POST UTME COVENANT UNIVERSITY 2017 Chemistry | Objective

Are you preparing for POST UTME COVENANT UNIVERSITY exams? Reviewing past questions is one of the most effective ways to guarantee a high score. This practice hub features authentic 2017 Chemistry (Objective) questions designed to simulate the real exam environment.

Practice these randomly selected questions to test your readiness.

Question 1
Determine the pH of a 0.1 M solution of HCl.
Correct A. 1
B. 2
C. 3
D. 4

Correct Answer: A

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Question 2
A 2.5 g sample of a polymer is dissolved in 100 mL of a solvent. Calculate the molar mass of the polymer.
A. 100 g/mol
B. 200 g/mol
Correct C. 500 g/mol
D. 1000 g/mol

Correct Answer: C

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Question 3
A cell is placed in a 0.1 M solution of KCl. Calculate the potential of the cell.
A. -0.1 V
Correct B. -0.2 V
C. -0.3 V
D. -0.4 V

Correct Answer: B

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Question 4
A 1.0 M solution of NaOH is titrated with a 1.0 M solution of HCl. Calculate the pH of the solution after 10 mL of HCl has been added.
A. 1
B. 2
Correct C. 3
D. 4

Correct Answer: C

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Question 5
A 2.0 g sample of a metal is heated in a crucible. Calculate the mass of the metal after 1 hour.
A. 1.5 g
B. 2.0 g
Correct C. 2.5 g
D. 3.0 g

Correct Answer: C

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Question 6
A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
A. 12.5 mL
B. 25.0 mL
Correct C. 37.5 mL
D. 50.0 mL

Correct Answer: C

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Question 7
The pH of a solution is 4.25. Calculate the concentration of H+ ions in the solution.
Correct A. 1.0 x 10^-4 M
B. 1.0 x 10^-5 M
C. 1.0 x 10^-6 M
D. 1.0 x 10^-7 M

Correct Answer: A

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Question 8
A 2.50 g sample of a metal carbonate is heated to produce a metal oxide and carbon dioxide gas. The mass of the metal oxide produced is 2.00 g. Calculate the percentage yield of the metal oxide.
A. 80.0%
B. 85.0%
Correct C. 90.0%
D. 95.0%

Correct Answer: C

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Question 9
A solution contains 0.250 M NaCl and 0.150 M CaCl2. Calculate the total concentration of ions in the solution.
A. 0.400 M
B. 0.450 M
Correct C. 0.500 M
D. 0.550 M

Correct Answer: C

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Question 10
A 5.00 g sample of a metal hydroxide is treated with 20.0 mL of 1.00 M HCl. Calculate the mass of the metal chloride produced.
A. 2.50 g
B. 3.00 g
Correct C. 3.50 g
D. 4.00 g

Correct Answer: C

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Question 11
A 0.1 M solution of a weak base, B, has a pH of 8.5. If 10 mL of 1 M HCl is added to 90 mL of the base solution, what is the pH of the resulting solution?
A. 7.5
B. 8.5
Correct C. 9.5
D. 10.5

Correct Answer: C

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Question 12
A sample of a hydrocarbon, C_xH_y, has a molecular weight of 42 g/mol. If 1.5 g of the sample is burned in a combustion tube, 1.2 L of CO2 and 0.9 L of H2O are produced at STP. What is the empirical formula of the hydrocarbon?
Correct A. C2H6
B. C3H8
C. C4H10
D. C5H12

Correct Answer: A

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Question 13
A 1.0 M solution of a strong acid, HA, has a pH of 1.0. If 10 mL of 1 M NaOH is added to 90 mL of the acid solution, what is the pH of the resulting solution?
A. 2.0
Correct B. 3.0
C. 4.0
D. 5.0

Correct Answer: B

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Question 14
A sample of a salt, NaCl, is dissolved in water to form a 0.1 M solution. If 10 mL of 1 M HCl is added to 90 mL of the salt solution, what is the pH of the resulting solution?
A. 1.0
B. 2.0
C. 3.0
Correct D. 4.0

Correct Answer: D

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Question 15
A 0.1 M solution of a weak acid, HA, has a pH of 4.0. If 10 mL of 1 M NaOH is added to 90 mL of the acid solution, what is the pH of the resulting solution?
A. 3.0
Correct B. 4.0
C. 5.0
D. 6.0

Correct Answer: B

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Question 16
The reaction of zinc metal with copper(II) sulfate solution is represented by the equation: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s). What is the oxidation state of copper in the product Cu(s)?
A. +1
Correct B. 0
C. +2
D. -1

Correct Answer: B

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Question 17
The solubility of lead(II) chloride in water is 1.7 g/100 mL at 20°C. What is the molar solubility of lead(II) chloride in water at 20°C?
Correct A. 0.01 M
B. 0.1 M
C. 0.5 M
D. 1.0 M

Correct Answer: A

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Question 18
The half-life of a radioactive subs\tance is 5 days. If 100 mg of the subs\tance is present initially, how much of the subs\tance will remain after 15 days?
A. 50 mg
B. 25 mg
Correct C. 12.5 mg
D. 6.25 mg

Correct Answer: C

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Question 19
The reaction of sodium hydroxide with hydrochloric acid is represented by the equation: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l). What is the pH of the solution after the reaction?
Correct A. 7
B. 8
C. 9
D. 10

Correct Answer: A

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Question 20
The diagram below shows a setup for the electrolysis of water. What is the purpose of the anode in this setup?
A. To release oxygen gas
Correct B. To release hydrogen gas
C. To release chlorine gas
D. To release bromine gas

Correct Answer: B

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Question 21
The reaction between sulfur dioxide and oxygen to form sulfur trioxide is highly exothermic. What is the value of ΔH for this reaction, given that the s\tandard enthalpy of formation of SO2 is -296.8 kJ/mol and the s\tandard enthalpy of formation of SO3 is -395.7 kJ/mol?
Correct A. -99.9 kJ/mol
B. -99.1 kJ/mol
C. -98.3 kJ/mol
D. -97.5 kJ/mol

Correct Answer: A

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Question 22
A 2.50 M solution of sodium hydroxide is mixed with a 1.00 M solution of hydrochloric acid. What is the concentration of the resulting solution?
A. 1.75 M
Correct B. 2.25 M
C. 2.50 M
D. 3.00 M

Correct Answer: B

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Question 23
A sample of a non-metallic element has a mass of 25.0 g and a volume of 5.00 mL. What is the density of the element?
Correct A. 5.00 g/mL
B. 5.50 g/mL
C. 6.00 g/mL
D. 6.50 g/mL

Correct Answer: A

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Question 24
A 1.00 M solution of potassium nitrate is mixed with a 2.00 M solution of sodium chloride. What is the concentration of the resulting solution?
A. 1.00 M
B. 1.50 M
Correct C. 2.00 M
D. 2.50 M

Correct Answer: C

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Question 25
A sample of a metal has a mass of 30.0 g and a volume of 10.0 mL. What is the density of the element?
A. 3.00 g/mL
B. 3.50 g/mL
Correct C. 4.00 g/mL
D. 4.50 g/mL

Correct Answer: C

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