Objective: 1)To practice the procedure for preparing a standard solution 2)To perform the standardization of an unknown hydrochloric acid solution 3)To determine the given sodium hydroxide solution 4)To estimate the ethanoic acid content in commercial

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Course Code: 13554/Y1

Student Name: Chow Man Chung

             Lam Kwok Kei

             Lee Long Sing

             Chan Ka Chun

Date performed: 22nd September, 2010

Experiment 2: Acid base titration I

Objective:

  1. To practice the procedure for preparing a standard solution
  2. To perform the standardization of an unknown hydrochloric acid solution
  3. To determine the given sodium hydroxide solution
  4. To estimate the ethanoic acid content in commercial vinegar solution

Apparatus & equipments used:

  1. Burette, 50mL capacity
  2. Bulb pipette, 25mL capacity
  3. Volumetric flask, 250mL capacity
  4. Conical flask, 250mL capacity
  5. Analytical balance

Chemicals used:

  1. Anhydrous sodium carbonate
  2. Hydrochloric Acid, 0.1M
  3. Methyl orange indicator
  4. Phenolphthalein indicator
  5. Commercial vinegar solution

Results and Data Treatment:

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Weighting Data:

Mass of vial: 6.281g

Mass of vial and Na2CO3: 7.583g

Mass of Na2CO3: 1.302g

Na2CO3 solution made up to: 250.0cm3

Titration I: Standardization of 0.1M hydrochloric acid solution

Titrant (in burette): Hydrochloric acid

Titrate (in conical flask): 25.0cm3 of Na2CO3

Indicator used: Methyl Orange

Colour of indicator changed from: yellow to pink

Average volume: 23.18 cm3

Calculation:

Na2CO3 (s) + 2HCl → 2NaCl(s) + H2O(l) + CO2(g)

Number of mole of Na2CO3(aq) = 1.302g / 105.8089gmol-1

               = 0.0123

HCl : Na2CO3 = 2 : 1

Number of mole of HCl = ...

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