GEWATA GENERAL SECONDARY SCHOOL

2017 E.C / 2025 G.C CHEMISTRY FINAL EXAMINATION FOR

GRADE 12TH
TIME ALLOWED: 2:30
GENERAL DIRECTIONS
THIS QUESTION PAPER CONTAINS 80 MULTIPLE CHOICE QUESTIONS,
DEAR STUDENTS ATTEMPT ALL THE ITEMS.
THERE IS ONLY ONE BEST ANSWER FOR EACH ITEM, CAREFULLY SELECT
THE BEST ANSWER FROM THE SUGGESTED OPTIONS AND WRITE ONLY
THE LETTER OF YOUR CHOICE ON THE SEPARATE ANSWER SHEET
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YOU ARE ALLOWED TO WORK ON THE EXAMINATION FOR 2:30 HOURS. IF
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HALL RESULT IN AN AUTOMATIC DISMISSAL FROM THE EXAMINATION
HALL AND CANCELLATION OF YOUR SCORE.
PLEASE MAKE SURE THAT YOU HAVE WRITTEN ALL THE REQUIRED
INFORMATION ON THE SEPARATE ANSWER SHEET PROVIDED.
DO NOT TURN THIS PAGE OVER UNTILL YOU ARE TOLD TO DO SO!

You may refer to the information given below when you work on some of the
questions. (If Necessary)

PHYSICAL CONSTANTS
Speed of light, C = 3𝗑108m/s
Planck‟s constant, h = 6.626 𝗑10-34 J/s
Faradays constant, F = 96500 C/mol
Mass of an electron = 9.11 𝗑10-31Kg
Rydberg‟s constant, RH = 2.18 𝗑10-18 J

element F Na Si P S Cl Ca Cr Ni Cu Ga Br Ag I Xe
A 19 11 28 31 32 35.5 40 52 58.7 63.5 69.7 79.9 108 127 131
Z 9 23 14 15 16 17 20 24 27 29 31 35 47 53 54
ATOMIC NUMBERS (Z) AND MASS NUMBERS (A)

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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 1
1. Which of the following statement describe Chemical industries? It is :
A. A process in which dissolved solute comes out of solution and form crystals.
B. An area of chemistry concerned with the rate at which chemical reaction occur.
C. A firm that involves the usage of raw material to form desired products by means of
chemical reaction.
D. An expression for the chemical composition of compound.
2. What is the [OH-] of a solution with a pH of 4?
A. 10-4 M B. 104 M C. 1010 M D. 10-10 M
3. As opposed to a galvanic cell, in an electrolytic cell:
A. spontaneous redox reaction generates electricity C. the anode is positive
B. electrons flow from cathode to anode D. oxidation takes place at the cathode
4. The electrolyte in lead storage battery is; A. HCl B. H2SO4 C. NaOH D. HNO3
5. For the reaction below, which pair of species are both bases?
HCN + H2O H3O+ + CN-
-
A. HCN & CN B. H3O+ & H2O C. HCN & H3O+ D.H2O & CN-
6. What is the chemical symbol for Antimony?
A. At B. Sb C. As D. Sn
7. pKa values of three acids X, Y and Z are 4.5, 3.5 and 6.5, respectively. Point out the
CORRECT order of acid strength?
A. X > Y > Z B. Z > X > Y C. Y > X > Z D. Z > Y > X
8. Two wires are connected to battery and a light bulb in series. When the free ends of the wires
are dipped into a beaker of water, the bulb remains unlit. A substance was dissolved in the
water but the bulb remains unlit. Which substance was added?
A. HNO3 B. KCl C. C2H5OH D. NaOH
9. Which species is NOT amphiprotic species?
A. H2PO4- B. H2SO4 C. H2O D. NH3
10. Which of the following reactions occur spontaneously as written, with the production of a
measurable electric current?
A. I2 + NaBr Br2 + 2NaI C. Li+ + Na+ NaLi E. Ag + Li Ag++ Li+
+
B. Li + NaCl LiCl + Na D. 2Li +F2 2LiF
11. A buffer solution a mixture of:
A. a weak acid and a strong acid C. a weak acid and its conjugate base
B. a strong acid and its conjugate base D. a strong acid and its conjugate acid
12. An atom of an element has the following ground-state configuration:
[Kr]4d105s25pb . If the element is in Group VIIA, What is the symbol of element? What is b?
A. I, 5 B. Se, 4 C. Xe, 5 D. Zn, 3
13. Why salts of weak acid and strong base give a basic solution? because the
A. The cations derived from a strong base can hydrolyzed
B. The anions derived from a strong base can hydrolyzed
C. The cations derived from a weak acid can hydrolyzed
D. The anions derived from a weak acid can hydrolyzed
14. . Electroplating is used to coat one metal with usually less reactive metal. If you want to plate
out iron spoon with silver metal, then which of the following is TRUE?
A. The electrolyte must be contained silver ion
B. The iron spoon must be set at the anode
C. The silver metal must be the cathode
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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 2
 D. The material to be plated must be the anode
15. Which of the following statements is TRUE?
A. A universal indicator is a mixture of indicators that will give a d/t color for a d/t pH.
B. Phenolphthalein is a universal indicator
C. A universal indicator can only be used in either strongly acidic or basic solution.
D. The color of a universal indicator is red in a weak acid.
16. What half-reaction would be expected to occur at the cathode in the electrolysis of aqueous
conc. Sodium fluoride?
A. 2F−(aq) → F2(g) + 2e − C. 2H2O(l) +2e − → H2(g) + 2OH−(aq)
B. 2H2O(l) → O2(g) + 4H+(aq)+ 4e− D. Na+(aq) + e−→ Na(s)
17. Which of the following titrations will have an equivalence point at a pH < 7?
A. Strong acid with weak base C. Weak acid with weak base
B. Strong acid with strong base D. Weak acid with strong base
18. In titration of acids and bases, the point at which stoichiometrically equal amounts of
substances have been brought together is
A. End point B. Standard point C. Equivalence point D. common ion
19. The species that being reduced and causes oxidation is a/an
A. Reduction B. Reducing agent C. Oxidation D. Oxidizing agent
20. A criterion for the strength of an acid is: - A. its density C. its corrosive action
B. its degree of ionization D. its concentration
21. Which substances is reduced in the following reaction?
O
+
A. H B. C. D.
22. The pH of NaC2H3O2 to C2H4O2 buffer is 5.74. Then what is ratio of [CH3COOH] to
[CH3COO–]? A. 0.001 B. 0.01 C. 0.1 D. 0.2
23. Which of the following pairs of solution CANNOT be used to prepare a buffer?
A. HCOOH and HCOONa C. NaOH and HCl
B. H2CO3 andNaHCO3 D. NaH2PO4 andNaHPO4
24. It takes 20mL of 0.5N NaOH to neutralize a 5mL solution of H2SO4. What is the normality
of the H2SO4 solution? A. 4 B. 3 C. 2 D. 1
25. In electrolytic cell, anions move towards_______, cations move towards _____ and electron
flow from _________ to __________
A. Cathode, Anode, Cathode, Anode C. Anode, Cathode, Cathode, Anode
B. Anode, Cathode, Anode, Cathode D. Anode, Anode, Cathode, Cathode
26. Four 0.1M aqueous solution of KOH, KBr, K2CO3, and KHCO3 are given. Which of the
following arrangement has these solutions in order of increasing pH?
A. KOH > KBr > K2CO3 > KHCO3 C. K2CO3< KBr < KHCO3 < KOH
B. KHCO3 < KBr < K2CO3 < KOH D. KHCO3 > K2CO3 >KBr > KOH
27. Which of the following CANNOT reduced by Fe? (E°Fe2+/Fe =-0.44V)
A. Sn4+/Sn2+, E°Sn4+/Sn2+ = + 0.15V C. Ni2+/Ni , E°Ni2+/Ni = –0.26V
B. Mg2+/Mg ,E°Mg2+/Mg = – 2.37V D. Ag+/Ag , E° Ag+/Ag = +0.80V
28. A laboratory technician a prepared 58g of 0.005L Mg(OH)2 solution. What is the pH of this
solution? (M.Wt : Mg =24, O=16 , H=1) A. 2 B. 11 C. 12 D. 3
29. What is the difference between metallic conduction and electrolytic conduction?

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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 3
 A. Metallic conduction involves transfer of matter in the form of ions, whereas electrolytic
conduction does not involves transfer of matter.
B. In metallic conduction passage of charge brings about physical and chemical changes,
whereas electrolytic conduction brings about only physical changes.
C. In metallic conduction electrical charge is carried by electrons, whereas in electrolytic
conduction electrical charge is carried by ions.
D. In metallic conduction the ions are able to move in the solution, whereas in electrolytic
conduction delocalized valence electrons are able to move in the solution
30. What are the expected products of the electrolysis of an aqueous solution of Cu using an
inert electrode?
A. Cu and H2 at the cathode and dissolving of Cu at the anode
B. Cu at the cathode and O2 at the anode only
C. Cu and H2 at the cathode and only O2 at the anode
D. Cu at the cathode, O2 at the anode and solution
31. During the electrolysis of an aqueous solution of AgNO3, What would happen to the mass of
Ag metal deposited, if the current is quadrupled and the electrolysis time is decreased to ½ of
its original state?
A. Doubled B. Halved C. Quadrupled D. Tripled
32. A cup of coffee has a hydroxide ion concentration of 1.0 × 10–10 M. What is the pH of this coffee?
A. 6 B. 7 C. 4 D. 2
33. Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl2 (g). The reaction that
occurs at the anode is 2Cl −(aq) Cl2 (g) +2e − A constant electric current deposits 152 g Cl2 in 56.1
min from an aqueous solution of sodium chloride. What is the current?
A. 123A B. 61.5A C. 4.36 x103 D. 6.18 x105A
34. How much time is required to electroplate 4.4mg of Silver from a AgNO3 solution, using a
current of 0.50A?
A. 7.9 sec B. 790 sec C. 1.966 sec D. 1966 sec
35. A 1M solution of Cu (NO3)2 is placed in a beaker with a strip of Cu metal. A 1M of SnSO4 is
placed in a second beaker with a strip of Sn metal. The two beakers are then connected by a
salt bridge and the two metal electrodes are connected by wires to a voltammeter. Which of
the following electrode serves as the anode and which electrode gains mass?
Given that: E0 Cu = + 0.34V and E0 /Sn 0.14V
A. Sn, Sn electrode gains mass C. Sn, Cu electrode gains mass
B. Cu, Sn electrode gains mass D. Cu, Cu electrode gains mass
36. Which of the following beakers best represents a container of a weak acid, HA, in water?
(Water molecules have been omitted for clarity.)

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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 4
 A. Only beaker“A”
B. Beaker “A” and beaker “C”
C. Only beaker “C”
D. Only beaker “B”

37. Which of the following is WRONG concerning a Galvanic cell?

A. It involves the deposition of one metal at one electrode when oxidations of another
metal occur at the second electrode.
B. A spontaneous chemical reaction generates an electric current
C. A non-spontaneous chemical reaction generates electrical energy
D. It does not require an external source of electric current to function
38. Consider Ka= 1.8x10–5 for CH3COOH, Ka= 6.8x10–4 for HF then which one is correct?
A. Ka for CH3COOH is greater than HF B. pKa for CH3COOH is less than for HF
C. CH3COOH is weaker acid than HF D. CH3COOH is stronger acid than HF
39. A battery is „„dead‟‟ if:
A. Reactants and products reach their equilibrium concentrations.
B. Ecell is equal to zero.
C. ΔG is equal to zero.
D. All of the above.
40. Which of the following statements is TRUE?
A. The larger pKa value of an acid, the stronger an acid
B. Smaller pH or higher pOH; weaker the acid & larger pH or smaller pOH; weaker the base.
C. As [OH-] grows; pH of solution raised or pOH decreased.
D. The aqueous solution of a strong acid contains both H3O+ and OH–.
41. Adding Sodium hydroxide (KOH) to a solution of Acetic acid (CH3COOH)
A. Increase [OH–] C. Increase [H3O+]
–
B. Increase [CH3COO ] D. Decrease [CH3COO–]
42. Point out the basic solution
A. [H+] = 1.0x10–7M C. [H+] = 1.0x10–9M
– –12
B. [OH ] = 2.2x10 M D. [OH–] = 3x10–8M
43. For the electrochemical cell represented by: Zn(s)/ZnSO4(aq) // CuSO4(aq)/Cu(s). The standard
reduction potentials for Cu2+/Cu and Zn2+/Zn are + 0.34 and -0.76V, respectively. What will
be the cell reaction that occurs spontaneously and its cell voltage?
E°(V)
A. Cu + Zn2 + Cu2 + + Zn 1.10
B. Zn + Cu2+ Zn2+ + Cu 0.42
2+ 2+
C. Cu + Zn Zn + Cu 0.42
D. Cu2+ Zn Cu + Zn2+ 1.10
44. Given the acid ionization constant:
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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 5
 Acids Ionization Constants (Ka)
HOCN 3.5x10–4
HNO2 4.5x10–4
HCN 4.9x10–10
CH3COOH 1.8x10–5
When the conjugate bases of the above acids are arranged in descending order of base
strength, the CORECT order is:
A. OCN– < NO2– < CN– < CH3COO–
B. NO2– > CN– > CH3COO– > OCN–
C. CN– < CH3COO– < OCN– < NO2–
D. NO2– > OCN– > CH3COO– > CN–
45. Which of the following is a non-renewable resource:
A. soil B. petroleum C. water D. plants
46. The pH of 0.002M Ca(OH)2 solution is A. 14 B. 12 C. 11 D. 10
47. The value of E˚ for the following reaction is 1.10 V. What is the value of Ecell when the
concentration of Cu2+ is 1.0 M and the concentration of Zn2+ is 0.025M
Zn (s) + Cu2+(aq) →Cu(s) + Zn2+(aq) , E˚ =1.10 V, [Cu2+]=1.0M and Zn2+M =0.025M
A. 1.40V B. 0.80V C. 1.15V D. 0.95V
48. In the following reaction of trichloroacetic acid, HC2Cl3O2, with formate ion, CHO2– the
formation of trichloroacetate ion, HC2Cl3O2– and formic acid, HCHO2 is favored.
HC2Cl3O2 + CHO2– → HC2Cl3O2– + HCHO2 Then, which one is CORRECT?
A. HC2Cl3O2 is strong acid C. CHO2– is weak base than HC2Cl3O2–
B. HCHO2 is strong acid D. HCHO2 is weak acid
49. What is the standard cell potential of the following voltaic cell at 250C using standard
electrode potentials? Au(s) | Au3+(aq)||Fe2+(aq) | Fe(s)
3+
Au (aq) + 3e- → Au(s); Eo red (Au3+/Al) = + 1.50 V
2+
Fe (aq) + 2e- → Fe(s); Eo red (Fe2+/Fe) = – 0.44 V
A. 1.94V B. 1.06V C. -1.06V D. -1.94V
50. Which of the following salts would produce the most basic aqueous solution?
A. NH4Cl B. KBr C. NaF D. LiNO3
51. A shampoo solution at 25ºC has a hydroxide-ion concentration of 1.5x10– 9 M. Then the solution:
A. Is acidic B. Is basic C. Is neutral D. Has both pH and POH is greater than 7
52. What are the oxidation numbers for Nickel, Sulfur, and Oxygen in Ni2(SO4)3
A. Ni =+3; S =+6; O = –2 C. Ni = +2; S = +2; O = –2
B. Ni =+2; S =+4; O = –2 D. Ni = +3; S = +4; O = –2
53. If you mix 0.10mol of NH3 and 0.10mol of HCl in a bucket of water, you would expect the
resulting solution to be:
A. Very basic B. Slightly basic C. Neutral D. Slightly acidic E. Very acidic
2+
54. How many Faraday would be required to reduce one mole of Cu ions to free metal?
A. 3 B. 2 C. 1 D. 4
55. Point out that DOESNOT have an influence on the preferential discharge of ions during
electrolysis?
A. The tendency of each ions to gain or loss e- C. The conc. of each kind of ion
B. The partition b/n the cathode and anode compartment D. The type of electrode

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Chemistry Model Examination Grade -12 2024/2025G.C (2017E.C) 6
 End

ANSWER SHEET
Name: Roll No : Grade/ Section: 12th

Choice Items

1 11 21 31 41 51 61 71

2 12 22 32 42 52 62 72

3 13 23 33 43 53 63 73

4 14 24 34 44 54 64 74

5 15 25 35 45 55 65 75

6 16 26 36 46 56 66 76

7 17 27 37 47 57 67 77

8 18 28 38 48 58 68 78

9 19 29 39 49 59 69 79

10 20 30 40 50 60 70 80

80

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