POST UTME JOSEPH AYO BABALOLA UNIVERSITY 2018 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A 0.1 M solution of a weak base B(OH)3 is titrated with 0.1 M HCl. If the initial pH of the solution is 9.5, what is the pH after the addition of 20 mL of 0.1 M HCl?
A. 5.5
B. 6.5
C. 7.5
D. 8.5
Question 2
A 2.0 M solution of a strong acid HCl is mixed with a 2.0 M solution of a weak base NH3. What is the pH of the resulting solution?
A. 1.0
B. 2.0
C. 3.0
D. 4.0
Question 3
A 2.0 M solution of sodium hydroxide (NaOH) is prepared by dissolving 40 g of NaOH in 1 L of water. What is the molarity of the solution?
A. 1.0 M
B. 2.0 M
C. 3.0 M
D. 4.0 M
Question 4
A 2 M solution of HCl is prepared by dissolving 40 g of HCl in water to make 1 L of solution. What is the molarity of the solution?
A. 2 M
B. 4 M
C. 6 M
D. 8 M
Question 5
The reaction of sodium hydroxide with hydrochloric acid is represented by the equation: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l). Calculate the number of moles of sodium chloride formed when 2.50 g of NaOH is mixed with 2.50 g of HCl.
A. 0.050 mol
B. 0.100 mol
C. 0.150 mol
D. 0.200 mol
Question 6
A 0.1 M solution of NaOH is prepared by dissolving 4 g of NaOH in water to make 1 L of solution. What is the molarity of the solution?
A. 0.1 M
B. 0.5 M
C. 1 M
D. 2 M
Question 7
A 100.0 mL sample of 0.200 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution after the addition of 50.0 mL of NaOH?
A. 1
B. 2
C. 3
D. 4
Question 8
The molar mass of a compound is 180 g/mol. If 2.5 g of the compound is dissolved in 250 mL of water, what is the concentration of the solution in mol/L?
A. 0.014 M
B. 0.028 M
C. 0.056 M
D. 0.112 M
Question 9
A 2.5 L sample of a solution containing 0.1 M NaCl is electrolyzed u\sing a platinum electrode. What is the mass of chlorine gas produced at the anode?
A. 0.05 g
B. 0.1 g
C. 0.2 g
D. 0.5 g
Question 10
A 0.500 M solution of HCl is prepared by dissolving 25.0 g of HCl in enough water to make 1.00 L of solution. Calculate the pH of the solution.
A. 0.5
B. 1.0
C. 1.5
D. 2.0
Question 11
A 1.5 L sample of oxygen gas is collected over water at a temperature of 25°C and a pressure of 1.2 atm. What is the partial pressure of the oxygen gas?
A. 1.0 atm
B. 1.1 atm
C. 1.2 atm
D. 1.3 atm
Question 12
The reaction of sodium hydroxide with hydrochloric acid is represented by the equation: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l). Calculate the number of moles of sodium chloride formed when 2.50 g of NaOH is mixed with 2.50 g of HCl.
A. 0.050 mol
B. 0.100 mol
C. 0.150 mol
D. 0.200 mol
Question 13
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. What is the s\tandard enthalpy of combustion of 1 mole of C6H12O6(s) at 298 K?
A. -2800 kJ/mol
B. -2900 kJ/mol
C. -3000 kJ/mol
D. -3100 kJ/mol
Question 14
The s\tandard enthalpy of combustion of methane (CH4) is -890.3 kJ/mol. Calculate the s\tandard enthalpy of formation of methane u\sing the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l).
A. -74.8 kJ/mol
B. -75.0 kJ/mol
C. -75.2 kJ/mol
D. -75.4 kJ/mol
Question 15
What is the major difference between the periodic table of elements and the periodic table of atomic masses?
A. The periodic table of elements is arranged by atomic mass, while the periodic table of atomic masses is arranged by atomic number.
B. The periodic table of elements is arranged by atomic number, while the periodic table of atomic masses is arranged by atomic mass.
C. The periodic table of elements is arranged by electron configuration, while the periodic table of atomic masses is arranged by atomic number.
D. The periodic table of elements is arranged by atomic mass, while the periodic table of atomic masses is arranged by electron configuration.

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