Required Practical 2:Carrying Out a Titration (T)

• What should you be able to describe by the end of the video?

  The procedure for carrying out a titration
• Why is titration considered a required practical for triple chemistry students?

  It is likely to appear on exams
• What type of reaction occurs between sulfuric acid and sodium hydroxide?

  A neutralization reaction
• How can you determine the concentration of sulfuric acid using titration?

  By knowing the volume of sodium hydroxide
• What is the first step in carrying out a titration?

  Transfer 25 cm³ of sodium hydroxide
• What type of flask is used to reduce the risk of splashing?

  A conical flask
• Why is it important to use a pipette filler?

  To ensure accurate liquid volume measurement
• What should you do instead of blowing liquid out of the pipette?

  Allow the liquid to drain out
• What indicator can be added to the alkali in the conical flask?

  Methyl orange
• Why do we place the conical flask on a white tile?

  To see the color change more clearly
• What color change indicates neutralization with methyl orange?

  From yellow to permanently red
• What should you do once you start to see a color change during titration?

  Add acid drop by drop
• Why is it important to swirl the solution during titration?

  To ensure proper mixing of acid and alkali
• How should you read the volume of acid added from the burette?

  At the bottom of the meniscus
• What is the correct reading of the burette in the example given?

  17.9 cm³
• How many times should you repeat the titration for accuracy?

  Several times until two readings match
• What should you do with the readings obtained from multiple titrations?

  Take a mean for a final volume
• What can you calculate once you know the volume and concentration of the alkali?

  The concentration of the acid
• Where can you find more questions on carrying out a titration?

  In the vision workbook
• What are the stages involved in carrying out a titration?

  1. Transfer 25 cm³ of sodium hydroxide to a conical flask.
  2. Add 5 drops of an indicator.
  3. Place the flask on a white tile.
  4. Fill a burette with sulfuric acid.
  5. Add acid to the alkali until neutral.
  6. Swirl the solution to mix.
  7. Read the volume of acid from the burette.
  8. Repeat until two readings are within 0.1 cm³.
  9. Calculate the concentration of the acid.