Unit 2Chapters 4, and 5

Solution:

Electrolyte:

Nonelectrolyte:

Aqueous Reactions

Dissolving compounds and molecules

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

Solubility of Ionic Compounds

Double Replacement Reaction:

Ionic Equation:

Net Ionic Equation:

Precipitation Reactions

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

Acid:

Base:

Strong acid or base vs weak acid or base:

Acid-Base Reactions

Neutralization Reactions

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:

Oxidation-Reduction Reactions

Oxidation Numbers

Determine the oxidation number of sulfur in each of the following:

a.) SCl2

b.) Na2SO3

c.) SO42-

By acid:

By soluble salt:

Oxidation of Metals

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

Activity Series

Molarity:

Solution Concentration

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

Concentration of Electrolytes

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

Converting molarity, moles, and volume

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

Dilution

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

Titration:

Titrations

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

Chapter 5Thermochemistry

Thermodynamics:

Thermochemistry:

Thermochemistry

Types of Energy

Units of Energy

System:

Surroundings:

System and Surroundings

Transferring Energy

First Law of Thermodynamics

Internal Energy

Heat, Work, and ΔE

Endothermic:

Exothermic:

Endothermic vs. Exothermic

State Functions

Enthalpy

Heat transfer from system to surroundings

Heat transfer from surroundings to system

Enthalpy

CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l)

ΔH = -890 kJ

Enthalpies of Reaction

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

Hess’s Law

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)

Standard Enthalpy of Formation

Formation Reactions

Enthalpies of Formation

Hess’s Law

Equation:

Using Enthalpies of Formation