- #1
Grove1996
- 15
- 0
Problem:
I've been working on my assignment and the purpose of it is to determine the concentration of a contaminant present in a sample of water. I've discovered the contaminant is ammonium phosphate with the levels of each being 200% higher than normal water. I obtained these results using an ion-selective electrode and a colorimeter.
Probe Results:
Ammonium: 407.14 mg/L
Phosphate: 9.42 mg/L
I have to determine the amount of ammonium phosphate originally put into the sample of water, and its concentration (molarity). Usually I would do an "ICE" table but I don't know how much ammonium phosphate has originally been put in. I've done the stoichometry and determined that the 3:1 ratio between ammonium and phosphate does not exist (as the probe results suggest). Regardless, I have to determine the amount originally put in (preferably in grams) and the molarity of the solution.
I have no idea where to start, as I said before I would usually do an ICE table but that will not work in this case.
TLDR:
Probe readings show a total of approximately 407 mg/L of ammonium and 9.5 mg/L of phosphate. What process would I do in order to determine the original amount put in, and the molarity of the concentration.
Any help would be much appreciated.
I've been working on my assignment and the purpose of it is to determine the concentration of a contaminant present in a sample of water. I've discovered the contaminant is ammonium phosphate with the levels of each being 200% higher than normal water. I obtained these results using an ion-selective electrode and a colorimeter.
Probe Results:
Ammonium: 407.14 mg/L
Phosphate: 9.42 mg/L
I have to determine the amount of ammonium phosphate originally put into the sample of water, and its concentration (molarity). Usually I would do an "ICE" table but I don't know how much ammonium phosphate has originally been put in. I've done the stoichometry and determined that the 3:1 ratio between ammonium and phosphate does not exist (as the probe results suggest). Regardless, I have to determine the amount originally put in (preferably in grams) and the molarity of the solution.
I have no idea where to start, as I said before I would usually do an ICE table but that will not work in this case.
TLDR:
Probe readings show a total of approximately 407 mg/L of ammonium and 9.5 mg/L of phosphate. What process would I do in order to determine the original amount put in, and the molarity of the concentration.
Any help would be much appreciated.