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 first calculate the mass of iron in the Fe2O3 product.
1 mole of Fe2O3 contains 2 moles of Fe.
The molar mass of Fe2O3 is 159.69 g/mol.
So, the mass of Fe in Fe2O3 is (2/159.69) x 0.3210 g = 0.004015 g.
Since Fe2O3 is the product of heating Fe(OH)3, we can assume that the mass of Fe in the Fe(OH)3 gel before ignition is the same as the mass of Fe in the Fe2O3 product.
Therefore, the weight percent of iron in the sample is (0.004015 g / 0.5962 g) x 100% = 0.6734%.