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# Lab Report Determining The Relative Molecular Mass of Amidosulphuric Acid

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Introduction

ï»¿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.

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