POST UTME IMS U 2019 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
Determine the s\tandard enthalpy of formation of CaCO3(s) from the following data: ΔHf(CaO(s)) = -635.09 kJ/mol, ΔHf(CO2(g)) = -393.51 kJ/mol, ΔHf(C(s)) = 0 kJ/mol.
A. -1206.60 kJ/mol
B. -1206.61 kJ/mol
C. -1206.59 kJ/mol
D. -1206.62 kJ/mol
Question 2
A 5.00 g sample of a metal hydroxide is dissolved in water to produce a solution with a pH of 10.5. If the metal hydroxide is a strong base, what is the concentration of the resulting solution?
A. 0.0500 M
B. 0.0625 M
C. 0.0750 M
D. 0.0875 M
Question 3
Determine the number of moles of oxygen gas (O2) produced at STP when 2.5 moles of hydrogen gas (H2) react with oxygen gas according to the equation: 2H2 + O2 → 2H2O.
A. 1.25 moles
B. 2.5 moles
C. 3.75 moles
D. 5 moles
Question 4
A solution containing 0.50 M NaCl is prepared by dissolving 0.50 g of NaCl in 100 mL of water. Calculate the molar concentration of the solution.
A. 0.25 M
B. 0.50 M
C. 0.75 M
D. 1.00 M
Question 5
A 2.0 g sample of a metal is dissolved in 10 mL of 1 M HCl. If the resulting solution has a pH of 1.5, what is the concentration of the metal ion in the solution?
A. 0.1 M
B. 0.01 M
C. 0.001 M
D. 0.0001 M
Question 6
At 273 K, the volume of 1 mole of an ideal gas is 22.4 L. What is the volume of 2 moles of the same gas at the same temperature?
A. 44.8 L
B. 45.6 L
C. 46.4 L
D. 47.2 L
Question 7
The diagram below shows a titration setup.
A. The burette contains NaOH.
B. The burette contains HCl.
C. The beaker contains NaOH.
D. The beaker contains HCl.
Question 8
A 0.500 M solution of NaOH is mixed with a 0.500 M solution of HCl. What is the pH of the resulting solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 9
A diagram of a titration setup is shown below. What is the purpose of the burette in this setup?
A. To measure the volume of the acid
B. To measure the volume of the base
C. To mix the acid and base
D. To measure the pH of the solution
Question 10
A 2.5 L flask contains 0.5 mol of an ideal gas at 27°C. Calculate the pressure of the gas.
A. 1 atm
B. 2 atm
C. 3 atm
D. 4 atm
Question 11
A 1.0 M solution of H2SO4 is titrated with 1.0 M NaOH. If 20 mL of NaOH is required to reach the equivalence point, what is the volume of H2SO4 in liters?
A. 0.02 L
B. 0.02 mL
C. 0.2 L
D. 0.2 mL
Question 12
A 2.5 L flask contains 0.5 mol of an ideal gas at 27°C. Calculate the volume of the gas at 37°C.
A. 2.5 L
B. 3 L
C. 4 L
D. 5 L
Question 13
Calculate the molar solubility of AgCl in a 0.1 M solution of NaCl.
A. 0.01 M
B. 0.1 M
C. 1 M
D. 10 M
Question 14
A 1.00 M solution of Ca(OH)2 is mixed with a 1.00 M solution of HCl. What is the pH of the resulting solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 15
Determine the pH of a 0.1 M solution of HCl.
A. 1
B. 2
C. 3
D. 4

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