A 0.800 g sample of impure potassium chloride (KCI) was dissolved in deionised water and was treated with a silver nitrate (AgNO3) solution in excess to give 1.460 g of silver chloride (AgCl) precipitates. Calculate the percentage of potassium chloride in the sample. An impure sample of Na3PO, weighing 0.1392 g is dissolved in 25 mL of water. A solution containing 50 mL of 3% w/v HgCl2, 20 mL of 10% w/v sodium acetate, and 5 mL of glacial acetic acid is then prepared. Adding the solution of Na3PO3 to the solution containing HgCl2, oxidizes PO to PO, precipitating HgCl. After digesting, filtering, and rinsing the precipitate, 0.4320 g of Hg:Cl is obtained. Report the purity of the original sample as % w/w Na3PO3. Na3PO3(aq) + 2HgCl(aq) + HO(1) HgCl(s) + NaPO(aq) + HCl(aq) To determine the amount of magnetite, Fe3O4, in an impure ore, a 1.5419-g sample is dissolved in concentrated HCL, giving a mixture of Fe+ and Fe+. After adding HNO; to oxidize Fe to Fe+ and diluting with water, Fe+ is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing, and igniting the precipitate provides 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample. Quinone, which is used in the dye industry and in photography, is an organic compound containing only C, H and O. In a combustion reaction, 0.105 g of the compound is completely burnt to give 0.257 g of CO2 and 0.0350 g of HO. a) Calculate the mass of oxygen in quinone. b) Find quinone's empirical formula. c) Deduce quinone's molecular formula if the molecular weight of quinone is approximately 108 g/mol.