Asked by John

Hey guys, i have a question about how to figure out how much mass of a compound i need to find 130ppm here is the question.

What mass of Fe(NH4)2(SO4)2*6H2O is required to prepare 2.25 L of a 130 ppm iron solution?

Now i know that ppm is (mg of desired compoun)/(kg of solvent used) But in this case im not quite sure what the solvent would be?

Would the solvent be the previously explained Fe..... compound just minus the Fe? or would the compound just bethe 6H2O? im confused, if anyone could help that would be great.
Answered by DrBob222
Isn't that definition of yours 1 ppm = mg desired compound/kg SOLUTION. USUALLY when a solvent is not specified it is understood to be H2O. And I remember for solutions that 1 ppm = 1 mg/L.
So 130 ppm = 130 mg/L solution or
130*2.25 = about (estimate) 292 mg of Fe. To convert that to what must be weighed to obtain that 292, just convert by
292 estimate x (molar mass Fe(NH4)2(SO4)2.6H2O/atomic mass Fe) = ?
Answered by John
Oh okay, I understand. Wow thanks alot.
There are no AI answers yet. The ability to request AI answers is coming soon!