A0.8965 g sample is dissolved in HNO; and filtered The alumimum is present in solution as AP. The solution is made basic with ammonium hydroxide, NH.OH, and the aluminum hydroxide, Al(OH): (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed The resulting alumina, Al:O: (FW 101.94), weighed 0.1605 g • Why is the solution filtered after acid dissolution? Why rinse with ammonium hydroxide solution? • What chemical transformation takes place during ignition? (Show the balanced chemical equation) • Why use a desiccator during cooling? Calculate the weight percent Al (AW 26.9815) in the sample.

A0.8965 g sample is dissolved in HNO; and filtered The alumimum is present in solution as AP. The solution is made basic with ammonium hydroxide, NH.OH, and the aluminum hydroxide, Al(OH): (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed The resulting alumina, Al:O: (FW 101.94), weighed 0.1605 g • Why is the solution filtered after acid dissolution? Why rinse with ammonium hydroxide solution? • What chemical transformation takes place during ignition? (Show the balanced chemical equation) • Why use a desiccator during cooling? Calculate the weight percent Al (AW 26.9815) in the sample.

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Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.195QP

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World production of chromite (FeCr₂O₄), the main ore ofchromium, was 1.5107metric tons in 2003. To isolate chro-mium, a mixture of chromite and sodium carbonate is heated inair to form sodium chromate, iron(III) oxide, and carbon diox-ide. The sodium chromate is dissolved in water, and this solutionis acidified with sulfuric acid to produce the less soluble sodiumdichromate. The sodium dichromate is filtered out and reduced with carbon to produce chromium(III) oxide, sodium carbonate,and carbon monoxide. The chromium(III) oxide is then reduced to chromium with aluminum metal. (a) Write balanced equations for each step. (b) What mass of chromium (in kg) could be pre-pared from the 2003 world production of chromite?
A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
The key reaction (unbalanced) in the manufacture of syn-thetic cryolite for aluminum electrolysis is HF(g)+ Al(OH)₃(s) +NaOH(aq) →Na₃AlF₆(aq) +H₂O(l) Assuming a 95.6% yield of dried, crystallized product, whatmass (in kg) of cryolite can be obtained from the reaction of 365 kg of Al(OH)₃, 1.20 m3of 50.0% by mass aqueous NaOH (d=1.53 g/mL), and 265 m³ of gaseous HF at 305 kPa and 91.5°C? (Assume that the ideal gas law holds.)
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgO
The purity of hydrazine, N2H4 is determined by titration with iodine. A sample of the oily liquid weighing 1.4286 is dissolved in water and diluted to 1.00L in volumetric flask. A solution of 50.00mL aliquot is taken with a pipet and titrated with a standard iodine solution, requiring 42.41 mL. The iodine was standardized against 0.4123g of primary standard As2O3, by dissolving As2O3 in a small amount of NaOH solution, adjusting the pH to 8.0, and titrating, requiring 40.28 mL iodine solution. Calculate the percentage purity of the hydrazine.
Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32
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In the alloy containing sn pb and cd, the mole ratio sn/pb is 2.73/1 and the mass ratio of pb/cd is 1.78/1, the percentage of cd by mass in the alloy
A 0.6599-g sample of impure magnesite, MgCO3 (MW = 84 g/mole), was decomposed with HCl; the liberated CO2 (MW = 44 g/mole) was collected on absorbent and found to weigh 0.1673-g. Calculate the percentage of magnesium (MW = 24 g/mole) in the sample. MgCO3 (s) + 2 HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O(l) Weight of pure magnesium in the sample is a. 0.1825 g b. 0.0913 g c. 0.3194 g d. 0.0456 g Percentage of magnesium carbonate in the sample is a. 24.20% b. 27.66% c. 48.40% d. 96.80%
A sample of pyrolusite weighing 0.6000 g is dissolved in a solution containing 5.00 mL of 6.00 N H2SO4 and 0.900 g of H2C2O4 .2H2O. The excess oxalate then requires 24.00 mL of KMnO4 solution for titration. If each mL of the KMnO4 will oxidize the Fe(II) in 0.03058 g FeSO4 .7H2O, what is the oxidizing power of the sample in terms of MnO2?

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