Unknown Molarity Of HCL
Chemistry Assessment Practical and Report:
Introduction:
The experiment was conducted to find the unknown molarity of HCL. The unknown molarity of HCL was found by the use of the titration method and then comparing the results between the titrant and analyte HCL solutions. Molarity is a concentration unit, it is defined by the number of moles the total volume of the solution. This experiment included a process called titration, used to work out the unknown concentration of a known substance. The process of titration is adding titrant(known substance) from a burette, to a known quantity of analyte (unknown substance). The titration process was continued until the substance was neutralized, which was represented by the use of a universal …show more content…
The burette and pipette were then washed to ensure accurate results. Subsequently, HCL and NaOH were poured in the beakers by a professional to avoid injuries as HCL and NaOH are both highly concentrated solutions, any spills on the skin can cause severe burns. Once all the solutions were organised, the burette and pipette were set up. The burette was safely held using a boss head to avoid any spills. According to the ratios, five different solutions were poured into separate conical flask. The initial concentration was HCL:H2O (2:8) mL, it was commenced by measuring for the accurate volume. Respectively, the mixture of the HCL and H2O was poured in the conical flask where 3 drops of the indicator was added, which resulted in the solution turning pink, indicating the solution to be a acidic and a scale of ph 4. Then the flask containing the mixture of HCL+ H20 was placed under the burette containing NaOH. Then the titrant(NaOH) was steadily added to the analyte solution, drop by drop, to avoid excessive use of NaOH as it can result in a sudden change in ph. Whilst the titrant was being added, the flask was carefully shaken to ensure accurate results. Safety gloves were worn whilst shaking to avoid any spills on the skin. When the solution ph level reached 7 the stopcock was closed to stop the flowing of the titrant. Then the volume of …show more content…
The graph represents the quantity NaOH used in different concentrated solutions. Just as hypothesized the solution that is highly concentrated in HCL needs more NaOH(base) to neutralise. The titration method was used in this experiment as it is a common laboratory practice to find the quantitative chemical analysis that is used to determine the concentration of an identified analyte. This method plays a key role in chemical science as it is known to achieve accurate results. The volume of the NaOH used was recorded in units of mL to achieve best possible results. Before the experiment was commenced, all the apparatus were rinsed and wiped to avoid any contamination. The apparatus were also then examined to locate any faults. The cleaning procedure played a key part in this experiment as any faults or contamination would have resulted in inaccurate results. Despite of all the precaution, the experiment was not completely successful. The team was only successfully able to neutralise 3 solutions, this could be due to the lack of knowledge during the experiment. A white piece of sheet was not applied underneath the conical flask whilst waiting for the solution to neutralise. A white piece of sheet would have made the change of colour more visible to a naked eye. The errors could be minimised if proper research was done in
Introduction:
The experiment was conducted to find the unknown molarity of HCL. The unknown molarity of HCL was found by the use of the titration method and then comparing the results between the titrant and analyte HCL solutions. Molarity is a concentration unit, it is defined by the number of moles the total volume of the solution. This experiment included a process called titration, used to work out the unknown concentration of a known substance. The process of titration is adding titrant(known substance) from a burette, to a known quantity of analyte (unknown substance). The titration process was continued until the substance was neutralized, which was represented by the use of a universal …show more content…
The burette and pipette were then washed to ensure accurate results. Subsequently, HCL and NaOH were poured in the beakers by a professional to avoid injuries as HCL and NaOH are both highly concentrated solutions, any spills on the skin can cause severe burns. Once all the solutions were organised, the burette and pipette were set up. The burette was safely held using a boss head to avoid any spills. According to the ratios, five different solutions were poured into separate conical flask. The initial concentration was HCL:H2O (2:8) mL, it was commenced by measuring for the accurate volume. Respectively, the mixture of the HCL and H2O was poured in the conical flask where 3 drops of the indicator was added, which resulted in the solution turning pink, indicating the solution to be a acidic and a scale of ph 4. Then the flask containing the mixture of HCL+ H20 was placed under the burette containing NaOH. Then the titrant(NaOH) was steadily added to the analyte solution, drop by drop, to avoid excessive use of NaOH as it can result in a sudden change in ph. Whilst the titrant was being added, the flask was carefully shaken to ensure accurate results. Safety gloves were worn whilst shaking to avoid any spills on the skin. When the solution ph level reached 7 the stopcock was closed to stop the flowing of the titrant. Then the volume of …show more content…
The graph represents the quantity NaOH used in different concentrated solutions. Just as hypothesized the solution that is highly concentrated in HCL needs more NaOH(base) to neutralise. The titration method was used in this experiment as it is a common laboratory practice to find the quantitative chemical analysis that is used to determine the concentration of an identified analyte. This method plays a key role in chemical science as it is known to achieve accurate results. The volume of the NaOH used was recorded in units of mL to achieve best possible results. Before the experiment was commenced, all the apparatus were rinsed and wiped to avoid any contamination. The apparatus were also then examined to locate any faults. The cleaning procedure played a key part in this experiment as any faults or contamination would have resulted in inaccurate results. Despite of all the precaution, the experiment was not completely successful. The team was only successfully able to neutralise 3 solutions, this could be due to the lack of knowledge during the experiment. A white piece of sheet was not applied underneath the conical flask whilst waiting for the solution to neutralise. A white piece of sheet would have made the change of colour more visible to a naked eye. The errors could be minimised if proper research was done in