Physic Lab Report on Amidosulphuric Acid

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Summary

The experiment aimed to determine the relative molecular mass of amidosulphuric acid through titration with sodium hydroxide solution. When diluted with distilled water, the solution remained clear and turned pale pink at the endpoint. The average volume of sodium hydroxide solution used was 27.2 cm3, and the calculated relative molecular mass was 92.20 g mol-1 with a total percentage error of 0.5516%. The experimental value was smaller than the theoretical value of 97.1 g mol-1, possibly due to systematic and random errors during the experiment, such as leftover powdered acid, parallax error, and overshot during titration.

Table of Content

Qualitative Data

  1. When amidosulphuric acid was diluted with distilled water, the beaker feels cold.
  2. When the phenolphthalein indicator was dropped into the solution, the solution color does not change and remains clear.
  3. When the diluted amidosulphuric acid was titrated with the sodium hydroxide solution, the color of the solution turns to pale pink and it is called an endpoint. Mass of amidosulphuric acid powder = 2. 5050 g ± 0. 0001 g

Calculation

The average volume of sodium hydroxide solution used =First reading+Second reading+Third reading

3 24. 7 + 29. 8 + 27. 0 3 = 27. 2 cm3 = 27. 2 cm3 ± 0. 1 cm3

Chemical equation: H3NSO3 + NaOH > NaH2NSO3 + H2O No of mole of sodium hydroxide, n=Molarity of solution?

Volume of solution 1000 = 0. 002720 mol 1 mole of NaOH reacts with 1 mole of H3NSO3 So, 0. 002720 mol of NaOH reacts with 0. 002720 mol of H3NSO3

Volume of solution = 0. 0109 mol dm-3

The relative molecular mass of 250. 00 cm3 amidosulphuric acid, RMM= Mass of compound

No of a mole of the compound 10 = 2. 50500. 002720 = 92. 20 g mol-1

Error Analysis

  1. Burette = 0. 127. 2? 100% = 0. 3676 %
  2. Pipette = 0. 0325. 00? 100% = ± 0. 1200 %
  3. Volumetric flask = 0. 15250. 00? 100% 0. 06000 %
  4. Analytical balance = 0. 00012. 5050? 100% = 0. 004000 %

Total percentage error = 0. 3676% + 0. 1200% + 0. 06000% + 0. 004000% = 0. 5516 %

Absolute error = ±0. 5086 g mol-1

Conclusion and Evaluation

From the experiment, the relative molecular mass of amidosulphuric acid obtain is 92. 20 g mol-1 ± 0. 5086 g mol-1. The total percentage error from the instrument is 0. 5516%. The experimental value obtain is smaller than the theoretical value of the acid which is 97. 1 g mol-1. This different is most likely from systematic errors and also random errors during the experiment. The errors are may come from

  1. There are some of the powdered amidosulphuric acids left at the weighing bottle.
  2. There is a parallax error when the observer taking the reading of sodium hydroxide solution in the burette.
  3. Overshot happen during the titration which affects the amount of sodium hydroxide used to neutralize the amidosulphuric acid.

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Physic Lab Report on Amidosulphuric Acid. (2016, Sep 18). Retrieved from

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