Discussion:
As the results show, both solutions had varying degrees of success in determining the two different anions and cations contained by solutions, respectively, Solution A(anion) and Solution 1(Cation). To fully understand these results, the General solubility rules must be used:
(see bibliography: ’Precipitation Rules’)
Interpretation / justification of the unknown cation solution tests ‘1’ results:
The unknown cation solution selected was ‘1’. Firstly this solution was tested for Pb2+using HCl. This was done because as the 3rd general solubility rule on the table provided states, all salts containing Chloride are soluble, with one of exceptions being if salt contains Pb2+. Thus if Pb2+exists in the solution, a precipitate …show more content…
The second anion within the solution, judging by the reliability of the results, is most likely Phosphate as its precipitation was clearly also detected within the 2nd procedure performed (albeit only very slightly) within both trials. Likewise, chloride could also be the second anion (while less likely) as it was also detected through its insoluble precipitation reaction with Ag+from silver nitrate (AgCl).
This means that sulfate (SO4 -2) is a definite anion within solution ‘A’. The second detected anion found would most likely be Phosphate (PO4 -3) due to its reliable recurrence within the results. Chloride (Cl -) still may also be an anion within the solution, as it produced more precipitate than phosphate, however due to its unreliability, this may just be an experimental error produced by unfiltered phosphate anions within the first trial.
Experimental sources of error within both tests:
Sources of Error
Why this is a source of experimental error
Improvements to be …show more content…
Whereby these light bands could have been then related to a table to find the two unknown ions in either test (with the exception of firstly testing for lead). Alternatively, an AES machine could have also been utilized, whereby the unknown ions would have been determined via accurate computing softwares.
Conclusion:
In conclusion to this experiment, the hypothesis has been met, being that a series of tests were performed to find differing anions / cations, while the aim has been met to various degrees.
In the case of solution ‘A’, it has been interpreted to contain Sulfate (SO4 -2), some phosphate(PO4 -3) and possibly also chloride (Cl -) anions. Likewise, Solution ‘1’ was also interpreted to contain Ba2+cations, while reliably detecting no others over two separate tests (which may have been due to how dilute the second or any additional cations may have been or become prior to or during the
As the results show, both solutions had varying degrees of success in determining the two different anions and cations contained by solutions, respectively, Solution A(anion) and Solution 1(Cation). To fully understand these results, the General solubility rules must be used:
(see bibliography: ’Precipitation Rules’)
Interpretation / justification of the unknown cation solution tests ‘1’ results:
The unknown cation solution selected was ‘1’. Firstly this solution was tested for Pb2+using HCl. This was done because as the 3rd general solubility rule on the table provided states, all salts containing Chloride are soluble, with one of exceptions being if salt contains Pb2+. Thus if Pb2+exists in the solution, a precipitate …show more content…
The second anion within the solution, judging by the reliability of the results, is most likely Phosphate as its precipitation was clearly also detected within the 2nd procedure performed (albeit only very slightly) within both trials. Likewise, chloride could also be the second anion (while less likely) as it was also detected through its insoluble precipitation reaction with Ag+from silver nitrate (AgCl).
This means that sulfate (SO4 -2) is a definite anion within solution ‘A’. The second detected anion found would most likely be Phosphate (PO4 -3) due to its reliable recurrence within the results. Chloride (Cl -) still may also be an anion within the solution, as it produced more precipitate than phosphate, however due to its unreliability, this may just be an experimental error produced by unfiltered phosphate anions within the first trial.
Experimental sources of error within both tests:
Sources of Error
Why this is a source of experimental error
Improvements to be …show more content…
Whereby these light bands could have been then related to a table to find the two unknown ions in either test (with the exception of firstly testing for lead). Alternatively, an AES machine could have also been utilized, whereby the unknown ions would have been determined via accurate computing softwares.
Conclusion:
In conclusion to this experiment, the hypothesis has been met, being that a series of tests were performed to find differing anions / cations, while the aim has been met to various degrees.
In the case of solution ‘A’, it has been interpreted to contain Sulfate (SO4 -2), some phosphate(PO4 -3) and possibly also chloride (Cl -) anions. Likewise, Solution ‘1’ was also interpreted to contain Ba2+cations, while reliably detecting no others over two separate tests (which may have been due to how dilute the second or any additional cations may have been or become prior to or during the