POST UTME KSU 2017 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A metal $M$ has a s\tandard electrode potential of $-0.5, \text{V}$. What is the s\tandard electrode potential of $M^{2+}$?
A. $-1.0, \text{V}$
B. $-0.5, \text{V}$
C. $0.0, \text{V}$
D. $1.0, \text{V}$
Question 2
The diagram below shows a titration setup.
A. The burette is used to measure the volume of the titrant.
B. The beaker is used to measure the volume of the analyte.
C. The burette is used to measure the volume of the analyte.
D. The beaker is used to measure the volume of the titrant.
Question 3
A metal $M$ has a s\tandard electrode potential of $-0.5, \text{V}$. What is the s\tandard electrode potential of $M^{2+}$?
A. $-1.0, \text{V}$
B. $-0.5, \text{V}$
C. $0.0, \text{V}$
D. $1.0, \text{V}$
Question 4
A solution of $0.1, \text{mol}, \text{dm}^{-3}$ of $NaOH$ is mixed with a solution of $0.2, \text{mol}, \text{dm}^{-3}$ of $HCl$. If the volume of the resulting solution is $100, \text{cm}^3$, calculate the concentration of $OH^-$ ions.
A. $0.002, \text{mol}, \text{dm}^{-3}$
B. $0.01, \text{mol}, \text{dm}^{-3}$
C. $0.02, \text{mol}, \text{dm}^{-3}$
D. $0.05, \text{mol}, \text{dm}^{-3}$
Question 5
A 0.500 M solution of NaOH is titrated with a 0.500 M solution of HCl. What is the pH of the solution after the addition of 25.0 mL of HCl?
A. 2.00
B. 2.50
C. 3.00
D. 3.50
Question 6
A metal X reacts with chlorine gas to form a white solid. The reaction is represented by the equation: X + Cl2 → XCl2. What is the oxidation state of metal X in the product XCl2?
A. +1
B. +2
C. +3
D. +4
Question 7
A 1.00 M solution of NaOH is titrated with a 1.00 M solution of HCl. What is the pH of the solution after the addition of 50.0 mL of HCl?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 8
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(Ca(s)) = -178.2 kJ/mol.
A. -1206.8 kJ/mol
B. -1206.9 kJ/mol
C. -1206.7 kJ/mol
D. -1206.6 kJ/mol
Question 9
The pH of a solution is 4.5. What is the concentration of hydrogen ions in the solution?
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
Question 10
The diagram below shows a setup for the electrolysis of water.
A. O2 is produced at the anode
B. H2 is produced at the cathode
C. O2 is produced at the cathode
D. H2 is produced at the anode
Question 11
The diagram below shows a cell with a salt bridge.
A. The cell is a galvanic cell.
B. The cell is an electrolytic cell.
C. The salt bridge is used to connect the two half-cells.
D. The salt bridge is used to separate the two half-cells.
Question 12
A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.0025
B. 0.0050
C. 0.0075
D. 0.0100
Question 13
The reaction between chlorine gas and sodium hydroxide solution is represented by the equation: Cl2 + 2NaOH → NaCl + NaClO + H2O. What is the oxidation state of chlorine in the product NaClO?
A. 0
B. +1
C. +2
D. +3
Question 14
A solution of $0.1, \text{mol}, \text{dm}^{-3}$ of $NaOH$ is mixed with a solution of $0.2, \text{mol}, \text{dm}^{-3}$ of $HCl$. If the volume of the resulting solution is $100, \text{cm}^3$, calculate the concentration of $H^+$ ions.
A. $0.002, \text{mol}, \text{dm}^{-3}$
B. $0.01, \text{mol}, \text{dm}^{-3}$
C. $0.02, \text{mol}, \text{dm}^{-3}$
D. $0.05, \text{mol}, \text{dm}^{-3}$
Question 15
A solution of $0.1, \text{mol}, \text{dm}^{-3}$ of $NaOH$ is mixed with a solution of $0.2, \text{mol}, \text{dm}^{-3}$ of $HCl$. If the volume of the resulting solution is $100, \text{cm}^3$, calculate the concentration of $OH^-$ ions.
A. $0.002, \text{mol}, \text{dm}^{-3}$
B. $0.01, \text{mol}, \text{dm}^{-3}$
C. $0.02, \text{mol}, \text{dm}^{-3}$
D. $0.05, \text{mol}, \text{dm}^{-3}$

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