Quiz  /  Acid Base Titration Class 12 MCQ Questions With Answers

  • 1. 
    From the list of indicators shown, choose one that is suitable for this reaction.

  • Phenolphthalein
  • Bromophenol Blue
  • Bromocresol Green
  • Any indicator can be used and an accurate result will be obtained.

  • 2. 
    Identify the strongest acid

  • HCN
  • H2O
  • CH3OH
  • HNO3

  • 3. 
    The concentration of the 30ml of citric acid solution is determined to be 1.23 M. Using the titration equation, predict the titration volume for the standard solution of 2.3 M.

  • 14 ml
  • 15 ml
  • 16 ml
  • 17 ml

  • 4. 
    What is the endpoint of a titration

  • Where the amount of acid and base are equal as shown by a colour change
  • Where there is no base
  • When the volume of base in the burette is used up
  • When there is no acid

  • 5. 
    Which acid base pair will produce a pH jump from 2.7 to 11.3 at equivalent point?

  • HCI and NH3
  • HCI and NaOH
  • CH3COOH and NH3
  • CH3COOH and NaOH

  • 6. 
    In the titration equation, M1V1 = M2V2, what is M?

  • Molarity
  • Concentration
  • Amount of solution
  • Both A & B

  • 7. 
    In which of the following reactions does H2PO4- act as an acid?

  • H3PO4 + H2O --> H3O+ + H2PO4-
  • H2PO4- + H2O --> H3O+ + HPO42-
  • H2PO4- + OH- --> H3PO4 + O2-
  • The ion cannot act as an acid

  • 8. 
    The name of the apparatus used for holding the titrant is__________

  • Conical flask
  • Burette
  • Pipette
  • Volumetric flask

  • 9. 
    Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion in solution in largest concentration, other than the K+ ion, is

  • H2PO4 –
  • HPO4 2–
  • PO4 3–
  • OH-

  • 10. 
    The tirant is also known as_________

  • Standard solution
  • Saturated solution
  • Concentrated solution
  • Super solution

  • 11. 
    Using n = MV, calculate the mass required to prepare 2.5 L of 1.0 M NaOH solution. Given the MM for NaOH is 40 g/mol

  • 1000 g
  • 100 g
  • 10 g
  • 1 kg

  • 12. 
    20ml of 0.1M of acids are used below, which acid require a diff vol to neutralize 0.1M NaOH?

  • Nitric acid
  • Sulfuric acid
  • Ethanoic acid
  • Hydrochloric acid

  • 13. 
    Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

  • Q
  • R
  • S
  • T

  • 14. 
    Which acid base pair will produce a pH jump from 2.7 to 7.8 at equivalent point?

  • HCI with CH3COOH
  • HCI with NaOH
  • CH3COOH with NaOH
  • HCI with NH3

  • 15. 
    In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment?

  • The [H+] at the equivalence point equals the ionization constant of the acid.
  • The pH at the equivalence point depends on the indicator used.
  • The graph of pH versus volume of base added rises gradually at first and then much more rapidly.
  • The graph of pH versus volume of base added shows no sharp rise.

  • 16. 
    I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?

  • 0.8 M
  • 1 M
  • 1.25 M

  • 17. 
    What is the initial pH value when ethanoic acid was added into sodium hydroxide?

  • 13.0
  • 11.0
  • 3.5
  • 2.0

  • 18. 
    Which type of titration is shown by this titration curve?

  • Titration of a strong acid by a strong base
  • Titration of a weak acid by a strong base
  • Titration of a strong base by a strong acid
  • Titration of a weak base by a strong acid

  • 19. 
    CH3COOH is titrated with NaOH. Name the salt produced and its pH at the equivalence point.

  • CH3COONa, pH at 5
  • CH3COONa, pH at 7
  • CH3COONa, pH at 9
  • NaCH3COO, pH at 9

  • 20. 
    Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest?

  • Beaker 1
  • Beaker 2
  • Beaker 3
  • Beaker 4

  • 21. 
    In acid-base titration, the equivalent point is when

  • a certain amount of acid has reacted completely with a certain amount of base according to stoichiometry
  • a certain amount of acid has reacted partially with a certain amount of base according to stoichiometry

  • 22. 
    Ascorbic acid, H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10–5 and K2 = 1.6 × 10–12. In a 0.005 M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration?

  • H3O+(aq)
  • H2C6H6O6(aq)
  • HC6H6O6-(aq)
  • C6H6O62-(aq)

  • 23. 
    What is the pH at the equivalence point.

  • The pH is approximately 5
  • The pH is approximately 6
  • The pH is approximately 8
  • The pH is approximately 9

  • 24. 
    What is the concentration of citric acid if its volume is 25 ml and the titrated volume of the standard solution of 0.75 M is 12.4 ml

  • 0.47
  • 0.37
  • 0.30
  • 0.17

  • 25. 
    Using n = MV, calculate the number of moles of sodium chloride in a 1.7 L solution of 0.35 M.

  • 0.456 mol
  • 0.234 mol
  • 0.643 mol
  • 0.595 mol

  • 26. 
    The pH at the equivalence point of the titration of a weak acid with a strong base is usually:

  • acidic 3.9
  • acidic 4.5
  • neutral 7.0
  • basic 8.2

  • 27. 
    At point P in the titration, which of the following species has the highest concentration?

  • HA
  • A–
  • H3O+
  • OH–

  • 28. 
    Which curve is produced by the addition of a 0.1 molL-1 strong acid to a 0.1 molL-1 weak base?

  • A
  • B
  • C
  • D
Report Question
warning
access_time
  Time