3.HO4.H₂OH+ (cat.)MeOHNaOMe5.(CH3)2NHTsOH (cat.)

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Answered: 3. HO 4. H₂O H+ (cat.) MeOH NaOMe 5.…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 3CR

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Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
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)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
4-20 Calcium oxide is prepared by heating limestone (calcium carbonate, CaCO3) to a high temperature, at which point it decomposes to calcium oxide and carbon dioxide. Write a balanced equation for this preparation of calcium oxide.
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?
2. Write the complete chemical equation for the neutralization of NaOH with HCI. Include states of matter. (2pts) NaOH + HCl +> H,0 t Na cl i.
ter answ Aqueo us sulfurous acid (H2S03) was made by dissolving 0.200 L of sulfur dioxide gas at 19°C and 745 mm Hg in water to yield 500.0 mL of solutio n. The acid solution required 17.6 mL of so dium hydroxide solution to reach the titration end point. What was the molarity of the sodium hy droxide solution? M NaOH IID $4 7. CO
1. Phenol, CeHsOH, is a weak organic acid (MW=94 g/mol). C6H5OH(aq) + H2O(1) CeHsO (aq) + H³O*(aq) Although somewhat toxic to humans, phenol is widely used as a disinfectant and in the manufacture of plastics. If you dissolve 2.36 g of the acid in enough water to make 1.00 L of solution, what is the equilibrium hydrogen ion concentration? What is the pH of the Ans: 1.58 x 10 M; 5.80 solution?
H9SO4. H,SO4(aq)
f. ОН NaOCI CH3COOH 3.0
OEt H2SO4, H20, A EtO 3 b.) EtO OEt OEt

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3. HO 4. H₂O H+ (cat.) MeOH NaOMe 5. (CH3)2NH TsOH (cat.)