Quiz  /  Acid Base Titration Gate & PSU 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. 
    Scale that measures how acidic or basic something is.

  • aH
  • bH
  • pH
  • Hp

  • 3. 
    Identify the strongest acid

  • HCN
  • H2O
  • CH3OH
  • HNO3

  • 4. 
    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

  • 5. 
    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

  • 6. 
    In addition to neutralization, what other class of reaction occurs between KHP and NaOH solutions?

  • combustion
  • double replacement
  • single replacement
  • composition

  • 7. 
    A titration involves the chemical reaction between an analyte solution and the

  • titrant
  • titrator
  • standard
  • all of the above

  • 8. 
    Choose the CORRECT definition of acidimetry

  • the determination of the concentration of an acid
  • the determination of the concentration of a base
  • the determination of the amount of an acid
  • the determination of the amount of a base

  • 9. 
    If the Erlenmeyer flask contains acidic solution and a few drops of phenolphthalein, its color will be

  • pink
  • blue
  • red
  • colorless

  • 10. 
    What is the normal pH of gastric (stomach) juices?

  • 3
  • 6
  • 9
  • I don't drink juice

  • 11. 
    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

  • 12. 
    In the titration equation, M1V1 = M2V2, what is M?

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

  • 13. 
    What is the impact of adding small volume of water to the KHP in the Erlenmeyer in Part A?

  • dilutes KHP so less base solution required to neutralize
  • need to add a lil bit more KHP to even things out
  • must redo titration
  • no impact; only need approximate KHP solution volume for Part A

  • 14. 
    Which pH is considered neutral?

  • 1
  • 3
  • 7
  • 14

  • 15. 
    What color is phenolphthalein in a base?

  • colorless
  • pink
  • blue
  • green

  • 16. 
    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

  • 17. 
    How many mL of a 0.12 M NaOH solution are needed to neutralize 18 mL of 0.15 M H3PO4 solution?3NaOH (aq) + H3PO4 (aq) ----> Na3PO4 (aq) + 3H2O (l)

  • 7.5 mL
  • 0.015 mL
  • 68 mL
  • 23 mL

  • 18. 
    If a 40 mL solution of HCl required only 10 mL of NaOH titrant to reach the equivalence point, the relative molar concentration ratio (base:acid) is

  • 1/4
  • 1
  • 1:1
  • 4

  • 19. 
    What is the purpose of a titration?

  • To find the pH of an acid
  • To find the concentration of an unknown acid or base
  • To find the volume of an unknown acid or base
  • To find the pH of a base

  • 20. 
    Which acid base pair produce the titration curve shown below?

  • HCI + KOH
  • HCI + NH3
  • CH3COOH + KOH
  • CH3COOH + NH3

  • 21. 
    Which of the following would be the strongest acid

  • NaOH
  • HF
  • H2SO4
  • Ca(OH)2

  • 22. 
    What is the main purpose of acid-base titrations?

  • To test if reactants react.
  • To calculate the concentration of unknown analyte.
  • To calculate the concentration of known analyte.
  • To test quality of reactants.

  • 23. 
    The equivalence point is the

  • theoretical halfway point of the reaction
  • empirically derived completion of the reaction using phenolphthalein
  • theoretical completion of the reaction
  • the actual measurement based on the presence of the indicator

  • 24. 
    Back titrations are used when

  • the direct titration would be tediously slow
  • the analyte is completely insoluble
  • the end point cannot be visualized with any chemical indicators
  • a front titration just won't do

  • 25. 
    What is the impact of not transferring all of the KHP from your weigh boat to the Erlenmeyer in Part A?

  • lower volume of KHP needed
  • lower volume of base needed
  • concentration of base will be underestimated
  • no impact at all

  • 26. 
    Volumetric analysis can be defined as_____________

  • The determination of the identity of the solution
  • The determination of the mole of a mixture with a known solution
  • The determination of the concentration of a solution using a solution of known concentration

  • 27. 
    What is the purpose of indicator solutions?

  • To signal the end of a reaction
  • To colour the solution
  • To complete the reaction
  • To equivalent the reaction

  • 28. 
    The name of the apparatus used for holding the titrant is__________

  • Conical flask
  • Burette
  • Pipette
  • Volumetric flask
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