Titration In School Swimming Pool Water
Silver Nitrate Titration
Introduction
This experiment was conducted to work out the concentration of the chloride ions in the school swimming pool water and to see if it fits in the required range of concentration of chloride ions in the swimming pool water. This was done by titrating a small sample of the school swimming pool water with silver nitrate, which would form a white precipitate of silver chloride.
The equation of this process is:
The end point of the titration (when all of the chloride ions have been precipitated) was determined by the formation of a red-brown precipitate of silver chromate, by the reaction between the remaining silver ions and the chromate ions, from the indicator potassium chromate.
The equation …show more content…
Therefore, n(Cl)=1.53x10-42.5x10-5 moles.
Concentration in moldm-3=
c(Cl)==6.12x10-31x10-3 moldm-3
Aspect 3:
The calculations above show that the school swimming pool water has a concentration of 6.12x10-31x10-3 moldm-3 of chloride ions.
Conclusion & Evaluation
Aspect 1:
The main objective of this titration experiment was to calculate the concentration of the chlorine ions in the school swimming pool water and to see if it fits in the required range, which was between 1ppm and 3ppm(cdc.gov, 2014)
1ppm=1mgdm-3=0.001gdm-3=0.001/35.45 moldm-3 3x10-5 moldm-3
3ppm=3mgdm-3=0.003gdm-3=0.003/35.45 moldm-3 9x10-5 moldm-3
The value that I’ve calculated was 6.12x10-31x10-3 moldm-3, which does not fit into the recommended range of the concentration of chloride ions in the swimming pool …show more content…
Aspect 2:
The results show that the school swimming pool water is not suitable for swimming, as it has a higher concentration of chloride ions than the recommended concentration. But, looking at the methods of the investigation, one can see that this investigation had numerous systematic errors and human errors.
The first error in the investigation was the human error of opening and closing the tab on the burette. This is an error, which could not be eliminated in the investigation unless the investigation was conducted using an electronic burette, which was not required for the investigation. Because of this error, we could have added more silver nitrate past the end point of the titration, resulting in the final concentration of chloride ions to be
Introduction
This experiment was conducted to work out the concentration of the chloride ions in the school swimming pool water and to see if it fits in the required range of concentration of chloride ions in the swimming pool water. This was done by titrating a small sample of the school swimming pool water with silver nitrate, which would form a white precipitate of silver chloride.
The equation of this process is:
The end point of the titration (when all of the chloride ions have been precipitated) was determined by the formation of a red-brown precipitate of silver chromate, by the reaction between the remaining silver ions and the chromate ions, from the indicator potassium chromate.
The equation …show more content…
Therefore, n(Cl)=1.53x10-42.5x10-5 moles.
Concentration in moldm-3=
c(Cl)==6.12x10-31x10-3 moldm-3
Aspect 3:
The calculations above show that the school swimming pool water has a concentration of 6.12x10-31x10-3 moldm-3 of chloride ions.
Conclusion & Evaluation
Aspect 1:
The main objective of this titration experiment was to calculate the concentration of the chlorine ions in the school swimming pool water and to see if it fits in the required range, which was between 1ppm and 3ppm(cdc.gov, 2014)
1ppm=1mgdm-3=0.001gdm-3=0.001/35.45 moldm-3 3x10-5 moldm-3
3ppm=3mgdm-3=0.003gdm-3=0.003/35.45 moldm-3 9x10-5 moldm-3
The value that I’ve calculated was 6.12x10-31x10-3 moldm-3, which does not fit into the recommended range of the concentration of chloride ions in the swimming pool …show more content…
Aspect 2:
The results show that the school swimming pool water is not suitable for swimming, as it has a higher concentration of chloride ions than the recommended concentration. But, looking at the methods of the investigation, one can see that this investigation had numerous systematic errors and human errors.
The first error in the investigation was the human error of opening and closing the tab on the burette. This is an error, which could not be eliminated in the investigation unless the investigation was conducted using an electronic burette, which was not required for the investigation. Because of this error, we could have added more silver nitrate past the end point of the titration, resulting in the final concentration of chloride ions to be