A 0.5962g sample of iron ore is dissolved in percloric acid (h2lo4). All the iron present is oxidize to fe3+ the solution is filtered to remove solid matrix material and make basic with addition of ammonium hydroxide. the iron ppt as fe(oh)3.xh20 gel. the ppt is collected in a cistern crucible was ignited to produce fe2o3 what is the wt % of the iron in the sample if the analysis produce 0.3210g of fe2o3.

Answer 1

To find the weight percent of iron in the sample, we need to calculate the amount of iron in the Fe2O3 product.

1) Calculate the molar mass of Fe2O3:
Molar mass of Fe = 55.845 g/mol
Molar mass of O = 15.999 g/mol
Molar mass of Fe2O3 = (2 * 55.845) + (3 * 15.999) = 159.69 g/mol

2) Convert the weight of Fe2O3 product (0.3210 g) to moles:
Moles of Fe2O3 = (0.3210 g) / (159.69 g/mol) = 0.002012 mol

3) Since Fe2O3 is produced from Fe3+, the moles of Fe3+ in the original sample is also 0.002012 mol.

4) The molar mass of Fe3+ is 55.845 g/mol. Therefore, the weight of Fe3+ in the sample is:
Weight of Fe3+ = (0.002012 mol) * (55.845 g/mol) = 0.1123 g

5) The weight percent of iron in the sample is:
Weight percent of iron = (0.1123 g) / (0.5962 g) * 100 = 18.84%

Therefore, the weight percent of iron in the sample is approximately 18.84%.