Moving to another question will save this response. Question 2 What is the net ionic equation for the reaction of aqueous potassium hydroxide and aqueous magnesium chlori 1S K (aq) + OH (aq) KOH(s) КОНЕ) K*(aq) + Cl (aq) →KCI(s) Mg"(aq) + 2 CF (aq) MgCl2(s) 2+ o Mg-(aq)+3 OH (aq)Mg(0H)3(s) Mg-(aq) -2 OH (aq) Mg(OH)2(s) Me (aq) - Он (аq) — MgОН (9) MGOH (s A Moving to another question will save this response. search hp f11 f12 fg f10 f6 f7 f8 f4 f5 I미 & %24 4. 6. 7. 80 T. | 0O

Moving to another question will save this response. Question 2 What is the net ionic equation for the reaction of aqueous potassium hydroxide and aqueous magnesium chlori 1S K (aq) + OH (aq) KOH(s) КОНЕ) K*(aq) + Cl (aq) →KCI(s) Mg"(aq) + 2 CF (aq) MgCl2(s) 2+ o Mg-(aq)+3 OH (aq)Mg(0H)3(s) Mg-(aq) -2 OH (aq) Mg(OH)2(s) Me (aq) - Он (аq) — MgОН (9) MGOH (s A Moving to another question will save this response. search hp f11 f12 fg f10 f6 f7 f8 f4 f5 I미 & %24 4. 6. 7. 80 T. | 0O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) MnCl, (aq) + 2 H,0(1) + Cl, (g) How much MnO, (s) should be added to excess HCl(aq) to obtain 205 mL CI, (g) at 25 °C and 735 Torr? mass of MnO2: g
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCl(aq) - MnCl, (aq) + 2 H,O(1) + Cl, (g) How much Mn0, (s) should be added to excess HCI(aq) to obtain 235 mL Cl, (g) at 25 °C and 735 Torr? mass of MnO,: g
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq). The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.
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One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5
Write the net ionic equation, including phases, that corresponds to the reaction Cu(NO3)2(aq)+K2S(aq)⟶CuS(s)+2KNO3(aq)
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq) + Cl (aq) → AgCl(s), AH=-65.5 k.J |
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Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO, (s) + 4 HCI(aq) – MnCl, (aq) + 2 H,0(1) + Cl, (g) > How much MnO, (s) should be added to excess HCl(aq) to obtain 105 mL Cl, (g) at 25 °C and 755 Torr? mass of MnO,:
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[References] Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas ( CH4) by the following process: 2NH3 (g) + 30,(g) + 2CH, (g) →→ 2HCN(g) + 6H,0(g) Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 5.75 g NH3, 12.0 g 02, and 5.00 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written? Mass = HCN