Heavy metal sulfides like CdS and PbS are often significant components of mine tailings (the piles of waste and low-grade ores discarded by a mining operation). While these sulfides are quite insoluble in water (Ksp of CdS = 1 E -27, Ksp of PbS = 3 E -28), over the years rainwater and snowmelt can slowly dissolve small amounts of these heavy metals, washing them into streams and other natural waters. If these mine tailings are located in an area that is impacted by acid rain, would you expect heavy metal dissolution into natural waters to increase or decrease? Use chemical reactions to justify your answer.

Heavy metal sulfides like CdS and PbS are often significant components of mine tailings (the piles of waste and low-grade ores discarded by a mining operation). While these sulfides are quite insoluble in water (Ksp of CdS = 1 E -27, Ksp of PbS = 3 E -28), over the years rainwater and snowmelt can slowly dissolve small amounts of these heavy metals, washing them into streams and other natural waters. If these mine tailings are located in an area that is impacted by acid rain, would you expect heavy metal dissolution into natural waters to increase or decrease? Use chemical reactions to justify your answer.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter20: The Representative Elements

Section: Chapter Questions

Problem 54E

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The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; ClO- is reduced to Cl-. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S2O3; I2 is reduced to I-. The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S4O6. In this analysis, potassium iodide was added in excess to 5.00 mL of bleach (d=1.00g/cm3) . If 25.00 mL of 0.0700 M Na2S2O3 was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of NaClO in the bleach?
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 2.00 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
The use of silica to form slag in the production of phospho-rus from phosphate rock was introduced by Robert Boyle morethan 300 years ago. When fluorapatite [Ca₅(PO₄)₃F] is used inphosphorus production, most of the fluorine atoms appear in theslag, but some end up in toxic and corrosive SiF₄ (g).(a) If 15% by mass of the fluorine in 100. kg of Ca₅(PO₄)₃F forms SiF₄, what volume of this gas is collected at 1.00 atm andthe industrial furnace temperature of 1450.°C?(b) In some facilities, the SiF₄ is used to produce sodium hexa-fluorosilicate (Na₄SiF₆) which is sold for water fluoridation: 2SiF₄(g)+Na₂CO₃(s)+H₂O(l) →Na₂SiF₆(aq)+SiO₂(s)+CO₂(g)+2HF(aq) How many cubic meters of drinking water can be fluoridated toa level of 1.0 ppm of Fusing the SiF₄ produced in part (a)?
An impurity sometimes found in Ca₃(PO₄)₂ is Fe₂O₃, whichis removed during the production of phosphorus as ferrophos-phorus(Fe₂P). (a) Why is this impurity troubling from an eco-nomic standpoint? (b) If 50. metric tons of crude Ca₃(PO₄)₂ contains 2.0% Fe₂O₃ by mass and the overall yield of phospho-rus is 90.%, how many metric tons of P₄ can be isolated?
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)
The titanium chloride then reacts with liquid magnesium at 900°C to givetitanium and magnesium chloride (MgCl2). Write a balanced chemicalequation for this step in the refining of titanium.
Thortveitite is a mineral that contains the silicate ion [Si2O7]6-. The structure of this ion is such that the each Si atom is bonded to three terminal oxygen atoms, and the seventh O atom forms a bridge between the two Si atoms:[O3Si-O-SiO3]6-
Describe the role of (i) NaCN in the extraction of gold from gold ore. (ii) Si02 in the extraction of copper from copper matte. (iii) Iodine in the refining of zirconium. Write chemical equations for the involved reactions.
Define the term silicates?
Tourmaline is the most colorful of all gemstones. It neutralizes negative forces and offers emotional stability. It is crystalline boron silicates compounded with metals such as Mg, Fe, Al, Na and Li. The three most well-known minerals of tourmaline are: Elbaite Na(LiAl2)Al6Si6O18(BO3)3(OH)4 Schorl Na(Fe3)Al6(BO3)3Si6O18(OH)4 Dravite Na(Mg3)Al6(BO3)3Si6O18(OH)4 On a basis of 1000 kg of tourmaline rocks containing 25% Elbaite, 35% Schorl, 30% Dravite and 10% inerts, calculate the following: a) kg-mol Elbaite b) % by wt BO3 in tourmaline rocks
Tourmaline is the most colorful of all gemstones. It neutralizes negative forces and offers emotional stability. It is crystalline boron silicates compounded with metals such as Mg, Fe, Al, Na and Li. The three most well-known minerals of tourmaline are: Elbaite Na(LiAl2)Al6Si6O18(BO3)3(OH)4 Schorl Na(Fe3)Al6(BO3)3Si6O18(OH)4 Dravite Na(Mg3)Al6(BO3)3Si6O18(OH)4 On a basis of 1000 kg of tourmaline rocks containing 25% Elbaite, 35% Schorl, 30% Dravite and 10% inerts, calculate the following: a) kg Fe b) total kg-atom O and kg-mol O2 in the three minerals c) total number of Mg atoms in the rocks
1 Explain in detail what is the importance 2 the uses of pure Cobalt(II) sulphate ( CoSO4.7H2O )

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