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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. First Law of Thermodynamics

  34. Internal Energy

  35. Heat, Work, and ΔE

  36. Endothermic vs. Exothermic • Endothermic: • Exothermic:

  37. State Functions

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

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

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

  41. Hess’s Law

  42. 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)

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

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

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