You weigh out 196.07mg ferrous ammounium sulfate (FW 392.14) to prepare 250mL of solution which is 0.002M with respect to that compound.
The salt is quantitatively transferred into a 250mL volumetric flask and 8mL of 3M H2SO4 is added and then diluted to the mark (call this stock Fe solution).
So this 250 ml solution is
784.28 mg L^-1 (as FAS hydrate)
112 mg L^-1 as Fe
10mL of the stock solution is pipeted into a 100mL volumetric flask, adding 4mL of 3M H2SO4 and diluted to the mark (call this original Fe solution)
Here we have dilutes by a factor of 10
So this 100 ml solution is
78.428 mg L^-1 (as FAS hydrate)
11.2 mg L^-1 as Fe
10mL of the original fe solution is pipeted into a 50mL volumetric flask (call this standard Fe solution).
I presume this is made to the mark? In which case there is a further dilution by a factor of 5.
15.69 mg L^-1 (as FAS hydrate)
2.24 mg L^-1 as Fe
So perhaps the question is looking for the Fe concentration in mg L^-1?
(You should check my figures as I have rounded in places)
Um, exactly how did you calculate the 112 mg L^-1 as Fe, 11.2 mg L^-1 as Fe and 2.24 mg L^-1 as Fe ?
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