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- 2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting solution was diluted with water, and the iron(III) was precipitated as hydrous oxide Fe,03 .XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,03 (FW = 159.69). Calculate (a) the percent Fe (FW = 55.847) and (b) the percent Fe;04 (FW = 231.54) in the sample.g. Aluminium in 1.200 g sample of impure ammonium aluminium sulphate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the percentage of aluminium in the sample (Atomic weight Al= 26.98 g mol-1; Molecular weight Al2O3 = 101.96 g mol-1).1. A 0.8040 g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated with 47.22 ml of 0.02242 M KMnO4 solution. Calculate the results of this analysis in terms of (a) %Fe (MW = 55.845) and (b) %Fe3O4 (MW = 231.535). Consider the reaction 5 Fe²+ + MnO4 + 8H+ → 5Fe3+ + Mn²+ + 4H₂O
- A mixture containing onlyl FeCl3 and AlCl3 weighs 5.95 g. The chlorides are converted to the hydrous oxides and ignited to Fe2O3 and Al2O3. The oxide mixture weighs 6.62 g. Calculate the % w/w Fe and % w/w Al in the original mixture.0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
- A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. Calculate the %w/w Ag in the alloy. (Mwt of Ag = 107.87 g/mol)The iron content of a large lump of ore is determined by taking a single small sample, dissolving it in acid, and titrating with ceric sulphate after reduction of Fe (III) to Fe (II). What are the possible source of random and systematic errors?Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and twice that molar concentration of thiosulfate ions at equilibrium? The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. Your answer should have 2 sig figs.
- Hardness in groundwater is due to the presence of metal ions, primarily Mg2+and Ca2+. Hardness is generally reported asppm (mg/L) CaCO3or mmol/L Ca2+. To measure water hardness, a sample of groundwater is titrated with EDTA, a chelating agent, in the presence of the indicator eriochrome black T, symbolized here as In. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2+and turns blue when Ca2+is removed. A 50.00-mL sample of groundwater is titrated with 0.0850M EDTA. Assume that Ca2+accounts for all of the hardness in the groundwater. If 10.10 mL of EDTA is required to titrate the 50.00-mL sample, what is the hardness of the groundwater in molarity Ca2+and in ppm CaCO3?Compare statement A with B. Indicate whether Statement A is (Greater than, Less than, Equal, or Cannot be Compared) with Statement B Statement A: Analyzed for Fe % w/w Fe. Statement B: Analyzed for Fe % w/w FeOA 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. What is the %w/w Ag in the alloy?