With the completion of the determinations of % potassium, %iron, and % oxalate in the crystals, you may calculate the % water.The percentage compositionof the crystals,KxFe(C2O4)y ·zH2O, has then been completely determinedexperimentally. The simplest formula (x,y,z) can now be calculatedfrom the the percentage composition. Once the formula is know it isthen possible to calculate the percent yield of product that wasobtained in the preparation and purification of the crystals.
From Part A:
Mass of KxFe(C2O4)y· zH2O prepared : 4.800 g
Mass of FeCl3 : 1.60 g
From Part B:
% Potassium in compound : 18.97 %
% Iron (from ion exchange & titration vs. NaOH) : 10.95 %
From Part C:
% Oxlate : 43.50 %
The questions below are part of the final analysis
Calculate the % water of hydration : 26.58
Calculate the following for Fe3+:
| g in 100 g sample | mol in 100 g sample | mol/mol Fe
(3 sig figs) | mol/mol Fe
(whole number) |
| | | |
Calculate the following for K+:
| g in 100 g sample | mol in 100 g sample | mol/mol Fe
(3 sig figs) | mol/mol Fe
(whole number) |
| | | |
Calculate the following forC2O42-:
| g in 100 g sample | mol in 100 g sample | mol/mol Fe
(3 sig figs) | mol/mol Fe
(whole number) |
| | | |
Calculate the following for H2O
| g in 100 g sample | mol in 100 g sample | mol/mol Fe
(3 sig figs) | mol/mol Fe
(whole number) |
| | | |
Enter the simplest formula of the Iron Oxalate Complex Salt:
Now that the formula of the complex salt is known, thepercent yield can be determined.
Calculate the moles of FeCl3 used in preparation:
Calculate the theoretical moles ofKxFe(C2O4)y ·zH2O:
Calculate the actual moles ofKxFe(C2O4)y ·zH2O synthesized:
Calculate the percent yield:
