Q.1
What is an equivalence point?
  • It is the point when enough analyte has been added.
  • It is the point when the amount of added titrant is equal to the amount of analyte in the solution.
  • It is the point when the volume of titrant is equivalent the volume of analyte.
  • It is the point when the concentration of titrant added is equivalent to the volume of analyte.
Q.2
What is the role of an indicator in a reaction?
  • To help reactants react successfully.
  • To bind to the analyte to form a products.
  • To show when the reaction has reached or past the equivalence point.
  • To provide a surface for the reaction to occur.
Q.3
How will I ensure I get an accurate final end point?
  • Be slow and careful
  • Repeat until you have 3 very similar titre
  • Rinse the Burette
  • Always use the same Pipette filler
Q.4
What term describes the change in color of the indicator during a titration?
  • colorizing
  • endpoint
  • equivalence point
  • endgame
Q.5
A student used a 0.M of sodium hydroxide solution in a titration experiment. The initial reading on the buret was 0.mL. After the titration, the buret reading was 14.mL. How many moles of sodium hydroxide was used?
  • 1.82 moles
  • 1.82 x 10-3 moles
  • 8.34 x 10-3 moles
  • 8.6 moles
Q.6
HCl + NaOH →
  • NaH + ClOH
  • NaCl + H2
  • NaCl + H2O
  • NaCl + Cl2
Q.7
Acid + Base ₋-->
  • salt + hydrogen
  • salt + water
  • salt + carbon dioxide + water
  • salt
Q.8
In which of the following reactions does H2POact as an acid?
  • H3PO4 + H2O --> H3O+ + H2PO4-
  • H2PO4- + H2O --> H3O+ + HPO42-
  • H2PO4- + OH- --> H3PO4 + O2-
  • The ion cannot act as an acid
Q.9
I have 25mL ofHCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
  • 0.8 M
  • 1 M
  • 1.25 M
Q.10
What is the initial pH value when ethanoic acid was added into sodium hydroxide?
  • 13.0
  • 11.0
  • 3.5
  • 2.0
Q.11
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
Q.12
What is mean by equivalence point
  • a point which complete neutralisation occur where indicator change colour
  • a point which complete neutralisation occur where volume of H+ is equal to volume of OH-
  • a point where pH is equal to pKa
Q.13
Which of the following indicator is suitable for weak acid weak base titration
  • phenolphthalein
  • methyl orange
  • litmus
  • none above is suitable
Q.14
Identify the strongest acid
  • HCN
  • H2O
  • CH3OH
  • HNO3
Q.15
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
Q.16
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-
Q.17
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.
Q.18
Ascorbic acid, H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10–5 and K2 = 1.6 × 10–In a 0.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)
Q.19
How many mL of a 0.M NaOH solution are needed to neutralizemL of 0.M H3PO4 solution?3NaOH (aq) + H3PO4 (aq) ----> Na3PO4 (aq) + 3H(l)
  • 7.5 mL
  • 0.015 mL
  • 68 mL
  • 23 mL
Q.20
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.
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