Need help on a lab results write-up. The lab is the synthesis and analysis of a transition metal complex. General reaction was stated as:
Fe(III) + x(acac) -> Fe(acac)x - we were to determine x by completing experiment. x = 1, 2, 3, 4...
acac = 2, 4 pentanedione
Procedure of experiment: dissolve 2 g of sodium acetate trihydrate in 25mL of water and add it to a solution of 1 g iron (III) chloride hexahydrate in 25 ml of water. Add 2mL of 2,4-pentanedione with stirring and continue to stir for 10 minutes. Filter red solid product and wash with cold water. Let filter paper dry until next class period. Weigh the solid obtained and determine % yield.
HOW DO I DO THIS? I've done the experiment. .967 grams of product was obtained, but how do I determine theoretical and % yield?
Next, we were suppose to analyze by following this procedure:
The overall idea here is to destroy the complex and reduce the freed Fe (III) to Fe (II) with iodide ions. The iodide becomes iodine which is easily quantified by a titration using thiosulfate ions as the titrant. Fe+3 + 2I -> 3Fe+2 + I2 and I2 + 2[S2O3]-2 -> 2I + S4O6.
Gently heat two carefully weighed 0.17 grams each of your complex in a flask with 5mL HCL and 2.5 mL HNO3 for about 20 minutes. Cool and add 40mL of water, 10mL 3M HCL and 0.5 g urea. Heat this new solution for 5 minutes at 60degrees celcius. Cool again and add 2 gram KI and a little sodium bicarbonate. Keep the flask covered until you titrate it with 0.20 M thiosulfate to a starch endpoint. Find the % iron in your complex by working back through your balanced reactions and compare it with the % iron expected if x = 1, 2, 3, 4 in the general complex formula. Decide which formula is correct. Draw the structure.
PLEASE HELP. Two titrations were performed. The first one used 1.69mL, and the second one used 1.65mL
To determine the theoretical yield and percent yield for the synthesis and analysis of the transition metal complex, you will need to follow these steps:
1. Theoretical Yield:
- Calculate the molar mass of the complex using the formula Fe(acac)x.
- Determine the mass of Fe(acac)x used in the reaction by multiplying the moles of Fe(acac)x with its molar mass.
- Use stoichiometry to find the molar ratio between Fe(acac)x and Fe(III) in the reaction (Fe(acac)x:Fe(III)).
- Convert the moles of Fe(III) to grams using its molar mass.
- Compare the moles of Fe(acac)x and Fe(III) based on the stoichiometric ratio to see which is the limiting reagent.
- The theoretical yield is the mass of the product that can be obtained based on the stoichiometric ratio of the limiting reagent.
2. Percent Yield:
- Divide the actual yield (0.967 grams) by the theoretical yield and multiply by 100 to obtain the percent yield.
To determine the percent iron in the complex, follow these steps for each titration:
1. Convert the volume of thiosulfate used in each titration to moles by multiplying with its molarity.
2. Use the stoichiometry of the reaction between thiosulfate ions and iodine to determine the moles of iodine produced in each titration (I2:2[S2O3]^2-).
3. Calculate the moles of iodine from the moles of thiosulfate used.
4. Determine the moles of Fe(III) reduced to Fe(II) based on the stoichiometry of the reaction between Fe(III) and iodide ions (Fe(III):2I-).
5. Calculate the percent iron in each titration by dividing the moles of Fe(III) by the moles of the complex used in the analysis (0.17 grams).
6. Compare the percent iron found in each titration with the expected percent iron based on the different possible values of x (1, 2, 3, 4) from the general complex formula (Fe(acac)x).
By comparing the experimental data with the expected values, you can determine which value of x in the general complex formula is correct.