- #1
Grove1996
- 15
- 0
Hey
I have a problem on my hands, I'm trying to find the concentration of ammonium phosphate in mol/L.
Equation:
Excuse the badly written equation, I'm not quite sure on how to use subscrips/arrow signs on here.
(NH4)3P04 --------------- 3NH4 + P04
Known Data:
Mass of 3NH4 measured with probe = 400 mg/L (0.40 g)
Mass of P04 measured with probe = 10 mg/L (0.01 g)
Moles of 3NH4 = 0.0678 moles
Moles of P04 = 0.00009915 moles
The problem:
I have found the mass of each of the products using a probe. The 3:1 ratio is not existent and this is due to a number of reasons (ignore this). How do I determine the mass of the original substance put in. Once I know that I can find the morality quite easily. I've attempted it but my high school teacher said I was wrong. I added the masses and now when I look back, it was a stupid thing to do. I think I need to use the solubility of ammonium phosphate some how, the solubility in water is 58g/100mL
Any help would be much appreciated, I really am stuck.
I have a problem on my hands, I'm trying to find the concentration of ammonium phosphate in mol/L.
Equation:
Excuse the badly written equation, I'm not quite sure on how to use subscrips/arrow signs on here.
(NH4)3P04 --------------- 3NH4 + P04
Known Data:
Mass of 3NH4 measured with probe = 400 mg/L (0.40 g)
Mass of P04 measured with probe = 10 mg/L (0.01 g)
Moles of 3NH4 = 0.0678 moles
Moles of P04 = 0.00009915 moles
The problem:
I have found the mass of each of the products using a probe. The 3:1 ratio is not existent and this is due to a number of reasons (ignore this). How do I determine the mass of the original substance put in. Once I know that I can find the morality quite easily. I've attempted it but my high school teacher said I was wrong. I added the masses and now when I look back, it was a stupid thing to do. I think I need to use the solubility of ammonium phosphate some how, the solubility in water is 58g/100mL
Any help would be much appreciated, I really am stuck.
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