Chapters 4, and 5.  Solution:  Electrolyte:  Nonelectrolyte:

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Presentation transcript:

Chapters 4, and 5

 Solution:  Electrolyte:  Nonelectrolyte:

 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?

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

 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.

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

 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.

 Oxidation-Reduction:  Oxidation:  Reduction:

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

 By acid:  By soluble salt:

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

 Molarity:

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

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

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

 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 ?

 Titration:

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

Thermochemistry

 Thermodynamics:  Thermochemistry:

 System:  Surroundings:

 Endothermic:  Exothermic:

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

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

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

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

 Standard Enthalpy of Formation  Formation Reactions

 Hess’s Law  Equation: