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Lab report on experiment number 2, Lab Reports of Chemistry

LaSalle CollegeChemistry

This is a lab report for experiment number 2

Typology: Lab Reports

2021/2022

Uploaded on 05/26/2022

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aaida-hossain 🇨🇦

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Dawson College
Department of Chemistry and Chemical Technology
Laboratory Report
Experiment # 01
Experiment Title: Volumetric Analysis of
an Acid Solution
Lab report done by: Aaida Hossain (2132500)
Partner: Mia Alyssa Nardelli
Presented to: Silja Makinen
202-NYA-05, Lab Section 14
Date of the Experiment: 27-10-2021
Date of the Lab Report Submission: 03-11-2021
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Dawson College

Department of Chemistry and Chemical Technology

Laboratory Report

Experiment # 01

Experiment Title: Volumetric Analysis of

an Acid Solution

Lab report done by: Aaida Hossain (2132500) Partner: Mia Alyssa Nardelli Presented to: Silja Makinen 202-NYA-05, Lab Section 14 Date of the Experiment: 27-10- Date of the Lab Report Submission: 03-11-

Procedure: Part A

  1. Calculate the mass of oxalic acid dihydrated needed to prepare 250 mL of 0.050 M solution.
  2. Weigh the amount of acid close to the mass calculated earlier.
  3. Transfer it into a clean 250-mL volumetric flask.
  4. Dissolve the acid in a small quantity of distilled water, then proceed to fill the bottle with distilled water to the mark.
  5. Shake the bottle.
  6. Rinse a clean burette with the NaOH solution of unknown concentration and discard the rinsate.
  7. Make sure that there is no air bubble at the tip of the burette.
  8. Clamp the burette.
  9. Read the level of NaOH in the burette to two decimal places. This will be your initial reading.
  10. Rinse a small clean beaker with a few milliliters of oxalic acid solution and discard the acid solution and discard the rinsate.
  11. Rinse a 10.00-mL pipette with a small amount of oxalic acid solution and discard the rinsate.
  12. Fill the pipette with the acid solution to the mark and transfer the acid aliquot into a clean 250-mL Erlenmeyer flask.
  13. Add water to the 50-mL mark and add five drops on phenolphthalein indicator.
  14. Shake well.
  15. Place the flask under the burette and start titrating very slowly while swirling the flask continuously.
  16. Once it is a light pink color, stop the titration and record the final reading of the burette.
  17. Repeat the titration process (steps 12–16) with two other 10.00-mL aliquots of the oxalic acid solution. Part B
  18. Rinse a small beaker.
  19. Fill the beaker with hydrochloric acid of unknown concentration.
  20. Rinse and fill a 10.00-mL pipette with the hydrochloric acid.
  21. Fill a burette with NaOH and note down the initial reading after clamping it
  22. Transfer the acid aliquot to a clean 250-mL Erlenmeyer flask.
  23. Add water to the 50-mL mark and add 5 drops of the phenolphthalein indicator.
  24. Shake well.
  25. Titrate with the NaOH solution used previously and repeat this process twice with 10.00- mL aliquots of the hydrochloric acid.

A. H 2 C 2 O 4 ( aq )+^2 NaOH ( aq ) →^ Na 2 C 2 O 4 ( aq )+^2 H 2 O ( l ) B. NaOH ( aq )+^ HCl ( aq ) →^ NaCl ( aq )+ H 2 O ( l ) Table 1 : Part A : Standardization of NaOH Mass of oxalic acid dihydrate, g 1. Number of moles of oxalic acid dihydrate, mol 0. Volume of the volumetric flask, mL 50. Concentration of oxalic acid dihydrate solution, (^) mol ∙ L −^1 0. Table 2 : Part A : Determination of the unknown concentration of NaOH Titration 1 Titration 2 Titration 3 Final burette reading, mL 0.10 11.10 21. Initial burette reading, mL 11.10 21.60 32. Volume of NaOH delivered, mL 11.00 10.50 10. Volume of oxalic acid used, mL 10.00 10.00 10. Moles of oxalic acid used, mol 0.004 0.004 0. Moles of NaOH, mol 0.008 0.008 0. Concentration of NaOH, (^) mol ∙ L −^1 0.73^ 0.76^ 0. Average concentration of NaOH, (^) mol ∙ L −^1 0. Table 3: Part B: Determination of the unknown concentration of an HCl Solution Titration 1 Titration 2 Titration 3 Final burette reading, mL 10.90 20.90 31. Initial burette reading, mL 20.90 31.00 41. Volume of NaOH delivered, mL 10.00 10.10 10. Moles of NaOH, mol 0.0075 0.0076 0. Moles of acid used, mol 0.0075 0.0076 0. Volume of acid consumed, mL 10.00 10.00 10. Concentration of the acid, (^) mol ∙ L −^1 0.75^ 0.76^ 0. Average concentration of the acid, (^) mol ∙ L −^1 0. Sample calculations: Number of moles: mass molar mass = moles Number of moles of oxalic acid dihydrate =¿

¿ ¿ Moles = Molarity ∗ Volume Moles of oxalic acid used =0. mol L ∗0.4 L =0.004 mol

Stoichiometry Moles of NaOH = 0.004 mol H 2 C 2 O 4 ( aq ) 1 mol H 2 C 2 O 4 ( aq ) ∗ x moles NaOH (^) ( aq ) 2 mol NaOH ( aq ) =0.008 mol Concentration: Concentration = moles volume Concentration of oxalic acid dihydrate solution = 0.02 mol 0.05 L =0.40 mol ∙ L − 1 Volume of the NaOH delivered: Final reading − Initial reading = Volume of NaOH dilivered Volume of NaOH delivered =11.10 mL −0.10 mL =11.00 mL Average concentration ( C (^) ¿¿ 1 + C 2 + C 3 ) 3 = Cavg ¿ Average concentration of NaOH =

mol L

mol L

mol L 3

mol L References:

  1. Department of Chemistry. (2018). Chemistry of Solutions: Laboratory experiments. Dawson College. Montreal, QC.