sulphate, (NH4)2SO4 is an example of a fertilizer. Calculate the percentage of nitrogen in 1 mole of ammonium sulphate.[Relative atomic mass: N=14, H=1, S=,32, O=16]

A 12.12 %B 21.21 %C 23.23 %D 31.31 %

30 Which salt solution is colourless?

A Iron(III) sulphate C Copper(II) chlorideB Aluminium nitrate D Potassium dichromate(VI)

Dilute hydrochloric acid0.1 moldm-3

Blue litmus paperBlue litmus paper Blue litmus paper

Dry glacial ethanoic acidAqueous solution of ethanoic acid 0.1 moldm-3

1. Diagram 4 shows three test tubes contain dry glacial ethanoic acid, aqueous solution of ethanoic acid and dilute hydrochloric acid.

P Q R Diagram 4

(a) (i) State the colour change of the litmus paper in test tubes R.

...................................................................................................................................... [1 mark]

(ii) Write the formula of ion which caused the colour change of the litmus paper.

.......................................................................................................................................[1 mark]

(b) Is there any changes of colour of the litmus paper in test tube P? Explain why.

.....................................................................................................................................

.....................................................................................................................................[2 marks]

(c) Table 4 shows the pH value of aqueous solution of ethanoic acid and dilute hydrochloric acid of the same molarity.

Type of acid aqueous solution of ethanoic acid

dilute hydrochloric acid

Molarity 0.1 moldm-3 0.1 moldm-3

pH value 2.9 1.0 Table 4

Explain the difference in the pH value of aqueous solution of ethanoic acid and dilute hydrochloric acid.

....................................................................................................................................

....................................................................................................................................

....................................................................................................................................[3 marks]

Calcium carbonate powder is added into test tube R.(i) State one observation in test tube R.

..................................................................................................................................[1 mark]

2(a) Diagram 2 shows an industrial preparation of Ammonium sulphate from the product(s) of Process I and Process II.

Diagram 2(i) State the names of compound X.

………………………………………………………………………………….………[1 mark]

(ii) State the name of Process I and Process II.

Process I: ………………..………… Process II: ………….…………………..…...[1 mark]

(iii) State the reaction Y:

…………………………………………………………………………………….….. [1 mark]

(iii) Write the balanced chemical equation for reaction Y to produce ammonium sulphate.

…………………………………………………………………………………………..[2 marks]

(b) Qualitative analysis can be used to determine the presence of cations and anions in solutions.

(i) Describe chemical tests that can be used to verify the sulphate ion, SO42-

.

………………………………………………………………………………………...

…………………………………………………………………………………………

………………………………………………………………………………………… [3 marks]

(ii) In table 3, state the observation made when confirmatory test is carried out for ammonium ion, NH4

+.Confirmatory Test Observation

Added small amount of sodium hydroxide solutions to ammonium ion, NH4

+ solution.

Followed by heat the mixture of sodium hydroxide solutions and ammonium ion, NH4

+ solution.[2 marks]

Process I

Process II

Sulphuric acid

Compound X

Ammonium sulphate

Reaction Y

3. An experiment is carried out to determine the concentration of nitric acid. 25 cm3 0.10 mol dm-3 potassium hydroxide solution is titrated with nitric acid from a burette. Phenolphthalein is used as an indicator. Figure 1 shows the initial and final readings of the three titrations carried out.

(a) Record the readings for each titration in the spaces provided in Figure 1.[3 marks]

(b) A change in the colour of phenolphthalein indicator is observed at the end point.(i) State the colour change.

…………………………………………………………………………………………….

[3 marks](ii) State the operational definition for end point in this titration.

…………………………………………………………………………………………….[3 marks]

(c) Construct a table to show all the data in each of these titrations.

[3 marks]

(d) Calculate the concentration of nitric acid that is used in this experiment.

[3 marks]

+ Dilute sulphuric acidHeated

Substance Q

Solid U + Gas RSolid U is black

Solution V + Gas R

Solution ZSolution W + Solid X

+ Dilute nitric acid + Metal M

4 The flow chart in the diagram shows a series of chemical changes of solid Q .

(a) Draw a labelled diagram of the set-up of apparatus for the chemical reaction of converting substance Q to solid U and gas R. In your diagram show how gas R is tested.

[4 marks]

(b) Solution Z and V are the products from reaction in flow chart.(i)Name the possible metal cation in solution Z(ii)Describe the confirmatory test for a cation mention in b(i)

[3 marks]

(c) Describe how to obtain crystal salt V from their solution V[4 marks]

(d) Metal M is more electropositive than the metal in solution V. When metal M is added into solution V , chemical reaction occured. Name the metal M and give an observations for the reaction that produces solution W and solid X.

[2 marks]

(e) The chemicals supplied are Zinc oxide Sodium carbonate solution Dilute nitric acid

Describe briefly how you can prepare a sample of dry zinc carbonate in the laboratory. Include in your answer all chemical equations involved.

[7 marks]

5. Diagram 3 shows two beakers containing colourless solution labelled A and B.

Diagram 3

You are told that the two colourless solutions are calcium nitrate and magnesium nitrate. You are

required to label correctly the name of each solution in the containers.

Design an experiment to identify which is calcium nitrate and which is magnesium nitrate

solution by using aqueous of ammonia solution as a reagent.

Your answer should include the following:

(a) Problem statement

(b) Hypothesis

(c) All variables

(d) List of materials and apparatus

(e) Procedure

(f) Tabulation of data

[17 marks]

END OF QUESTION PAPER

Beaker A Beaker B