Acid-Alkali Titrations (Edexcel IGCSE Chemistry) : Revision Note

Stewart Hird

Written by: Stewart Hird

Reviewed by: Lucy Kirkham

Updated on

What is a titration?

  • Titrations are a method of analysing the concentration of solutions

  • Acid-base titrations are one of the most important kinds of titrations

  • They can determine exactly how much alkali is needed to neutralise a quantity of acid – and vice versa

  • You may be asked to calculate the moles present in a given amount, the concentration or volume required to neutralise an acid or a base

  • Titrations can also be used to prepare salts

How to carry out a titration

Titration, downloadable IB Chemistry revision notes
Titration apparatus, downloadable AS & A Level Chemistry revision notes

Performing a titration

Method

  1. Use the pipette and pipette filler and place exactly 25 cm3 sodium hydroxide solution into the conical flask

  2. Fill the burette with hydrochloric acid

    • Ensure an empty beaker is underneath the tap to catch in case the tap is accidentally open

  3. Run a small portion of hydrochloric acid through the burette to remove any air bubbles

    • The main air bubble is likely to be in the "jet space", which is the area between the tap and the tip of the burette

  4. Record the starting point on the burette to the nearest 0.05 cm3

    • You can add more hydrochloric acid so that the burette reading starts at 0.0 cm3

  5. Place the conical flask on a white tile

    • The purpose of the white tile is to make colour changes more obvious

  6. Add a few drops of a suitable indicator to the solution to the conical flask

  7. Ensure the tip of the burette is inside the conical flask

  8. Perform a rough titration by taking the burette reading and running in the solution in 1 – 3 cm3 portions

    • Remembe to swirl the flask vigorously

  9. Quickly close the tap when the end-point is reached

    • The end-point wil be indicated by a sharp colour change

  10. Record the final volume

    • Ensure you read off the meniscus at eye level

  11. Now repeat the titration with a fresh batch of sodium hydroxide

  12. As the rough end-point volume is approached, add the solution from the burette one drop at a time until the indicator just changes colour

  13. Record the volume to the nearest 0.05 cm3

  14. Repeat until you achieve two concordant results (two results that are within 0.1 cm3 of each other) to increase accuracy

Results

Results table for a titration

Rough titre (cm3)

Titre 1 (cm3)

Titre 2 (cm3)

Mean (cm3)

15.50

14.90

15.00

14.95

Examiner Tips and Tricks

Use a funnel to fill the burette but be sure to remove it before starting the practical as it can drip liquid into the burette, making the initial reading false.

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Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.

Lucy Kirkham

Reviewer: Lucy Kirkham

Expertise: Head of STEM

Lucy has been a passionate Maths teacher for over 12 years, teaching maths across the UK and abroad helping to engage, interest and develop confidence in the subject at all levels.Working as a Head of Department and then Director of Maths, Lucy has advised schools and academy trusts in both Scotland and the East Midlands, where her role was to support and coach teachers to improve Maths teaching for all.