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WAEC May/June Free Chemistry Questions and Answers EXPO Room (11th June, 2026).
WAEC May/June 2026 FREE CHEMISTRY QUESTION AND ANSWER ROOM [School Candidates]
Thursday, 11th June 2026
Chemistry 2 (Essay) – 9:30am – 11:30am
Chemistry 1 (Objective) – 11:30am – 12:30pm
Thursday, 11th June 2026
Chemistry 2 (Essay) – 9:30am – 11:30am
Chemistry 1 (Objective) – 11:30am – 12:30pm
2026 WAEC CHEMISTRY (CHEM) OBJECTIVES (OBJ) ANSWERS:
1. When the pressure on 200 cm³ of a gas is doubled and its absolute temperature is halved, its volume would become — B. 50 cm³
2. In the periodic table, an element with electronic configuration of 1s² 2s² 2p⁶ is in — D. Period 2 and Group V
3. An element X has a valency of +3. The correct formula of its chloride is — C. XCl₃
4. A zwitterion is — A. bipolar
5. Transition elements possess variable oxidation states because they have — C. electrons in the d-orbitals
6. Oxygen and ozone are — A. allotropes
7. A solution was found to have a soapy touch. The pH of the solution is likely to be — B. 12
8. Which of the following substances is not a mixture? — D. Iron rod
9. Which of the following carbohydrates contains fructose? — A. Sucrose
10. The following orbitals present in a potassium atom contain electrons except — D. 3d
11. Carbon(IV) oxide could be produced from glucose by — B. fermentation
12. NH₄Cl is more soluble than NaCl. When a mixture of NH₄Cl and NaCl are separated by fractional crystallization — B. NH₄Cl would crystallize first
13. Metallic solids are good conductors of electricity because — C. of the presence of mobile electrons
14. How many sub-atomic particles are contained in ³⁷₁₇X⁴⁺ ? — A. 37
15. Liquid X has a sour taste. The pH value of X is likely to be — C. 5
16. Which of the following periodic properties increases from right to left in the periodic table? — A. Atomic radius
17. The flame test of a certain metal produced a yellow colouration. The metal is most likely to be — D. Na
18. Equal volumes of CH₄(g) and NH₃(g) at the same temperature and pressure would have the same — A. number of molecules
19. The effect of greenhouse gases could be reduced by — A. planting of trees
20. The value of y is — A. 8
21. A balloon was filled with a mixture containing equal volumes of H₂, He and N₂. The correct statement is — B. The pressure in the balloon would be a sum of the partial pressures of H₂, He and N₂
22. If carbon forms CN₄ and CY₄ with elements X and Y respectively, the formula of the compound formed between X and Y is — A. X₂Y
23. Which substance could be used in galvanization of iron to prevent rusting? — D. Zinc
24. The molar mass of a chloride of iron is 127 g mol⁻¹. The formula of the chloride is — A. FeCl₂
25. Which apparatus is used in transferring a solution into a burette during titration? — A. Funnel
26. When X was added to aqueous FeCl₃, its colour changed from reddish-brown to pale-green. X could be — A. LiAlH₄
27. Which of the following substances is a mixture? — C. Brine
28. An atom of chlorine could be converted to chloride ion by — D. reduction
29. The empirical formula of a compound is given as CₓHᵧO. Its relative molecular mass would be — D. 44
30. A molecule is the smallest independent particle of — B. an element
31. Which of the following acids is most volatile when concentrated? — A. HCl
32. The value of X in the redox half reaction is — A. 2
33. The simplest ratio of carbon atom to hydrogen atom in benzene represents — B. empirical formula
34. Potassium chloride may be used on farmlands because it — B. is essential for healthy plant growth
35. The mass of sodium hydroxide required to prepare 250 cm³ of 2.0 mol dm⁻³ NaOH(aq) is — D. 20 g
36. Ethanol could be produced from — C. sugar cane
37. X²⁺ is formed from X atom by — D. losing two electrons
38. It can be deduced that — D. the oxidation number of X increases
39. A particle made up of 10 electrons and 13 protons is — A. a cation
40. Magnesium oxide is an example of — D. a basic oxide
41. Degenerate orbitals are orbitals of — A. the same subshell having equal energy
42. The general formula of an alkyl group is — A. CₙH₂ₙ₊₁
43. Which of the following compounds is covalent? — D. HCl
44. The preparation of carbon(II) oxide is done in a fume cupboard because the gas is — C. poisonous
45. Which of the following elements would evolve hydrogen most rapidly from dilute HCl? — A. Zn
46. Which pair of enthalpy changes is always negative? — D. Combustion and neutralization
47. The reaction represented by the equation MgCl₂ + 2H₂O → Mg(OH)₂ + 2HCl is — D. hydrolysis
48. Y is a weak acid that turns blue and green when added to aqueous solutions of NaHSO₃ and Na₂CO₃ respectively. Y could be — C. an acid-base indicator
2. In the periodic table, an element with electronic configuration of 1s² 2s² 2p⁶ is in — D. Period 2 and Group V
3. An element X has a valency of +3. The correct formula of its chloride is — C. XCl₃
4. A zwitterion is — A. bipolar
5. Transition elements possess variable oxidation states because they have — C. electrons in the d-orbitals
6. Oxygen and ozone are — A. allotropes
7. A solution was found to have a soapy touch. The pH of the solution is likely to be — B. 12
8. Which of the following substances is not a mixture? — D. Iron rod
9. Which of the following carbohydrates contains fructose? — A. Sucrose
10. The following orbitals present in a potassium atom contain electrons except — D. 3d
11. Carbon(IV) oxide could be produced from glucose by — B. fermentation
12. NH₄Cl is more soluble than NaCl. When a mixture of NH₄Cl and NaCl are separated by fractional crystallization — B. NH₄Cl would crystallize first
13. Metallic solids are good conductors of electricity because — C. of the presence of mobile electrons
14. How many sub-atomic particles are contained in ³⁷₁₇X⁴⁺ ? — A. 37
15. Liquid X has a sour taste. The pH value of X is likely to be — C. 5
16. Which of the following periodic properties increases from right to left in the periodic table? — A. Atomic radius
17. The flame test of a certain metal produced a yellow colouration. The metal is most likely to be — D. Na
18. Equal volumes of CH₄(g) and NH₃(g) at the same temperature and pressure would have the same — A. number of molecules
19. The effect of greenhouse gases could be reduced by — A. planting of trees
20. The value of y is — A. 8
21. A balloon was filled with a mixture containing equal volumes of H₂, He and N₂. The correct statement is — B. The pressure in the balloon would be a sum of the partial pressures of H₂, He and N₂
22. If carbon forms CN₄ and CY₄ with elements X and Y respectively, the formula of the compound formed between X and Y is — A. X₂Y
23. Which substance could be used in galvanization of iron to prevent rusting? — D. Zinc
24. The molar mass of a chloride of iron is 127 g mol⁻¹. The formula of the chloride is — A. FeCl₂
25. Which apparatus is used in transferring a solution into a burette during titration? — A. Funnel
26. When X was added to aqueous FeCl₃, its colour changed from reddish-brown to pale-green. X could be — A. LiAlH₄
27. Which of the following substances is a mixture? — C. Brine
28. An atom of chlorine could be converted to chloride ion by — D. reduction
29. The empirical formula of a compound is given as CₓHᵧO. Its relative molecular mass would be — D. 44
30. A molecule is the smallest independent particle of — B. an element
31. Which of the following acids is most volatile when concentrated? — A. HCl
32. The value of X in the redox half reaction is — A. 2
33. The simplest ratio of carbon atom to hydrogen atom in benzene represents — B. empirical formula
34. Potassium chloride may be used on farmlands because it — B. is essential for healthy plant growth
35. The mass of sodium hydroxide required to prepare 250 cm³ of 2.0 mol dm⁻³ NaOH(aq) is — D. 20 g
36. Ethanol could be produced from — C. sugar cane
37. X²⁺ is formed from X atom by — D. losing two electrons
38. It can be deduced that — D. the oxidation number of X increases
39. A particle made up of 10 electrons and 13 protons is — A. a cation
40. Magnesium oxide is an example of — D. a basic oxide
41. Degenerate orbitals are orbitals of — A. the same subshell having equal energy
42. The general formula of an alkyl group is — A. CₙH₂ₙ₊₁
43. Which of the following compounds is covalent? — D. HCl
44. The preparation of carbon(II) oxide is done in a fume cupboard because the gas is — C. poisonous
45. Which of the following elements would evolve hydrogen most rapidly from dilute HCl? — A. Zn
46. Which pair of enthalpy changes is always negative? — D. Combustion and neutralization
47. The reaction represented by the equation MgCl₂ + 2H₂O → Mg(OH)₂ + 2HCl is — D. hydrolysis
48. Y is a weak acid that turns blue and green when added to aqueous solutions of NaHSO₃ and Na₂CO₃ respectively. Y could be — C. an acid-base indicator
49. Which molecule possesses polar bonds but is non-polar? — A. Carbon(IV) oxide
50. A suitable substance used to purify ethanol is — A. calcium oxide
2026 WAEC CHEMISTRY (CHEM) THEORY (ESSAY) ANSWERS:
(1ai)
Suspension:
(PICK ANY ONE)
-Muddy water
-Sand in water
-Flour in water
(1aii)
Colloid:
(PICK ANY ONE)
-Milk
-Starch solution
-Fog
-Smoke
-Gelatin
(1b)
(PICK ANY ONE)
An isoelectronic series is a group of atoms or ions having the same number of electrons and the same electronic configuration.
OR
An isoelectronic series is a group of atoms, ions, or molecules that contain the same number of electrons but have different nuclear charges (different numbers of protons).
(1ci)
Heat of formation:
The heat change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.
(1aii)
Heat of combustion:
The heat evolved when one mole of a substance is completely burnt in excess oxygen under standard conditions.
(1d)
(PICK ANY ONE)
Helium is preferred to hydrogen because it is chemically inert and non-flammable. Whereas hydrogen is highly flammable and can form explosive mixtures with air. Therefore, helium is safer to use.
OR
Helium is preferred to hydrogen because it is a noble gas and is chemically inert, so it does not react readily and is non-flammable. Hydrogen, on the other hand, is highly flammable and can form explosive mixtures with air.
(1e)
(i) CO₂ – Linear
(ii) CH₄ – Tetrahedral
(iii) NH₃ – Trigonal pyramidal
(1f)
(i) Sulphur
(ii) Phosphorus
(1g)
(PICK ANY THREE)
(i) They exhibit variable oxidation states.
(ii) They form coloured ions or compounds.
(iii) They readily form complex ions
(iv) They act as catalysts.
(v) They have high melting and boiling points.
(1h)
(i) Aluminium
(ii) Sodium
(1i)
(PICK ANY ONE)
The atomic number of an element is the number of protons in the nucleus of an atom of that element.
OR
Atomic number is the number of protons contained in the nucleus of an atom of an element.
(1j)
(i) Ionic (electrovalent) bond between NH₄⁺ and Cl⁻.
(ii) Covalent bond between N and H atoms in NH₄⁺.
(iii) Dative (coordinate) bond formed when NH₃ donates a lone pair to H⁺ to form NH₄⁺.
Suspension:
(PICK ANY ONE)
-Muddy water
-Sand in water
-Flour in water
(1aii)
Colloid:
(PICK ANY ONE)
-Milk
-Starch solution
-Fog
-Smoke
-Gelatin
(1b)
(PICK ANY ONE)
An isoelectronic series is a group of atoms or ions having the same number of electrons and the same electronic configuration.
OR
An isoelectronic series is a group of atoms, ions, or molecules that contain the same number of electrons but have different nuclear charges (different numbers of protons).
(1ci)
Heat of formation:
The heat change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.
(1aii)
Heat of combustion:
The heat evolved when one mole of a substance is completely burnt in excess oxygen under standard conditions.
(1d)
(PICK ANY ONE)
Helium is preferred to hydrogen because it is chemically inert and non-flammable. Whereas hydrogen is highly flammable and can form explosive mixtures with air. Therefore, helium is safer to use.
OR
Helium is preferred to hydrogen because it is a noble gas and is chemically inert, so it does not react readily and is non-flammable. Hydrogen, on the other hand, is highly flammable and can form explosive mixtures with air.
(1e)
(i) CO₂ – Linear
(ii) CH₄ – Tetrahedral
(iii) NH₃ – Trigonal pyramidal
(1f)
(i) Sulphur
(ii) Phosphorus
(1g)
(PICK ANY THREE)
(i) They exhibit variable oxidation states.
(ii) They form coloured ions or compounds.
(iii) They readily form complex ions
(iv) They act as catalysts.
(v) They have high melting and boiling points.
(1h)
(i) Aluminium
(ii) Sodium
(1i)
(PICK ANY ONE)
The atomic number of an element is the number of protons in the nucleus of an atom of that element.
OR
Atomic number is the number of protons contained in the nucleus of an atom of an element.
(1j)
(i) Ionic (electrovalent) bond between NH₄⁺ and Cl⁻.
(ii) Covalent bond between N and H atoms in NH₄⁺.
(iii) Dative (coordinate) bond formed when NH₃ donates a lone pair to H⁺ to form NH₄⁺.
OR
(3ai)
(PICK ANY ONE)
Enthalpy of neutralization is the heat change that occurs when one mole of water is formed by the reaction between an acid and a base in dilute aqueous solution.
OR
Enthalpy of neutralization is the enthalpy change when one mole of H⁺ ions reacts completely with one mole of OH⁻ ions to form one mole of water.
(3aii)
H⁺(aq) + OH⁻(aq) --> H₂O(l)
(3bi)
W = Sodium propanoate (C₂H₅COONa)
X = Ethyl propanoate (C₂H₅COOC₂H₅)
Y = Propan-1-ol (CH₃CH₂CH₂OH)
Z = Propene (CH₃CH=CH₂)
(3aii)
CH₃CH₂COOH + CH₃CH₂OH ⇌ CH₃CH₂COOCH₂CH₃ + H₂O
(3ci)
(PICK ANY ONE)
An acid anhydride is an oxide of a non-metal that reacts with water to form an acid.
OR
An acid anhydride is a compound which on addition of water produces the corresponding acid.
(3cii)
(I) H₂SO₄ --- SO₃
(II) HNO₃ -- N₂O₅
(III) H₂CO₃ -- CO₂
(3di)
(PICK ANY ONE)
Aluminium is extracted from purified alumina (Al₂O₃) by the Hall-Héroult process. Alumina is dissolved in molten cryolite to lower its melting point and increase electrical conductivity. The molten mixture is electrolysed using carbon electrodes. During electrolysis, aluminium ions gain electrons at the cathode to form molten aluminium, while oxide ions lose electrons at the anode to form oxygen. The molten aluminium collects at the bottom of the cell and is tapped off periodically.
OR
Purified aluminium oxide is dissolved in molten cryolite and electrolysed in a steel tank lined with carbon. On passing electric current, Al³⁺ ions are discharged at the cathode to produce aluminium metal, while O²⁻ ions are discharged at the anode to produce oxygen gas. The molten aluminium settles at the bottom and is removed regularly.
(3dii)
Graphite electrodes
(3diii)
The carbon anode reacts with the oxygen produced during electrolysis to form CO₂ (and some CO), causing the anode to be gradually consumed; therefore it must be replaced periodically.
(3ei)
By Graham's law:
Rate of diffusion ∝ 1/√M
Given that gas X diffuses twice as fast as oxygen,
2 = √(32/Mₓ)
4 = 32/Mₓ
Mₓ = 32/4
Mₓ = 8
Relative molecular mass of X = 8
(PICK ANY ONE)
Enthalpy of neutralization is the heat change that occurs when one mole of water is formed by the reaction between an acid and a base in dilute aqueous solution.
OR
Enthalpy of neutralization is the enthalpy change when one mole of H⁺ ions reacts completely with one mole of OH⁻ ions to form one mole of water.
(3aii)
H⁺(aq) + OH⁻(aq) --> H₂O(l)
(3bi)
W = Sodium propanoate (C₂H₅COONa)
X = Ethyl propanoate (C₂H₅COOC₂H₅)
Y = Propan-1-ol (CH₃CH₂CH₂OH)
Z = Propene (CH₃CH=CH₂)
(3aii)
CH₃CH₂COOH + CH₃CH₂OH ⇌ CH₃CH₂COOCH₂CH₃ + H₂O
(3ci)
(PICK ANY ONE)
An acid anhydride is an oxide of a non-metal that reacts with water to form an acid.
OR
An acid anhydride is a compound which on addition of water produces the corresponding acid.
(3cii)
(I) H₂SO₄ --- SO₃
(II) HNO₃ -- N₂O₅
(III) H₂CO₃ -- CO₂
(3di)
(PICK ANY ONE)
Aluminium is extracted from purified alumina (Al₂O₃) by the Hall-Héroult process. Alumina is dissolved in molten cryolite to lower its melting point and increase electrical conductivity. The molten mixture is electrolysed using carbon electrodes. During electrolysis, aluminium ions gain electrons at the cathode to form molten aluminium, while oxide ions lose electrons at the anode to form oxygen. The molten aluminium collects at the bottom of the cell and is tapped off periodically.
OR
Purified aluminium oxide is dissolved in molten cryolite and electrolysed in a steel tank lined with carbon. On passing electric current, Al³⁺ ions are discharged at the cathode to produce aluminium metal, while O²⁻ ions are discharged at the anode to produce oxygen gas. The molten aluminium settles at the bottom and is removed regularly.
(3dii)
Graphite electrodes
(3diii)
The carbon anode reacts with the oxygen produced during electrolysis to form CO₂ (and some CO), causing the anode to be gradually consumed; therefore it must be replaced periodically.
(3ei)
By Graham's law:
Rate of diffusion ∝ 1/√M
Given that gas X diffuses twice as fast as oxygen,
2 = √(32/Mₓ)
4 = 32/Mₓ
Mₓ = 32/4
Mₓ = 8
Relative molecular mass of X = 8
OR
(3eii)
Volume of gas = 5 dm³
Molar volume at s.t.p. = 22.4 dm³ mol⁻¹
Number of moles = 5/22.4 = 0.223 mol
Mass = number of moles × molar mass
= 0.223 × 8
= 1.79 g
Mass of gas X = 1.79 g
≈ 1.8 g
(4ai)
(PICK ANY ONE)
Hydrogen gas is tested by bringing a lighted splint to the mouth of the container holding the gas. The gas burns with a characteristic squeaky pop sound, confirming the presence of hydrogen.
OR
Bring a lighted splint to the mouth of a container containing the gas. If the gas is hydrogen, it burns with a 'pop' sound.
(4aii)
(PICK ANY THREE)
(i) It is used in the manufacture of ammonia by the Haber process.
(ii) Hydrogenation of vegetable oils to make margarine.
(iii) It is used as a fuel (e.g., rocket fuel/fuel cells).
(iv) Oxy-hydrogen flame for welding and cutting metals.
(v) It is used in the preparation of hydrochloric acid.
(4aiii)
(I) Sodium metal:
2Na+H₂ --> NaH
(II) Copper(II) chloride solution:
CuCl₂+H₂ --> Cu+2HCl
(III) Chlorine gas:
H₂+Cl₂ --> 2HCl
(4bi)
(I)Tin:
(PICK ANY ONE)
(i) It is resistant to corrosion
(ii) It does not readily react with food.
(iii) It is non-toxic (harmless) to food.
(iv) It forms a protective oxide layer that prevents rusting/corrosion.
(II) Copper:
(PICK ANY ONE)
(i) It is a good conductor of electricity.
(ii) It is ductile (can be drawn into wires).
(iii) It has low electrical resistance.
(iv)It is resistant to corrosion.
(4bii)
(I) Iron:
(PICK ANY ONE)
(i) Haematite (Fe₂O₃)
(ii) Magnetite (Fe₃O₄)
(II) Tin:
Cassiterite(SnO₂)
(4biii)
(I) Iron:
(PICK ANY ONE)
-Steel
-Cast iron
(II) Copper:
(PICK ANY ONE)
-Brass
-Bronze
(4ci)
Coke
(4cii)
C+H₂O(g) --> CO+H₂
(4ciii)
Water gas
(4di)
(I) Tin:
Reduction of its oxide with carbon (smelting).
(II) Iron:
Reduction of its oxide with carbon monoxide in the blast furnace.
(III) Aluminium:
Electrolysis of purified alumina dissolved in molten cryolite.
(4dii)
(PICK ANY ONE)
(i) It is used in the manufacture of aircraft bodies.
(ii) It is used in the manufacture of cooking utensils .
(iii) It is used in the manufacture of overhead electrical cables.
(iv) It is used in the manufacture of roofing sheets.
(PICK ANY ONE)
Hydrogen gas is tested by bringing a lighted splint to the mouth of the container holding the gas. The gas burns with a characteristic squeaky pop sound, confirming the presence of hydrogen.
OR
Bring a lighted splint to the mouth of a container containing the gas. If the gas is hydrogen, it burns with a 'pop' sound.
(4aii)
(PICK ANY THREE)
(i) It is used in the manufacture of ammonia by the Haber process.
(ii) Hydrogenation of vegetable oils to make margarine.
(iii) It is used as a fuel (e.g., rocket fuel/fuel cells).
(iv) Oxy-hydrogen flame for welding and cutting metals.
(v) It is used in the preparation of hydrochloric acid.
(4aiii)
(I) Sodium metal:
2Na+H₂ --> NaH
(II) Copper(II) chloride solution:
CuCl₂+H₂ --> Cu+2HCl
(III) Chlorine gas:
H₂+Cl₂ --> 2HCl
(4bi)
(I)Tin:
(PICK ANY ONE)
(i) It is resistant to corrosion
(ii) It does not readily react with food.
(iii) It is non-toxic (harmless) to food.
(iv) It forms a protective oxide layer that prevents rusting/corrosion.
(II) Copper:
(PICK ANY ONE)
(i) It is a good conductor of electricity.
(ii) It is ductile (can be drawn into wires).
(iii) It has low electrical resistance.
(iv)It is resistant to corrosion.
(4bii)
(I) Iron:
(PICK ANY ONE)
(i) Haematite (Fe₂O₃)
(ii) Magnetite (Fe₃O₄)
(II) Tin:
Cassiterite(SnO₂)
(4biii)
(I) Iron:
(PICK ANY ONE)
-Steel
-Cast iron
(II) Copper:
(PICK ANY ONE)
-Brass
-Bronze
(4ci)
Coke
(4cii)
C+H₂O(g) --> CO+H₂
(4ciii)
Water gas
(4di)
(I) Tin:
Reduction of its oxide with carbon (smelting).
(II) Iron:
Reduction of its oxide with carbon monoxide in the blast furnace.
(III) Aluminium:
Electrolysis of purified alumina dissolved in molten cryolite.
(4dii)
(PICK ANY ONE)
(i) It is used in the manufacture of aircraft bodies.
(ii) It is used in the manufacture of cooking utensils .
(iii) It is used in the manufacture of overhead electrical cables.
(iv) It is used in the manufacture of roofing sheets.
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