Chemical Technology - Standard Titration - Report Writing Chemistry Assignment Help

Assignment Task:

Task 1 

A standard titration has been performed in order to determine the concentration of an unknown. Read the information given below, then use this data as though you had collected it yourself during a lab session. 

The titration was performed to determine the concentration of a solution of H2SO4. 3.957 g of NaHCO3 were first measured on a mass balance. The uncertainty present in this reading, as stated on the mass balance is ±0.01 g. The solid was then transferred completely into a 250.0 cm3 volumetric flask, performing washing steps as appropriate. The uncertainty stated on the volumetric flask is ±0.1 cm3. The volumetric flask was then filled correctly. Next, 25.00 cm3 of the solution in the volumetric flask were collected using a volumetric pipette and transferred completely into a clean conical flask. The uncertainty stated on the volumetric pipette is ±0.05 cm3. The H2SO4 solution of unknown concentration was placed in a burette. The uncertainty estimate in the burette is stated as ±0.1 cm3. A titration was then performed after adding a few drops of an appropriate indicator into the solution in the conical flask. The initial reading on the burette was 12.3 cm3 and the final reading at the end-point was 21.3 cm3. 

1. Calculate the number of moles of NaHCO3 measured and determine the total uncertainty present in this value. (A&A 4.2 – 2 marks) 

2. Calculate the concentration of the NaHCO3 solution in the volumetric flask in mol/dm3 and determine the total uncertainty present in this concentration. (A&A 4.2 – 2 marks) 

3. Calculate the number of moles of NaHCO3 present in the conical flask, and determine the total uncertainty present in this value. (A&A 4.2 – 2 marks) 

4. Calculate the titre value for this titration and determine the total uncertainty present in this value. (A&A 4.2 – 1 mark, S&E 4.1 – 1 mark) 

5. Calculate the concentration of the H2SO4 solution and determine the total uncertainty present in this value. (S&E 4.1 – 4 marks) 

6. The actual (real) concentration of the unknown was 0.275 mol/dm3. The discrepancy between this value and the value obtained in the titration can be caused by a number of reasons.

a) Explain the terms random error and systematic error. (S&E 4.1 – 1 mark)

b) Suggest two reasonable sources of systematic error which might have given rise to the difference observed between the measured and actual concentrations. (S&E 4.1 – 2 marks)

c) Suggest two improvements which could be implemented to reduce the effects of the random sources of error present in this titration. (S&E 4.1 – 2 marks) 

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