Questions on Titration: Experiment, Calculations, and Curves
TITRATION: EXPERIMENT, CALCULATIONS, AND CURVES – MULTIPLE CHOICE QUESTIONS
1. What is the primary purpose of a titration experiment?
A) To measure temperature changes in a solution
B) To determine the color of a compound
C) To find the concentration of an unknown solution
D) To separate solid and liquid components
E) To observe gas evolution
2. Which piece of laboratory equipment is most commonly used to deliver the titrant?
A) Beaker
B) Pipette
C) Volumetric flask
D) Burette
E) Test tube
3. What is the equivalence point in a titration?
A) When the solution changes color
B) When the titrant is completely consumed
C) When the volume of titrant added equals the volume of analyte
D) When the amount of titrant added neutralizes the analyte
E) When the pH of the solution is 7
4. Which indicator is commonly used for strong acid–strong base titrations?
A) Methyl orange
B) Bromothymol blue
C) Phenolphthalein
D) Litmus
E) Universal indicator
5. Phenolphthalein changes color in what pH range?
A) 3.1 – 4.4
B) 6.0 – 7.6
C) 4.5 – 8.0
D) 8.2 – 10.0
E) 11.0 – 13.0
6. If 25.00 mL of NaOH is required to neutralize 50.00 mL of 0.10 M HCl, what is the concentration of NaOH?
A) 0.10 M
B) 0.20 M
C) 0.05 M
D) 0.25 M
E) 0.50 M
7. Which of the following is a correct unit for molarity?
A) mol/g
B) g/L
C) mol/L
D) mol/mL
E) mol/cm³
8. What is the shape of the pH curve for a strong acid–strong base titration?
A) Gradual curve with no steep section
B) Linear
C) Sigmoid with a sharp vertical jump at equivalence
D) Flat with a sudden dip
E) Exponential curve
9. In a weak acid–strong base titration, the pH at equivalence is typically:
A) Less than 4
B) Exactly 7
C) Around 3
D) Greater than 7
E) Equal to 2
10. Which titration would result in a pH less than 7 at equivalence?
A) Strong base vs. strong acid
B) Weak acid vs. weak base
C) Weak base vs. strong acid
D) Strong acid vs. strong base
E) Weak base vs. weak acid
11. What volume of 0.2 M NaOH is required to neutralize 25.0 mL of 0.1 M H₂SO₄?
A) 12.5 mL
B) 25.0 mL
C) 37.5 mL
D) 50.0 mL
E) 100.0 mL
12. Which of these indicators is suitable for a strong acid–weak base titration?
A) Phenolphthalein
B) Methyl orange
C) Thymol blue
D) Bromocresol green
E) Bromothymol blue
13. In titration, the analyte is:
A) Always an acid
B) Always a base
C) The solution in the burette
D) The unknown solution being analyzed
E) The standard solution
14. During titration, why is it important to swirl the flask constantly?
A) To cool the reaction
B) To mix the indicator properly
C) To ensure uniform mixing of the reactants
D) To speed up evaporation
E) To reduce color change
15. Which formula is used to calculate the unknown concentration in titration?
A) pH = -log[H⁺]
B) M₁V₁ = M₂V₂ (for monoprotic reactions)
C) PV = nRT
D) C = n/V
E) ΔT = mcΔT
16. Which of the following is not a suitable requirement for a successful titration?
A) Known concentration of titrant
B) Suitable indicator
C) Accurate volumetric equipment
D) Clear solution
E) High temperature
17. A titration curve for a polyprotic acid would show:
A) A single equivalence point
B) Multiple equivalence points
C) No change in pH
D) A straight line
E) Only one buffer region
18. A buffer region in a titration curve appears when:
A) All acid is neutralized
B) The base is added in excess
C) The pH is constantly changing
D) The solution resists changes in pH
E) The temperature is constant
19. Which of the following could cause errors in titration results?
A) Using a freshly calibrated burette
B) Reading burette volume at eye level
C) Not rinsing the burette with titrant
D) Adding indicator in small amounts
E) Using deionized water for cleaning
20. Which type of titration would require back titration techniques?
A) Weak acid vs. strong base
B) Strong acid vs. strong base
C) Reactions that are too slow to reach equilibrium directly
D) Acid-base neutralizations
E) Titrations using only aqueous solutions
- Questions on pOH Scale and Calculations
- Questions on Strong and Weak Acids and Acid Ionization Constant (Ka) and Base (Kb)
- Questions on Neutralization Reactions
ANSWER KEY
1. C – Titration is used to determine the concentration of an unknown solution by reacting it with a known solution.
2. D – A burette is used for the precise delivery of the titrant during titration.
3. D – The equivalence point is reached when stoichiometric amounts of acid and base have reacted.
4. C – Phenolphthalein is commonly used for strong acid–strong base titrations because of its sharp color change.
5. D – Phenolphthalein changes from colorless to pink in the pH range of 8.2–10.0.
6. B – Using the neutralization formula, (0.10 M × 50.00 mL) = (x × 25.00 mL), x = 0.20 M.
7. C – Molarity is expressed in mol/L (moles of solute per liter of solution).
8. C – A strong acid–strong base titration curve is S-shaped with a sharp vertical rise at equivalence.
9. D – At the equivalence point in a weak acid–strong base titration, the pH is typically above 7 due to the basic salt formed.
10. C – Titrating a weak base with a strong acid results in an acidic solution at equivalence.
11. D – H₂SO₄ is diprotic, so it reacts in a 1:2 ratio with NaOH. 25.0 mL × 0.1 M × 2 = 5.0 mmol. 5.0 mmol ÷ 0.2 M = 25.0 mL.
12. B – Methyl orange is suitable for titrations that result in acidic equivalence points, such as strong acid–weak base.
13. D – The analyte is the solution being analyzed, usually placed in the conical flask.
14. C – Swirling ensures proper mixing of titrant and analyte for an accurate reaction.
15. B – M₁V₁ = M₂V₂ is used when titrant and analyte react in a 1:1 molar ratio.
16. E – High temperature is not a requirement and may interfere with the reaction.
17. B – Polyprotic acids like H₃PO₄ have more than one dissociable proton, leading to multiple equivalence points.
18. D – A buffer region is where the solution resists pH changes, typically before equivalence.
19. C – Not rinsing the burette with the titrant can introduce dilution errors.
20. C – Back titration is used when the reaction is slow or the endpoint is not easily detectable directly.
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