Investigating pH changes (Oxford AQA International A Level Chemistry)
Revision Note
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
Rinse the pH probe thoroughly with deionised water, and shake it gently to remove excess water
Place the probe in the standard pH 7.00 buffer solution provided, ensuring that the bulb is fully immersed
Record the pH reading in a suitable table.
Repeat this process using the standard pH 4.00 and 9.20 buffer solutions.
Rinse the pH probe thoroughly with deionised water before taking each reading.
Record the pH readings in your table.
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
Use one burette to transfer exactly 20.0 cm3 of ethanoic acid to a clean 100 cm3 beaker
Rinse and fill a second burette with NaOH solution
Clamp the pH probe so that its bulb is fully immersed in the ethanoic acid solution in the beaker.
Use a rod to stir the solution gently and record the pH reading in a suitable table
Add 2.0 cm3 of the NaOH solution from the burette to the ethanoic acid. Stir the solution and record its pH
Continue to add NaOH solution in 2.0 cm3 portions and record the pH until 18 cm3 has been added
As the end point is reached, add NaOH solution in 0.20 cm3 portions until 22.0 cm3 is reached
Then add the NaOH solution in 2.0 cm3 portions again until 40 cm3 have been added
How to set up your equipment
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
Use the pH probe calibration graph you obtained from part 1 to adjust the pH readings obtained in the experiment
Enter these pH values into a new column in the table of results
Plot a graph of the corrected pH values (y-axis) against volume of sodium hydroxide solution added (x-axis)
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.
What is meant by the equivalence point?
Give the volume of base at the equivalence point
Name a suitable indicator that could be used during a titration between these two chemicals.
Answer:
The equivalence point is the point at which neutralisation occurs
The volume of base at the equivalence point is 25 cm3
A suitable indicator would be phenolphthalein because this changes colour at a pH close to the equivalence point
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