1. Practical 4 Experimental Procedure recall

2. Before experiment starts Rinse all apparatus with water and distilled water Burette, pipette, conical flasks, graduated flask, beaker, dropper, glass rod, filter funnel Wipe beaker (for weighing) dry Wipe exterior of pipette dry

3. Weighing TARE function may be used Place beaker in balance, close the doors, press TARE, wait for 0.000 to appear TAKE OUT beaker to add solid Place beaker back in balance, close the doors, wait for the mass to stabilise Repeat till mass obtained is what you need

4. Making standard solution Add abt 20 cm3 of distilled water to dissolve the crystals (a little more may be added if solid cannot dissolve) Place filter funnel on top of graduated flask Use glass rod to guide solution from beaker into graduated flask Glass rod should be placed back into the beaker

5. Making standard solution Rinse the walls of the beaker and the glass rod with distilled water Transfer these washings into the graduated flask Repeat above 2-3 times Rinse the sides of the filter funnel with distilled water Add distilled water until a finger below the mark

6. Making standard solution Remove filter funnel Use dropper to add distilled water drop by drop into the graduated flask till bottom of meniscus meets the line/mark Close the cap, shake the flask to ensure homogeneous solution obtained

7. Adding solution from graduated flask into conical flask Rinse the pipette with solution (Suck solution till about 2 fingers above the mark) Discard the solution Suck solution till slightly above the mark Hold pipette tip above solution Release solution using E button till the bottom of meniscus touch the mark

8. Wipe the exterior of pipette dry, avoid touching the tip of the pipette Release the solution into the conical flask When end, twist the pipette against the bottom of the conical flask (Do not try to get all the solution into the flask, as this vol of solution has been accounted for)

9. Adding NaOH into burette Place filter funnel on top of burette Add a small amount of NaOH Remove filter funnel Rinse the wall of the burette Rinse the burette tip by releasing the burette clip

10. Place filter funnel on top the burette Add NaOH into the burette Remove filter funnel Release burette clip and ensure burette tip is filled with solution No bubbles found in burette Read the initial volume

11. Practical 4 Precision of apparatus

13. Practical 4 Evaluation

14. 1 Comment on the consistency of your titre values. Identify and explain the presence or absence of anomalous results in these titre values.

15. Situation 1 There is no anomalous result as the results obtained are consistent to ±0.10 cm3 Two reasons why (Pg 40) Note : the results includes the rough titration, and the rough titration is cancelled

16. Situation 2 The 2 results chosen are consistent to ±0.10 cm3. Two reasons why Note : the results does not include the rough titration, and the rough titration is cancelled

17. 2 NaOH solid is not suitable for preparation of standard solution as it is deliquescent, explain how this will affect the concentration of the solution prepared and suggest ways to overcome it.

18. How it affect NaOH absorbs moisture from the air which will cause the mass measured to include the mass of water absorbed by NaOH solid. For the same mass weighed, a smaller amount of NaOH is obtained. The concentration of NaOH solution will be lower than expected.

19. Ways to overcome Weighing of the NaOH solid has to be carried out fast. Container used to store NaOH solid must be properly sealed to minimise contact with air.

20. 3 State one precaution that should be taken to ‘maintain’ the quality of the sodium hydroxide prepared.

21. Facts NaOH solution being basic can absorb CO2 from the air. Amount of NaOH present in the solution is lesser than expected. [NaOH] < expected

22. Precaution The NaOH solid weighed must be used immediately to prepare the solution. After the NaOH solution is prepared, ensure that it is always covered to minimise contact with air.

23. 4 Is there a more accurate way of determining the endpoint instead of the use of indicator?

24. Facts When colour changes from colourless (acid) to permanent pale pink (alkali), the equivalence point has been exceeded.Vol. of end point > Vol. of equivalence point The observation of colour change to detect endpoint of the titration can be subjective, and sometimes ambiguous.

25. More accurate way Use instrumental method Use pH meter to monitor the pH value of the solution, and plot a graph of pH against volume of titre Use data logger to plot the change in pH with the addition of solution form the burette. The endpoint correspond to the drastic change in pH during titration.

26. Practical 4 Explain the importance of the following steps:

27. i Ethanedioic acid crystals must be weighed accurately and the ethanedioic solution must be prepared in graduated flask.

28. i A more precise weighing balance will give a smaller percentage error in the mass of ethanedioic acid crystals weighed. A graduated flask measure volume with high accuracy, lower percentage error in the volume of the ethanedioic solution.

29. ii Use of pipette and burette to measure the volume of acid and NaOH respectively.

30. ii More precise apparatus is used to measure the volume of the solution decreases the percentage error of volume measured. Using a pipette to 1 dp, ensures that an accurate volume of 10 cm3 acid is obtained. An accurate amount of acid is present in the conical flask for titration. Using a burette to 2dp ensures that the volume of NaOH used is more accurately determined, and therefore a more accurate [NaoH]

31. iii Washings must be transferred into the graduated flask when the standard ethanedioic acid solution was being prepared.

32. iii Ensure all the ethanedioic acid that was not transferred into the graduated flask and present in the washings was transferred. This ensures that the amount of ethanedioic acid present in graduated flask = amount of ethanedioic acid weighed. It will give rise to an accurate volume of NaOH used and therefore, accurate [NaOH]

33. iv Use of indicator is necessary.

34. iv It is to provide a distinct colour change to determine the end point.

35. v Only 1-2 drops of indicator is required.

36. v Indicators are also weak acids/bases that can also take part in the titration Excessive use will cause significant reactions to occur with the indicators Titration values will be higher/lower than expected [NaOH] determined will be lower/higher than actual