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POST UTME AAUA 2024 Chemistry | Objective

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Question 1

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

B. -1

Correct C. 0

D. +2

Correct Answer: C

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Question 2

A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution after the reaction is complete?

A. 1.00

Correct B. 2.00

C. 3.00

D. 4.00

Correct Answer: B

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Question 3

The diagram below shows a titration setup. What is the purpose of the burette?

Correct A. To measure the volume of the titrant

B. To measure the volume of the analyte

C. To mix the titrant and analyte

D. To measure the pH of the solution

Correct Answer: A

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Question 4

A polymer has a molecular weight of 50,000 g/mol and a degree of polymerization of 500. What is the molar mass of the monomer?

A. 100 g/mol

Correct B. 500 g/mol

C. 1000 g/mol

D. 5000 g/mol

Correct Answer: B

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Question 5

The diagram below shows a chemical apparatus setup. What is the purpose of the condenser?

Correct A. To cool the reaction mixture

B. To heat the reaction mixture

C. To mix the reac\tants

D. To measure the pH of the solution

Correct Answer: A

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Question 6

Determine the s\tandard electrode potential of the cell represented by the following reaction: MnO4- + 8H+ + 5e- → Mn2+ + 4H2O. Given that the s\tandard electrode potential of the MnO4-/Mn2+ couple is +1.23 V.

A. +1.23 V

Correct B. +1.38 V

C. +1.53 V

D. +1.68 V

Correct Answer: B

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Question 7

A sample of nitrogen gas is collected over water at a temperature of 25°C and a pressure of 1 atm. If the partial pressure of water vapor is 0.0313 atm, calculate the mole \fraction of nitrogen gas in the sample.

A. 0.999

Correct B. 0.998

C. 0.997

D. 0.996

Correct Answer: B

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Question 8

A 2.5 M solution of sodium hydroxide (NaOH) is prepared by dissolving 2.5 g of NaOH in 100 mL of water. Calculate the concentration of hydroxide ions \( OH- \) in the solution.

A. 0.05 M

Correct B. 0.10 M

C. 0.15 M

D. 0.20 M

Correct Answer: B

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Question 9

A 100 mL sample of a solution containing 0.1 M potassium chloride (KCl) is titrated with 0.1 M silver nitrate (AgNO3). Calculate the volume of AgNO3 required to reach the equivalence point.

A. 50 mL

Correct B. 75 mL

C. 100 mL

D. 125 mL

Correct Answer: B

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Question 10

A 2.0 g sample of a metal \( molar mass = 65 g/mol \) is dissolved in 100 mL of nitric acid (HNO3). The resulting solution is then titrated with 0.1 M sodium hydroxide (NaOH). Calculate the number of moles of NaOH required to reach the equivalence point.

A. 0.03 mol

B. 0.04 mol

Correct C. 0.05 mol

D. 0.06 mol

Correct Answer: C

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Question 11

In a reaction between hydrogen peroxide (H2O2) and potassium iodide (KI), the following equation is observed: 2H2O2 + 2KI + I2 → 2H2O + 2KIO3. If 25.0 mL of 0.100 M H2O2 is mixed with 25.0 mL of 0.100 M KI, what is the concentration of iodine (I2) produced after the reaction?

A. 0.0500 M

Correct B. 0.100 M

C. 0.200 M

D. 0.500 M

Correct Answer: B

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Question 12

A 1.00 L flask contains 0.500 mol of an ideal gas at 298 K. If the gas is heated to 373 K at cons\tant volume, what is the new pressure?

A. 1.00 atm

Correct B. 2.00 atm

C. 3.00 atm

D. 4.00 atm

Correct Answer: B

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Question 13

A solution contains 0.200 mol of a weak acid (HA) and 0.100 mol of its conjugate base \( A^- \). If the initial pH is 4.00, what is the new pH after the addition of 0.0500 mol of strong base \( OH^- \)?

A. 3.00

B. 4.00

Correct C. 5.00

D. 6.00

Correct Answer: C

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Question 14

A 1.00 L flask contains 0.500 mol of an ideal gas at 298 K. If the gas is compressed to 0.500 L at cons\tant temperature, what is the new pressure?

A. 2.00 atm

B. 3.00 atm

Correct C. 4.00 atm

D. 5.00 atm

Correct Answer: C

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Question 15

A 1.00 L flask contains 0.500 mol of an ideal gas at 298 K. If the gas is heated to 373 K at cons\tant pressure, what is the new volume?

A. 1.00 L

Correct B. 2.00 L

C. 3.00 L

D. 4.00 L

Correct Answer: B

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Question 16

Determine the pH of a 0.1 M solution of HCl after 10 mL of 0.1 M NaOH has been added to 20 mL of the HCl solution. Assume the volume of the resulting solution is 30 mL.

A. 1

Correct B. 2

C. 3

D. 4

Correct Answer: B

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Question 17

A 25 mL sample of a 0.5 M solution of NaOH is titrated with 0.5 M HCl. Calculate the volume of HCl required to reach the equivalence point.

A. 10 mL

B. 15 mL

Correct C. 20 mL

D. 25 mL

Correct Answer: C

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Question 18

A 50 mL sample of a 0.2 M solution of H2SO4 is mixed with 50 mL of a 0.2 M solution of NaOH. Calculate the pH of the resulting solution.

A. 1

B. 2

C. 3

Correct D. 4

Correct Answer: D

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Question 19

A 100 mL sample of a 0.1 M solution of HCl is titrated with 0.1 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.

A. 50 mL

B. 75 mL

Correct C. 100 mL

D. 125 mL

Correct Answer: C

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Question 20

A 50 mL sample of a 0.2 M solution of H2SO4 is mixed with 50 mL of a 0.2 M solution of NaOH. Calculate the concentration of the resulting solution.

A. 0.1 M

Correct B. 0.2 M

C. 0.3 M

D. 0.4 M

Correct Answer: B

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Question 21

The compound SO2 is classified as a(n) _______________________ oxide.

Correct A. dioxide

B. oxide

C. sulfide

D. sulfate

Correct Answer: A

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Question 22

A 2.5 g sample of a non-metallic element is found to have a mass of 3.75 g after being heated in a crucible. What is the percentage increase in mass?

A. 25%

Correct B. 50%

C. 75%

D. 100%

Correct Answer: B

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Question 23

The compound SO3 is classified as a(n) _______________________ oxide.

Correct A. trioxide

B. oxide

C. sulfide

D. sulfate

Correct Answer: A

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Question 24

A 2.5 g sample of a non-metallic element is found to have a mass of 3.75 g after being heated in a crucible. What is the percentage increase in mass?

A. 25%

Correct B. 50%

C. 75%

D. 100%

Correct Answer: B

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Question 25

The compound SO2 is classified as a(n) _______________________ oxide.

Correct A. dioxide

B. oxide

C. sulfide

D. sulfate

Correct Answer: A

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