1 answer

With the completion of the determinations of % potassium, % iron, and % oxalate in the...

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, KxFe(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 KxFe(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 KxFe(C2O4)y · zH2O:

Calculate the actual moles of KxFe(C2O4)y · zH2O synthesized:

Calculate the percent yield:


Answers

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 =

.

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