Questions About Dilution
Multiple-Choice Questions – Dilution
1. What does the process of dilution involve?
A) Increasing the temperature of a solution
B) Adding more solute to a solution
C) Adding solvent to decrease the solution's concentration
D) Heating the solute
E) Separating the solute from the solvent
2. Which equation is commonly used for dilution calculations?
A) PV = nRT
B) M = mol/L
C) M₁V₁ = M₂V₂
D) C₁ + C₂ = C₃
E) M₁ + M₂ = M₃
3. What happens to the number of moles of solute during dilution?
A) Increases
B) Decreases
C) Doubles
D) Remains the same
E) Becomes zero
4. A 2.0 M solution is diluted from 100 mL to 400 mL. What is the final concentration?
A) 0.25 M
B) 0.5 M
C) 1.0 M
D) 2.0 M
E) 4.0 M
5. A 1.5 M solution is diluted to twice its original volume. What is the new concentration?
A) 3.0 M
B) 1.5 M
C) 0.75 M
D) 0.5 M
E) 1.0 M
6. If 100 mL of a 3.0 M solution is diluted to 300 mL, what is the final molarity?
A) 1.0 M
B) 2.0 M
C) 3.0 M
D) 0.5 M
E) 0.25 M
7. What volume of water should be added to 50 mL of 6.0 M HCl to make a 1.0 M solution?
A) 250 mL
B) 300 mL
C) 350 mL
D) 400 mL
E) 450 mL
8. In the formula M₁V₁ = M₂V₂, M₁ stands for:
A) Final molarity
B) Volume of solvent
C) Initial molarity
D) Moles of solute
E) Molar mass
9. In dilution, which of the following remains constant?
A) Volume
B) Temperature
C) Number of solute particles
D) Concentration
E) Pressure
10. Which action best describes diluting a solution?
A) Evaporating the solvent
B) Adding solute
C) Adding more solution
D) Adding solvent
E) Removing solute
11. A student dilutes 100 mL of 2.0 M NaOH to 200 mL. What is the new concentration?
A) 4.0 M
B) 2.0 M
C) 1.0 M
D) 0.5 M
E) 0.25 M
12. What is the final volume when 20 mL of 5.0 M solution is diluted to 1.0 M?
A) 25 mL
B) 50 mL
C) 75 mL
D) 100 mL
E) 120 mL
13. What is the purpose of dilution in laboratory practice?
A) To increase solution’s temperature
B) To reduce concentration
C) To remove solute
D) To separate components
E) To concentrate a solution
14. A chemist has 10 mL of 6 M HNO₃. How much water is needed to prepare 30 mL of 2 M HNO₃?
A) 10 mL
B) 20 mL
C) 25 mL
D) 30 mL
E) 50 mL
15. Molarity after dilution depends on:
A) Volume of solute
B) Type of solute
C) Final volume only
D) Initial moles and final volume
E) Initial concentration only
16. What is the result of diluting a 0.8 M solution to four times its volume?
A) 0.1 M
B) 0.2 M
C) 0.4 M
D) 0.8 M
E) 1.6 M
17. 25 mL of a 4.0 M solution is diluted to 100 mL. Final molarity is:
A) 0.25 M
B) 1.0 M
C) 2.0 M
D) 3.0 M
E) 4.0 M
18. In M₁V₁ = M₂V₂, what does V₂ represent?
A) Initial volume
B) Final volume
C) Molar mass
D) Total moles
E) Volume of solute only
19. What volume of 10 M HCl is needed to prepare 500 mL of 1 M solution?
A) 10 mL
B) 25 mL
C) 50 mL
D) 100 mL
E) 200 mL
20. A 200 mL solution of 0.5 M is diluted to 1.0 L. What is the new molarity?
A) 0.1 M
B) 0.2 M
C) 0.25 M
D) 0.4 M
E) 0.5 M
- Questions on Solubility and Henry's Law of Solubility
- Questions About Molarity
- Questions About Molality
Answer Key with Full Explanations
1. C – Dilution decreases concentration by adding solvent, not solute.
2. C – The correct formula is M₁V₁ = M₂V₂.
3. D – The amount of solute remains constant during dilution.
4. B – M₂ = (2.0 M × 100 mL) / 400 mL = 0.5 M.
5. C – Doubling volume halves concentration: 1.5 M → 0.75 M.
6. A – M₂ = (3.0 × 100) / 300 = 1.0 M.
7. D – M₂ = (6.0 × 50) / x = 1.0 → x = 300 mL, water added = 250 mL.
8. C – M₁ = initial molarity.
9. C – Solute amount (moles) does not change during dilution.
10. D – Adding solvent dilutes a solution.
11. C – M₂ = (2.0 × 100) / 200 = 1.0 M.
12. D – V₂ = (5.0 × 20) / 1.0 = 100 mL.
13. B – Dilution reduces concentration for safe or precise handling.
14. B – M₁V₁ = M₂V₂ → 6×10 = 2×x → x = 30 → water = 20 mL.
15. D – Final molarity = moles / final volume.
16. B – 0.8 / 4 = 0.2 M.
17. B – M₂ = (4.0 × 25) / 100 = 1.0 M.
18. B – V₂ is the final volume after dilution.
19. C – 10 × x = 1 × 500 → x = 50 mL.
20. A – M₂ = (0.5 × 200) / 1000 = 0.1 M.
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