1. Chapters 4, and 5

2.  Solution:  Electrolyte:  Nonelectrolyte:

4.  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?

6.  Double Replacement Reaction:  Ionic Equation:  Net Ionic Equation:

7.  Predict the identity of the precipitate that forms when solutions of BaCl 2 and K 2 SO 4 are mixed. Write the balanced chemical equation for the reaction.

8.  Acid:  Base:  Strong acid or base vs weak acid or base:

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:  Oxidation:  Reduction:

13.  Determine the oxidation number of sulfur in each of the following: a.) SCl 2 b.) Na 2 SO 3 c.) SO 4 2-

14.  By acid:  By soluble salt:

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

17.  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.

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

22.  How many grams of Na 2 SO 4 are required to make 0.350 L of 0.500 M Na 2 SO 4 ?

24.  How many milliliters of 3.0 M H 2 SO 4 are needed to make 450 mL of 0.10 M H 2 SO 4 ?

25.  Titration:

26.  How many grams of Ca(OH) 2 are needed to neutralize 25.0 mL of 0.100 M HNO 3 ?

27. Thermochemistry

28.  Thermodynamics:  Thermochemistry:

31.  System:  Surroundings:

34.  Endothermic:  Exothermic:

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

36. CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O(l) ΔH = -890 kJ

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

39.  The enthalpy of reaction for the combustion of C(s) to CO 2 (g) is -393.5 kJ/mol, and the enthalpy for the combustion of CO to CO 2 is - 283.0 kJ/mol: C(s) + O 2 (g)  CO 2 (g) ΔH = -393.5 kJ CO(g) + ½ O 2 (g)  CO 2 (g) ΔH = -283.0 kJ Use this information to calculate the enthalpy for the combustion of C(s) to CO(g)

40.  Standard Enthalpy of Formation  Formation Reactions

41.  Hess’s Law  Equation:

42.  Which of the following is the correct net ionic equation for the reaction of sodium hydroxide and nitric acid?  (A) H + + OH -  H 2 O  (B) Na + + NO 3 -  NaNO 3  (C) NaOH + HNO 3  NaNO 3 + H 2 O  (D) Na + + OH - + H + + NO 3 -  NaNO 3 + H 2 O  (E) Na + + OH - + 2 H +  NaOH + H 2

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. CompoundΔh o f (kJ/mol) CO 2 (g)-393.5 CaO(s)-635.5 CaCO 3 (s)-1,207.1  The decomposition of CaCO 3 (s) is shown in the equation to the right. Using the data in the table, which of the following values is closest to the ΔH rxn of the decomposition of CaCO 3 (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 MgCl 2 (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 CH 6 N 2 + 5 O 2  2 N 2 + 2 CO 2 + 6 H 2 O(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 CH 6 N 2 if the reaction produced H 2 O(l) instead of H 2 O(g)? (The ΔH for the condensation of H 2 O(g) to H 2 O(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 Pb 2+ ions when a 100 mL 0.2M Pb(NO 3 ) 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