Investigating pH changes (Oxford AQA International A Level Chemistry)

Revision Note

Alexandra Brennan

Written by: Alexandra Brennan

Reviewed by: Stewart Hird

Required Practical 6: Investigating pH changes

Objective

To investigate how the pH of a solution of ethanoic acid changes as sodium hydroxide solution is added

Apparatus

  • two 50 cm3 burettes

  • two funnels

  • 100 cm3 beaker

  • deionised (or distilled) water in a wash bottle

  • stand and clamp

  • pH meter/probe

  • 0.100 mol dm–3 sodium hydroxide solution

  • 0.100 mol dm–3 ethanoic acid solution

  • standard pH buffer solutions at pH 4.00, 7.00 and 9.20

  • stirring rod

  • graph paper.

Method

Part 1: Calibrate the pH meter

  1. Rinse the pH probe thoroughly with deionised water, and shake it gently to remove excess water

  2. Place the probe in the standard pH 7.00 buffer solution provided, ensuring that the bulb is fully immersed

  3. Record the pH reading in a suitable table.

  4. Repeat this process using the standard pH 4.00 and 9.20 buffer solutions.

  5. Rinse the pH probe thoroughly with deionised water before taking each reading.

  6. Record the pH readings in your table.

  7. Plot a graph of your recorded pH reading (x-axis) against the pH of the buffer solution (y-axis).

Part 2: The measurement of the pH of the mixture of sodium hydroxide and ethanoic acid

  1. Use one burette to transfer exactly 20.0 cm3 of ethanoic acid to a clean 100 cm3 beaker

  2. Rinse and fill a second burette with NaOH solution

  3. Clamp the pH probe so that its bulb is fully immersed in the ethanoic acid solution in the beaker.

  4. Use a rod to stir the solution gently and record the pH reading in a suitable table

  5. Add 2.0 cm3 of the NaOH solution from the burette to the ethanoic acid. Stir the solution and record its pH

  6. Continue to add NaOH solution in 2.0 cm3 portions and record the pH until 18 cm3 has been added

  7. As the end point is reached, add NaOH solution in 0.20 cm3 portions until 22.0 cm3 is reached

  8. Then add the NaOH solution in 2.0 cm3 portions again until 40 cm3 have been added

How to set up your equipment

Investigate how pH changes when a weak acid reacts with a strong base

Practical Tip

  • You may need to wait a few seconds until the pH stabilises before you take a reading

  • Make sure the stirrer is not moving too fast as a rapid spin generates bubbles in the solution which gives an unsteady pH reading

Results

Record your results in a table like this:

Volume of sodium hydroxide (cm3)

pH

New pH

2.0

4.0

6.0

8.0

10.0

12.0

14.0

16.0

18.0

20.0

20.2

20.4

20.6

20.8

21.0

21.2

21.4

21.6

21.8

22.0

24.0

26.0

28.0

30.0

32.0

34.0

36.0

38.0

40.0

Evaluation

  1. Use the pH probe calibration graph you obtained from part 1 to adjust the pH readings obtained in the experiment

  2. Enter these pH values into a new column in the table of results

  3. Plot a graph of the corrected pH values (y-axis) against volume of sodium hydroxide solution added (x-axis)

  4. Join the points in the most appropriate way and comment on the shape of the curve

Worked Example

A student obtained the following pH curve from the reaction between sodium hydroxide and ethanoic acid.

Titration curve for strong base and weak acid
  1. What is meant by the equivalence point?

  2. Give the volume of base at the equivalence point

  3. Name a suitable indicator that could be used during a titration between these two chemicals.

Answer:

  1. The equivalence point is the point at which neutralisation occurs

  2. The volume of base at the equivalence point is 25 cm3

  3. A suitable indicator would be phenolphthalein because this changes colour at a pH close to the equivalence point

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Alexandra Brennan

Author: Alexandra Brennan

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.

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.