From Part A:
Mass of KxFe(C2O4)y· zH2O prepared : 5.100 g
Mass of FeCl3 : 1.60 g
From Part B:
% Potassium in compound : 17.95 %
% Iron (from ion exchange & titration vs. NaOH) : 8.35 %
From Part C:
% Oxlate : 43.97 %
Calculate the % water of hydration :
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) |
| | | |
Using your chemical knowledge and literature references (don’tforget to include the references in your lab report and discusspossible sources of errors) answer the questions below:
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:
