In 'Synthesis of an Iron Complex Salt', hydrogen peroxide (H202) is added to the solution and heat is applied until boiling. A side reaction is the formation of rust brown precipitate, which consists of potassium permanganate (KMN04) ferrous ammonium sulfate, Fe(NH4)2(SO4)2:6H20] iron (III) hydroxide, Fe(OH)3 Iron (II) oxalate (FeC204)

In 'Synthesis of an Iron Complex Salt', hydrogen peroxide (H202) is added to the solution and heat is applied until boiling. A side reaction is the formation of rust brown precipitate, which consists of potassium permanganate (KMN04) ferrous ammonium sulfate, Fe(NH4)2(SO4)2:6H20] iron (III) hydroxide, Fe(OH)3 Iron (II) oxalate (FeC204)

General Chemistry - Standalone book (MindTap Course List)

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ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.190QP

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An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)
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?
Uranium as U(VI) (as the uranyl ion; UO22+) is soluble and moves easily with groundwater, but U(VI) (as uraninite; UO2) is relatively insoluble. Several microorganisms are able to mediate this process. As such, in many uranium-contaminated aquifers, the reduction of soluble uranyl to insoluble uraninite by microorganisms has been proposed as a way to remove the dissolved uranium from water and keep it “locked up” in the subsurface. If the U(VI) is primarily complexed with carbonate (as UO2(CO3)34-), how does that influence the energy yield (or “reducibility”) of the U(VI), assuming “standard” conditions (i.e. not taking concentrations of any products or reactants into account? What about at pH 7? Under what kind of conditions would you expect to find UO2(CO3)34- vs UO22+ (and why)?
A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
The reaction 2A(g) ⇌ B(g) is found to have Kp = 24.5. What would the equilibrium constant be for 2B(g) ⇌ 4A(g)?
A student investigated the stoichiometry of the reaction of zinc (Zn) with HCl solution and reported the following data. When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCl, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 10-2M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol-1. The density of water at 27.0 °C is 0.9965 g mL-1 and its vapor pressure is 27.0 torr. R = 8.21 X 10-2 L-atm K-1 mol-1 a) determine the volume of the water displaced. b) Calculate the pressure of the H2 collected. c) Calculate the number of moles of H2 collected, using the ideal gas equation. d) Calculate the number of moles of HCl originally present in the reaction flask. e) Calculate the number of moles of HCl remaining in the flask at the end of the reaction. f) Calculate the number of moles of HCl reacting. g)…
To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.
A solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.
Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Co(NH3)62+ , Kf = 7.7×104 . Be sure to specify states such as (aq) or (s).
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.
1,5419 g of magnetite (Fe3O4) ore; Fe+2 and Fe + 3 in concentrated HCL to form a mixtureit's unraveling. Adding HNO3 to all Fe +2s Fe +3 e and Fe+3 s NH, addingwith Fe(OH)3, precipitating into. Sediment in the form of Fe3O4 after necessary operationsand 0.8525 g. Calculate the percentage of Fe3O4 in the sample.
Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudburymineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metalor metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped.Suppose that you roast 1.00 kg of the mineral maucherite, Ni11As8. The balanced equation for thereaction is:2 Ni11As8 + 31 O2 → 22 NiO + 8 As2O5(a) How many kg of NiO can be produced?(b) How many kg of the pollutant As2O5 can be produced?(c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass,and that the density of air at 25°C is 1.2 g/L.Molar masses: Ni11As8 1245.0 g/mol NiO 74.69 g/mol As2O5 229.84 g/mol

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ISBN:

9781305580343

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Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

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Cengage Learning