Question

With the completion of the determinations of % potassium, % iron, and % oxalate in the crystals, you may calculate the % water. The percentage compositionof the crystals, K_xFe(C₂O₄)_y · zH₂O, has then been completely determined experimentally. The simplest formula (x,y,z) can now be calculated from the the percentage composition. Once the formula is know it is then possible to calculate the percent yield of product that was obtained in the preparation and purification of the crystals.

From Part A:

Mass of K_xFe(C₂O₄)_y · zH₂O prepared : 4.800 g
Mass of FeCl₃ : 1.60 g

From Part B:

% Potassium in compound : 19.43 %
% Iron (from ion exchange & titration vs. NaOH) : 10.95 %

From Part C:

% Oxlate : 43.45 %

Enter the simplest formula of the Iron Oxalate Complex Salt:

K

Fe(C2O4)

·

H2O

Now that the formula of the complex salt is known, the percent yield can be determined.

Calculate the moles of FeCl₃ used in preparation:
Calculate the theoretical moles of K_xFe(C₂O₄)_y · zH₂O:

Calculate the actual moles of K_xFe(C₂O₄)_y · zH₂O synthesized:

Calculate the percent yield:

Answer 1

Mass of complex salt prepared = 4.800 g

Mass of FeCl3 = 1.60 g

% of water = 100- (19.43+10.95+43.45) = 26.17 %

Determination of simple formulae of complex salt and the resulting calculations are given below

Moles of hecla used = mass = 1.60 = 0.00996 . molar mass 162.2 reclz: Kz de CC209) 07H2O =1:1 moles of Kate (C204) .if H2O = 0.00986 moks. Theoretical moles of Kore (C209) .7H2O=0.00986 Theoretical, yeild = 0.009866 5 63.15= 5.5529 Actual moles of kzte (C204) .7H2O synthesized - Glass molas mass 563.16 = 0.00850 percentage yeild - Actual moles x Theoretical moles X100 0.00852 x 100 0.00986 86.40% OR Actual peild. Percentage yeild = Theoretical yeild 1 etical yeild x 100 = 408 x 100 5.552 86.4 %