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

Lab Report Determining The Relative Molecular Mass of Amidosulphuric Acid

Extracts from this document...

Introduction

Name : Muhd. Naqiyuddin Bin Misran Class : M11K Date : 22nd August 2011 Title : Determining The Relative Molecular Mass of Amidosulphuric Acid Qualitative Data Reading of Burette(±0.05cm³) Initial Reading(±0.05cm³) Final Reading(±0.05cm³) Volume of sodium hydroxide used(±0.10cm³) 1st titration 0.90 26.10 25.20 2nd titration 15.00 40.10 25.10 3rd titration 18.30 43.40 25.00 Molarity of sodium hydroxide used : 0.096 M Mass of amidosulphuric acid : 2.5001 g Uncertainties of instruments Pipette : ±0.03 cm³ Burette : ±0.05 cm³ Volumetric flask : ±0.25cm³ Electronic Balance : ±0.0001g Qualitative Data 1. No colour change for amidosulphuric acid when phenophthaelin is added into it. 1. Colour of amidosulphuric acid changes from colourless into light pink when titrated with sodium hydroxide until it reaches the end point. DATA PROCESSING Percentage of Uncertainties Mass of amidosulphuric acid 0.0001 x 100% = 0.004% 2.5001 Amidosulphuric acid in volumetric flask 0.25 x 100% = 0.1 % 250.00 ...read more.

Middle

Number of mole of Amidosulphuric acid in volume of 250 cm³ The mole 0.0024± 0.4% mole of amidosulphuric acid is in the volume of 25.0 cm³ ± 0.12% after measured using pipette. The actual mole of amidosulphuric acid is in the volume of 250 cm³ ± 0.1% after its preparation in volumetric flask. Mole : 0.0024 mol x 10 = 0.024 mol Percentage of uncertainty :0.4% + 0.1% = 0.5% Therefore,the number of mole of amidosulphuric acid in 250 cm³ is 0.024 mole ± 0.50%. Determining relative Molecular Mass of amidosulphuric acid Mole = Mass RMM 0.024 mol = 2.5001 RMM RMM = 2.5001 0.024 = 104.17 Percentage of uncertainties = 0.5% + 0.004% = 0.504% Therefore, the RMM for amidosulphuric acid is 104.3 ± 0.5040% Theoretical value for RMM of amidosulphuric acid H2NSO3H = 2(1.01)+14.01+32.06+3(16.00)+1.01 = 97.1 Percentage Error Percentage error = |Experiment value – theoretical value| x 100% Experiment value ...read more.

Conclusion

The water will eventually bring left acid along into the beaker. Secondly, during the dilution of solid amidosulphuric acid in distilled water in beaker. During the mixing using glass rod, there are possibilities that the acid did not dissolved completely in water. So, to overcome this, mix the acid harder in water to ensure complete dissolving of amidosulphuric acid in distilled water. Lastly, when the titration reached its end-point , students facing problems to actually defined what is light pink. They tend to confuse to differentiate which is pink and which is purple to ensure that the titration had reached the end point or wether they have overshoot the sodium hydroxide into amidosulphuric acid solution. So, to overcome this, a beaker with amidosulphulric acid solution that has been titrated until it reached the end point with sodium hydroxide and has colour of pink should be prepared as controlling variable and indicator for the students. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate 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 International Baccalaureate Chemistry essays

  1. Chemistry Lab Report - Determine the Relative Atomic Mass of Lithium

    With the results, I calculated the R.A.M of lithium. Data Collection & Processing Raw Data Experiment Initial Volume of water in measuring cylinder (cm3) (+/- 2.00) Amount of H2 produced (cm3)

  2. Ionic and Molecular Compounds Lab

    A red litmus paper will turn blue upon its contact with a base and stay red upon its contact with an acid or a neutral substance. Unknown compounds 2 and 10 may be molecular compounds because they were the only two unknowns that did not conduct electricity.

  1. im To determine the relative molecular mass of chloroacetic acid ClCH2COOH

    Number of moles of chloracetic acid in 100 cm3 chloroacetic acid solution 2.1* 10-3 moles of ClCH2COOH � 10.00 cm3 of ClCH2COOH x � 100.00 cm3 of ClCH2COOH Number of moles of ClCH2COOH in 100.00 cm3 solution = x = 2.1*10-3 * 100.00 = 2.1 * 10-2 mol 10.00 4.

  2. pKa. When constant successive portions of Sodium Hydroxide are added to Acetic Acid; how ...

    Since the products were neutralized solutions of common salts they can safely be disposed of down the sink. 12. The conical flask was then washed with distilled water and 20 cm3 of Acetic acid was then poured into it via the Mohr pipette.

  1. Change of Potential Difference in Voltaic Cells Lab Report

    Record your answer. Mass = number of moles molar mass Mass of copper sulfate pentahydrate = 1 249.71 = 249.71 g This mass is required to prepare 1L of 1M copper sulfate solution. For 50ml, divide it by 20 = 12.485g of CuSO4.5H2O 3.

  2. Measuring the fatty acid percentage of the reused sunflower oil after numerous times of ...

    Because of this, I chose free fatty acid percentage in frying oil as an extended essay subject and my aim in this experiment was to “prove the harmful effects 5 ASLAN Özge Cemre D129077 of reused vegetable oil in potato frying and to find out the consequences of aggregate in

  1. To determine the molecular mass of an unknown alkali metal carbonate, X2CO3.

    Therefore, the relative molecular mass of Na2CO3 = 107.05g/mol. Error Propagation: Total error = Total random error + Total systematic error. To calculate the total random error, the percentage uncertainty of the lowest reading on each instrument shall be added together. Percentage uncertainty = Apparatus Uncertainty in apparatus Lowest quantity measured Percentage uncertainty Pipette (25cm3)

  2. Chemistry Titration Acid Base Lab

    Through research it has been determined that phenolphthalein should have, in fact, been the best indicator of use. Phenolphthalein has a pH range between 8.0 to 9.8 which is an appropriate range for a weak acid strong base titration. This is because the equivalence point for this titration will take

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