Synthesis of oxalate complexes, post lab question

1. The problem statement, all variables and given/known data

Okay I'm having trouble with my post lab question. This lab is on the synthesis of Iron(III) Oxalates. I have to figure out the theoretical yield, but i cant seem to even find a balanced equation. I've gone over this a million times but cant seem to figure it out.

here is the procedure
1. a) prepare 10 g of ferrous ammonium sulfate dissolved in 30mL of water containing 2 drops of 6M H2SO4 b) 6g of oxalic acid in 50 mL of water c) 6.6 g of K2C2O4H2O in 18 mL of water d) 1.7 g oxalic acid in 15 mL of water

2. carry out the following preparation in a 250 mL beaker. To the ferrous ammonium sufate solution add, with stirring, the solution of 6 g oxalic acid in water. A yellow precipitate of iron(II) oxalate forms quickly. Carefully heat the mixture to near boiling, stirring constantly to avoid bumping. Allow the precipitate to settle, decant and discard the supernatant liquid.

3. wash the precipitate three times by adding 30mL of hot water, stirring and decanting the liquid. Filtering is not necessary at this stage of the synthesis.

4. add the 6.6g potassium oxalate/18mL water solution to the wet iron (II) oxalate precipitate and heat the mixture to about 50 C. Slowly add 17ml of 6% H2O2 while stirring and maintaining a temperature of about 50 C for at least 15 mins or until al the unconverted iron (II) oxalate is converted.

5. heat the mixture to boiling and slowly add the 1.7g oxalic acid in 15mL water solution ; maintain the temperature near boiling for 10 mins. filter away any precipitate before adding ethanol. Add 20 mL 95% ethanol t the filtrate. cover the beaker with a watchglass, wrap in aluminum foil and place the beaker in your locker until next week.

6.after 1 week, filter the green product crystals with a buchner funnel, and wash twice with a few mL of 50% aqueous ethanol, then with a few mL of 95% ethanol. Continue to aspirate the crystals on the filter for 30 mins. to air dry your samples. Cover with aluminum foil during drying to prevent photocomposition. when dry, isolate and weigh your sample to determine the % yield.

2. Relevant equations

%yield=actual yield/theoretical yeild *100 for actual yield i got 2.835g

3. The attempt at a solution

I'm not sure do I start out with 10g of ferrous ammonium sulfate and convert to moles to find theoretical so confused
1. The problem statement, all variables and given/known data

2. Relevant equations

3. The attempt at a solution
1. The problem statement, all variables and given/known data

2. Relevant equations

3. The attempt at a solution


What is formula of the complex you were preparing?

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