A 0.5962g sample of iron ore is dissolved in percloric acid (HCLO4). 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 iton ppt as FE(OH)3.xH2O gel. the ppt is collected in a cistern crucible was ignited to produce FE2SO3 what is the wt % of the iron in the sample if the analysis produce 0.3210g of FE2O3.
To calculate the weight percent of iron in the sample, we need to determine the amount of iron present in the sample and the total weight of the sample.
1. The weight of iron can be determined by converting the weight of Fe2O3 obtained in the analysis to Fe2SO3.
Fe2O3 + 3H2SO4 → Fe2(SO4)3 + 3H2O
From this balanced equation, we can see that the molar ratio of Fe2O3 to Fe2SO3 is 1:1. Therefore, the weight of Fe2SO3 is also 0.3210g.
2. The molar ratio of Fe2SO3 to Fe is 1:2. The molar mass of Fe2SO3 is 319.78 g/mol, and the molar mass of Fe is 55.85 g/mol.
Using dimensional analysis, we can calculate the weight of iron in the sample:
0.3210g Fe2SO3 * (2 mol Fe / 1 mol Fe2SO3) * (55.85 g Fe / 1 mol Fe) = 35.77 g Fe
3. The weight percent of iron in the sample is calculated by dividing the weight of iron by the weight of the sample and multiplying by 100.
(35.77 g Fe / 0.5962 g sample) * 100 = 6008.2%
Therefore, the weight percent of iron in the sample is approximately 6008.2%.