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Unit 2

Unit 2. Chapters 4, and 5. Aqueous Reactions. Solution: Electrolyte: Nonelectrolyte :. Dissolving compounds and molecules. The diagram below represents an aqueous solution of one of the following compounds: MgCl 2 , KCl , or K 2 SO 4 . Which solution does the drawing best represent?.

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Unit 2

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  1. Unit 2 Chapters 4, and 5

  2. Aqueous Reactions • Solution: • Electrolyte: • Nonelectrolyte:

  3. Dissolving compounds and molecules

  4. The diagram below represents an aqueous solution of one of the following compounds: MgCl2, KCl, or K2SO4. Which solution does the drawing best represent?

  5. Solubility of Ionic Compounds

  6. Precipitation Reactions • Double Replacement Reaction: • Ionic Equation: • Net Ionic Equation:

  7. Predict the identity of the precipitate that forms when solutions of BaCl2 and K2SO4 are mixed. Write the balanced chemical equation for the reaction.

  8. Acid-Base Reactions • Acid: • Base: • Strong acid or base vs weak acid or base:

  9. Neutralization Reactions

  10. Write a balanced molecular equation for the reaction between aqueous solutions of acetic acid and barium hydroxide. Write the net ionic equation for this reaction.

  11. Oxidation-Reduction Reactions • Oxidation-Reduction: • Oxidation: • Reduction:

  12. Oxidation Numbers

  13. Determine the oxidation number of sulfur in each of the following: a.) SCl2 b.) Na2SO3 c.) SO42-

  14. Oxidation of Metals • By acid: • By soluble salt:

  15. Write the balanced molecular and net ionic equation of aluminum with hydrobromic acid.

  16. Activity Series

  17. Solution Concentration • Molarity:

  18. Calculate the molarity of a solution made by dissolving 23.4 g of sodium sulfate in enough water to form 125 mL of solution.

  19. Concentration of Electrolytes

  20. What are the molar concentrations of each of the ions present in a 0.025 M aqueous solution of calcium nitrate?

  21. Converting molarity, moles, and volume

  22. How many grams of Na2SO4 are required to make 0.350 L of 0.500 M Na2SO4?

  23. Dilution

  24. How many milliliters of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?

  25. Titrations • Titration:

  26. How many grams of Ca(OH)2 are needed to neutralize 25.0 mL of 0.100 M HNO3?

  27. Chapter 5 Thermochemistry

  28. Thermochemistry • Thermodynamics: • Thermochemistry:

  29. Types of Energy

  30. Units of Energy

  31. System and Surroundings • System: • Surroundings:

  32. Transferring Energy

  33. Internal Energy

  34. Endothermic vs. Exothermic • Endothermic: • Exothermic:

  35. Enthalpy • Enthalpy • Heat transfer from system to surroundings • Heat transfer from surroundings to system

  36. Enthalpies of Reaction CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(l) ΔH = -890 kJ

  37. How much heat is released when 4.50 g of methane gas is burned in a constant pressure system?

  38. Hess’s Law

  39. The enthalpy of reaction for the combustion of C(s) to CO2(g) is -393.5 kJ/mol, and the enthalpy for the combustion of CO to CO2 is -283.0 kJ/mol: C(s) + O2(g)  CO2(g) ΔH = -393.5 kJ CO(g) + ½ O2(g)  CO2(g) ΔH = -283.0 kJ Use this information to calculate the enthalpy for the combustion of C(s) to CO(g)

  40. Enthalpies of Formation • Standard Enthalpy of Formation • Formation Reactions

  41. Using Enthalpies of Formation • Hess’s Law • Equation:

  42. Example Questions • Which of the following is the correct net ionic equation for the reaction of sodium hydroxide and nitric acid? • (A) H+ + OH- H2O • (B) Na+ + NO3- NaNO3 • (C) NaOH + HNO3 NaNO3 + H2O • (D) Na+ + OH- + H+ + NO3- NaNO3 + H2O • (E) Na+ + OH- + 2 H+NaOH + H2

  43. What volume of distilled water should be added to 20 mL of 5 M HCl to prepare a 0.8 M solution? • (A) 100 mL • (B) 105 mL • (C) 125 mL • (D) 200 mL

  44. The decomposition of CaCO3(s) is shown in the equation to the right. Using the data in the table, which of the following values is closest to the ΔHrxn of the decomposition of CaCO3(s)? • (A) -2,240 kJ/mol • (B) -180 kJ/mol • (C) 180 kJ/mol • (D) 1,207 kJ/mol • (E) 2,240 kJ/mol

  45. A 0.2 mol sample of MgCl2(s) and a 0.1 mol sample of KCl(s) are dissolved in 500 mL of water. What is the concentration of Cl- in the resulting solution? • (A) 0.15 M • (B) 0.30 M • (C) 0.60 M • (D) 1.0 M

  46. 2 CH6N2 + 5 O2 2 N2 + 2 CO2 + 6 H2O(g) • The combustion of methylhydrazine, is represented above. The ΔH of this reaction is -1,303 kJ/mol. What would bout the ΔH per mole CH6N2 if the reaction produced H2O(l) instead of H2O(g)? (The ΔH for the condensation of H2O(g) to H2O(l) is -44 jk/mol) • (A) -1,171 kJ • (B) -1,259 kJ • (C) -1,347 kJ • (D) -1,435 kJ

  47. What is the final concentration of Pb2+ ions when a 100 mL 0.2M Pb(NO3)2 solution is mixed with a 100 mL 0.30 M NaCl solution? • (A) 0.005 M • (B) 0.010 M • (C) 0.015 M • (D) 0.025 M

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