POST UTME CHRISTOPHER UNIVERSITY 2022 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A 1.0 M solution of a weak base B is titrated with 1.0 M HCl. If 20 mL of HCl is required to reach the equivalence point, what is the pOH of the resulting solution?
A. \( pOH = 1 \)
B. \( pOH = 2 \)
C. \( pOH = 3 \)
D. \( pOH = 4 \)
Question 2
A solution contains 5.0 g of glu\cose (C6H12O6) per 100 mL. Calculate the molarity of the solution.
A. 0.1 M
B. 0.2 M
C. 0.3 M
D. 0.4 M
Question 3
A 10.0 mL sample of a solution containing 0.10 M AgNO3 is mixed with 10.0 mL of a solution containing 0.10 M NaCl. What is the concentration of the resulting solution?
A. 0.05 M
B. 0.10 M
C. 0.15 M
D. 0.20 M
Question 4
Determine the molar solubility of BaSO4 in 0.1 M Na2SO4 solution, given that the solubility product cons\tant (Ksp) of BaSO4 is 1.1 × 10^\( -10 \).
A. 1.0 × 10^\( -5 \) M
B. 1.0 × 10^\( -6 \) M
C. 1.0 × 10^\( -7 \) M
D. 1.0 × 10^\( -8 \) M
Question 5
A 25.0 mL sample of a solution containing 0.10 M NaOH is titrated with 0.10 M HCl. What is the pH of the solution after the titration?
A. 7.00
B. 7.50
C. 8.00
D. 9.00
Question 6
A 0.1 M solution of a weak acid HA is titrated with 0.1 M NaOH. If 20 mL of NaOH is required to reach the equivalence point, what is the pH of the resulting solution?
A. \( pH = 7 \)
B. \( pH = 3 \)
C. \( pH = 10 \)
D. \( pH = 12 \)
Question 7
A metal M (atomic number 24) reacts with oxygen gas to form a compound MO2. If the molar mass of MO2 is 160 g/mol, what is the atomic mass of M?
A. \( 24.5 g/mol \)
B. \( 25.5 g/mol \)
C. \( 26.5 g/mol \)
D. \( 27.5 g/mol \)
Question 8
A 2.5 g sample of a subs\tance is dissolved in 50.0 mL of water. If the molar mass of the subs\tance is 120.0 g/mol, what is the concentration of the solution in units of M?
A. 0.05 M
B. 0.10 M
C. 0.15 M
D. 0.20 M
Question 9
A solution of 0.1 M HCl is titrated with 0.1 M NaOH. The pH of the solution at the equivalence point is 7. Calculate the initial volume of the HCl solution required to reach the equivalence point.
A. 50 mL
B. 100 mL
C. 150 mL
D. 200 mL
Question 10
What is the periodic tr\end for atomic radius across a period in the periodic table?
A. Increases
B. Decreases
C. Remains cons\tant
D. Varies randomly
Question 11
What is the formula for the compound formed when sulfur reacts with oxygen?
A. SO2
B. SO3
C. SO4
D. SO5
Question 12
A 0.1 M solution of NaOH is mixed with a 0.1 M solution of HCl. Determine the pH of the resulting solution.
A. 1.0
B. 2.0
C. 3.0
D. 4.0
Question 13
A 5.0 g sample of a subs\tance is burned in a bomb calorimeter. If the heat released is 1200 J/g, what is the enthalpy change for the combustion reaction?
A. 6000 J/mol
B. 8000 J/mol
C. 10000 J/mol
D. 12000 J/mol
Question 14
In a redox reaction, what is the role of the oxidizing agent?
A. To donate electrons
B. To accept electrons
C. To facilitate the reaction
D. To inhibit the reaction
Question 15
A 2.5 g sample of a metal carbonate is heated to produce a metal oxide. If the mass of the metal oxide is 2.0 g, calculate the percentage of the metal in the metal carbonate.
A. 20%
B. 25%
C. 30%
D. 35%

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