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:

36.  Endothermic:  Exothermic:

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

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

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

42.  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)

43.  Standard Enthalpy of Formation  Formation Reactions

44.  Hess’s Law  Equation: