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.
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%.