ABSTRACT FOR TITRATION: This practical is on making and testing solutions using titration. Titration is a practical technique
used in determining the amount or concentration of a substance in a sample. The titration practical involves three parts,
part1 (making a standard solution and standardisation of an acid using an indicator), part2 (Titration of sodium
hydroxide with hydrochloric acid using a pH meter) and the part 3 titration practical was on (titration of sodium
hydroxide with hydrochloric acid using an indicator). In the part1 practical, before making the standard solution and
standardisation of the acid, all the volumetric equipment that was going to be used were first calibrated using distilled
water in other to ensure the results gotten from the equipment's were accurate. The percentage error for this practical
was an extremely low percentage error of 0%. For the part 2 practical, the pH meter that was used during the practical
was first calibrated with the buffer solutions that was provided in order to prevent having an inaccurate result during the
practical. The percentage error gotten for this practical was 20.4%. For the part3 practical, a methyl orange indicator
was used to titrate sodium hydroxide with hydrochloric acid. The percentage error for this practical was 6%.
ABSTRACT FOR COLORIMETRY: This practical is on making and testing solutions using colorimetry procedures. Colorimetry
is the technique that is used to determine the concentration of coloured compounds in solutions by the application of
the Beer- Lambert Law. Before carrying out the colorimetry practical, the weighing balance that was going to be used
was first calibrated in order to ensure that the readings from the weighing balance were accurate. For the colorimetry
practical, a calibration curve of absorbance was plotted against the concentration of copper (II) sulphate to determine
the concentration of the two unknown solutions (unknown 1 and unknown 2). A low percentage error of 7% was gotten
for the concentration of unknown 1 and a percentage error of 2% was gotten for the concentration of unknown solution
2.
,Initials
Introduction: Titration can be defined as the technique of using the solution of a known concentration to calculate the
concentration of an unknown concentration. Titration is a practical technique used in determining the amount or
concentration of a substance in a sample. The aim of this practical is to make and test standard solutions using titration
procedures by ensuring that equipment used during the practical were properly calibrated and all the chemicals used
were also safety checked.
Calibrating a balance of volumetric equipment
Method (Method used was provided by my centre)
• Place an empty, clean, and dry beaker unto a balance and record the mass.
• Measure 25cm3 of water using one of the volumetric equipment
• Transfer the water into the beaker and record the mass.
• Calculate the mass of the water added.
• Repeat for all volumetric equipment (beaker, pipette, burette and measuring cylinder)
Volumetric Mass Mass reading(g) Mass reading(g) Mass reading(g)
equipment reading(g)
2(g) 3(g) Average(g)
1(g)
Pipette 24.98 24.98 24.98 24.98
Burette 24.8 24.81 24.8 24.8
Measuring 24.86 24.73 24.8 24.8
Cylinder
1 | Page
,Initials
Beaker 23.84 23.84 23.85 23.84
Calibrating a balance of Known mass
Method (Method used was provided by my censor)
• Place a known mass on the balance and record the mass
• Repeat three times to ensure the results are accurate.
• Repeat again with another mass.
Known mass Mass reading(g) Mass reading(g) Mass reading(g) Mass
1(g) 2(g) 3(g) reading(g)
Average(g)
10g 9.89 9.89 9.89 9.89
50g 49.62 49.62 49.61 49.62
100g 95 95 97.15 95.72
2 | Page
, Initials
Part 1 – Making a standard solution and standardisation of an acid using an indicator
Equipment used in the practical
• Sodium Carbonate
• Distilled water
• Weighing balance
• Beaker
• Safety goggles
• Pipette
• Burette
• Measuring cylinder
Risk Assessment
Investigation Title: Preparation of a Standard Solution for Sodium Carbonate
Aim of investigation: Preparing a standard solution for Sodium Carbonate and finding its accurate mass
3 | Page
used in determining the amount or concentration of a substance in a sample. The titration practical involves three parts,
part1 (making a standard solution and standardisation of an acid using an indicator), part2 (Titration of sodium
hydroxide with hydrochloric acid using a pH meter) and the part 3 titration practical was on (titration of sodium
hydroxide with hydrochloric acid using an indicator). In the part1 practical, before making the standard solution and
standardisation of the acid, all the volumetric equipment that was going to be used were first calibrated using distilled
water in other to ensure the results gotten from the equipment's were accurate. The percentage error for this practical
was an extremely low percentage error of 0%. For the part 2 practical, the pH meter that was used during the practical
was first calibrated with the buffer solutions that was provided in order to prevent having an inaccurate result during the
practical. The percentage error gotten for this practical was 20.4%. For the part3 practical, a methyl orange indicator
was used to titrate sodium hydroxide with hydrochloric acid. The percentage error for this practical was 6%.
ABSTRACT FOR COLORIMETRY: This practical is on making and testing solutions using colorimetry procedures. Colorimetry
is the technique that is used to determine the concentration of coloured compounds in solutions by the application of
the Beer- Lambert Law. Before carrying out the colorimetry practical, the weighing balance that was going to be used
was first calibrated in order to ensure that the readings from the weighing balance were accurate. For the colorimetry
practical, a calibration curve of absorbance was plotted against the concentration of copper (II) sulphate to determine
the concentration of the two unknown solutions (unknown 1 and unknown 2). A low percentage error of 7% was gotten
for the concentration of unknown 1 and a percentage error of 2% was gotten for the concentration of unknown solution
2.
,Initials
Introduction: Titration can be defined as the technique of using the solution of a known concentration to calculate the
concentration of an unknown concentration. Titration is a practical technique used in determining the amount or
concentration of a substance in a sample. The aim of this practical is to make and test standard solutions using titration
procedures by ensuring that equipment used during the practical were properly calibrated and all the chemicals used
were also safety checked.
Calibrating a balance of volumetric equipment
Method (Method used was provided by my centre)
• Place an empty, clean, and dry beaker unto a balance and record the mass.
• Measure 25cm3 of water using one of the volumetric equipment
• Transfer the water into the beaker and record the mass.
• Calculate the mass of the water added.
• Repeat for all volumetric equipment (beaker, pipette, burette and measuring cylinder)
Volumetric Mass Mass reading(g) Mass reading(g) Mass reading(g)
equipment reading(g)
2(g) 3(g) Average(g)
1(g)
Pipette 24.98 24.98 24.98 24.98
Burette 24.8 24.81 24.8 24.8
Measuring 24.86 24.73 24.8 24.8
Cylinder
1 | Page
,Initials
Beaker 23.84 23.84 23.85 23.84
Calibrating a balance of Known mass
Method (Method used was provided by my censor)
• Place a known mass on the balance and record the mass
• Repeat three times to ensure the results are accurate.
• Repeat again with another mass.
Known mass Mass reading(g) Mass reading(g) Mass reading(g) Mass
1(g) 2(g) 3(g) reading(g)
Average(g)
10g 9.89 9.89 9.89 9.89
50g 49.62 49.62 49.61 49.62
100g 95 95 97.15 95.72
2 | Page
, Initials
Part 1 – Making a standard solution and standardisation of an acid using an indicator
Equipment used in the practical
• Sodium Carbonate
• Distilled water
• Weighing balance
• Beaker
• Safety goggles
• Pipette
• Burette
• Measuring cylinder
Risk Assessment
Investigation Title: Preparation of a Standard Solution for Sodium Carbonate
Aim of investigation: Preparing a standard solution for Sodium Carbonate and finding its accurate mass
3 | Page
