• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Titration lab report - determine the percentage of acetic acid present in vinegar

Extracts from this document...

Introduction

´╗┐LAB REPORT PERCENTAGE OF ACETIC ACID IN VINEGAR Experiment #20 OBJECTIVE: Propose of this experiment is to determine the percentage of acetic acid present in vinegar. PROCEDURE: 1. Carefully clean a 50 mL buret and rinse it with water and then 2 times with 5 mL portions of NaOH solution. 2. Fill the buret and open the pinch clamp to fill the tip. 3. If the exact concentration of the base is given, record the value and move on. If not, standardize the base solution with primary standard H2C2O4.2H2O (oxalic acid): 1. Weigh approximately 0.15 g (down to 0.0002 g) of oxalic acid in a 125 mL Erlenmeyer flask. 2. Dissolve the solid in about 25 mL of distilled water. ...read more.

Middle

7. Deliver the 5 mL aliquot into a 125 mL Erlenmeyer flask. Touch off the last drop on the inside wall. 8. Fill the buret with the standardized NaOH solution 9. Record the initial buret reading. 10. Add 2 drops of phenolphthalein indicator to the vinegar solution. 11. Titrate to a faint pink end point. 12. Record final buret reading. 13. Repeat the titration at least once more until the volume of NaOH solution used in 2 different titrations agrees within 0.2 mL. Chemical equations: H2C2O4.2H2O+2NaOH?Na2C2O4.2H2O+2H2O CH3COOH+NaOH?CH3COONa+H2O DATA and CALCULATION: Standardization of NaOH solution: Titration 1 Titration 2 Titration 3 Weight of Erlenmeyer flask + solid H2C2O4.2H2O (g) 79.2380 82.9368 81.0613 Weight of empty Erlenmeyer flask (g) ...read more.

Conclusion

5.155% 5.168% 5.168% CH3COOH+NaOH→CH3COONa+H2O (2) From the equation (2): mol of CH3COOH=mol of NaOH=VNaOH (used)×MNaOH (average) Mvinegar=mol of CH3COOHVvinegar % of CH3COOH in vinegar=mass of CH3COOHmass of vinegar×100%=mol of CH3COOH×molar mass of CH3COOHdensity of vineger×Vvineger×100%=mol of CH3COOH×60.052 g/mol1 g/mL×5mL×100%=mol of CH3COOH×12.0104 mol-1×100% Titration 1: mol of CH3COOH=mol of NaOH=42.00×10-3L×0.1022molL=4.292×10-3 mol Mvinegar=4.292×10-3 mol5×10-3L=0.8584 M % of CH3COOH in vinegar=4.292×10-3 mol×12.0104 mol-1×100%=5.155% Titration 2 and 3: mol of CH3COOH=mol of NaOH=42.10×10-3L×0.1022molL=4.303×10-3 mol Mvinegar=4.303×10-3 mol5×10-3L=0.8605 M % of CH3COOH in vinegar=4.303×10-3 mol×12.0104 mol-1×100%=5.168% CONCLUSION: We did the experiment to standardize the NaOH solution in order to get the exact concentration of NaOH solution to be 0.1022 M that agrees with the given concentration of NaOH solution, 0.1 M. We did the titrations successfully in order to get the percentages of acetic acid in vinegar to be approximately to be 5.2%. The value is acceptable for the table vinegar that was given in the lab. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Physical Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related AS and A Level Physical Chemistry essays

  1. Peer reviewed

    Titration Lab Report

    4 star(s)

    Compare your answers to Questions 1 and 3. By examining a titration curve, how can you decide which acid-base indicator to use to find the equivalence point? After examining S Titration Curves, it is observed that color change is visible around the equivalence point, which can either be seen above or below the point of color change.

  2. Determination of the content of Mg (OH)2 in an indigestion remedy by back titration ...

    Mg (OH)2 + NaHCO3 + 3HCl --> NaCl + MgCl2 + 3H2O + CO2 As 3 moles of HCl would have being neutralised instead of 2 moles in the mixture, as calculated earlier there is less excess acid available for the back titration.

  1. Acid-Base Titrations.

    To select a proper indicator, then, requires determination of the pH of the solution at the equivalence point of the titration and selection of an indicator whose pKa is as close to that pH as possible. Indicators are usually organic structures of some complexity or natural products and, like dyeing

  2. Drug: Antacid Effectiveness Analysis To determine the neutralizing ability of antacids in different ...

    Use eye protection at all times and immediately wash spills from your skin and clothing. 6. The burette must be rinsed out with NaOH before use to prevent dilution of the solution.

  1. Determination of the Percentage of Oxalate in Iron(II) Oxalate by Redox Titration

    So, no. of moles of FeC2O4 .2H2O in every 25cm3= 5.473 X 10-4 /3 X 5 = 9.122 X10-4 moles There are also 9.122 X 10-4 moles of oxalate in every 25cm3.

  2. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    CONCLUSION 2: (Equation 3.5.2) Table 3.5.3 shows the values of average time (t) and when the concentration of the acid solution was varied (all results to two decimal places): [H+] /10-3 mol dm-3 Average time (t) /s /10-3 s-1 5.00 138.33 7.23 4.00 197.67 5.06 3.00 320.00 3.13 2.00 723.67 1.38 1.00 3136.33 0.32 0.00 - 0.00 (Table 3.5.3)

  1. Investigating how concentration affects rate of reaction

    This also meant that it was not included when further investigating the order of reaction for sulphuric acid. The fact that I still found that the order of reaction, respect to sulphuric acid, was two means that my results were still accurate even when excluding this anomaly.

  2. Activity Series of Metals Lab

    Any tests that were proven false against the hypothesis may just be the experimental errors that occur and the setting of which the experiment was performed in. For example the time the experiment was observed for was not long enough to notice change for some of the tests and oxidization occurred to cause an unwanted reaction with the lone metals.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work