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Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions:Mg2+(aq) + Ca(OH)2(aq) ⟶ Mg(OH)2(s) + Ca2+(aq)Mg(OH)2(s) + 2HCl(aq) ⟶ MgCl2(s) + 2H2 O(l)MgCl2(l) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯→ electrolysis Mg(s) + Cl2(g)Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium as Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2 is required to precipitate 99.9% of the magnesium in 1.00 × 103 L of sea water?

Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions:Mg2+(aq) + Ca(OH)2(aq) ⟶ Mg(OH)2(s) + Ca2+(aq)Mg(OH)2(s) + 2HCl(aq) ⟶ MgCl2(s) + 2H2 O(l)MgCl2(l) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯→ electrolysis Mg(s) + Cl2(g)Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium as Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2 is required to precipitate 99.9% of the magnesium in 1.00 × 103 L of sea water?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
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Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions:
Mg2+(aq) + Ca(OH)2(aq) ⟶ Mg(OH)2(s) + Ca2+(aq)
Mg(OH)2(s) + 2HCl(aq) ⟶ MgCl2(s) + 2H2 O(l)
MgCl2(l) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯→ electrolysis Mg(s) + Cl2(g)
Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium as Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2 is required to precipitate 99.9% of the magnesium in 1.00 × 103 L of sea water?

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