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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_{x}Fe(C_{2}O_{4})_{y} · zH_{2}O, 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_{x}Fe(C_{2}O_{4})_{y} · zH_{2}O prepared : 4.800 g

Mass of FeCl_{3} : 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(C_{2}O_{4}) | · | H |

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

Calculate the moles of FeCl_{3} used in preparation:

Calculate the theoretical moles of K_{x}Fe(C_{2}O_{4})_{y} · zH_{2}O:

Calculate the actual moles of K_{x}Fe(C_{2}O_{4})_{y} · zH_{2}O synthesized:

Calculate the percent yield:

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