Titration Review

Burette readings should be recorded ___________.

• to 2 d.p.

• to the nearest 0.01 mL

• to 4 s.f.

• to the nearest 0.05 mL

The purpose of using an indicator in a titration is to determine the _________.

• equivalence point

• end point

• pH at neutralisation

• final burette reading

The following header(s) must be present in a table when recording titration results:

• Initial burette reading (mL)

• Final burette reading (mL)

• Titration number

• Volume of titrant used (mL)

How will rinsing the burette with analyte affect the titration result?

• Titre volume will increase.

• Titre volume will decrease.

• Titre volume will remain the same.

• Titre volume will either increase or decrease.

For titration results to be deemed accurate, they will need to be __________.

• within 0.20 cm³ of the teacher's reading

• within 0.10 cm³ of the teacher's reading

• repeatable

• exactly the same for at least two titrations

Which of the following actions could lead to inaccurate titration results?

• Swirling the conical flask during titration.

• Reading the burette at eye level.

• Rinsing the conical flask with analyte.

• Rinsing the burette with deionised water only.

25.0 cm³ of sulfuric acid is neutralised by 20.0 cm³ of 0.100 M NaOH. State the concentration of sulfuric acid.

• 0.160 M

• 0.0800 M

• 0.100 M

• 0.0400 M

Which of the following statements about the end point is/are true?

• The end point occurs at pH 7.

• The end point is the exact point at which the titrant and analyte have reacted in stoichiometrically equivalent quantities.

• The end point can only be determined using a pH meter.

• The end point occurs when the indicator changes colour permanently.

Why is it inappropriate to leave the funnel in the burette while performing a titration?

• It is a safety hazard.

• It may decrease the titre volume.

• It may increase the titre volume.

• It will interfere with the view of the meniscus.

A student titrates 25.0 cm³ of a sample of sulfuric acid with 1.00 mol/dm³ NaOH stock solution. 18.0 cm³ of NaOH is required to reach the end point. By performing necessary calculations, determine the volume of water that needs to be added to 25.0 cm³ of the sample to achieve a final concentration of 0.100 mol/dm³.

• 90.0 cm³

• 155 cm³

• 65.0 cm³

• 180 cm³