1. Types of Reactions in Solution and their Stoichiometry
Chapter 4
Types of Reactions in Solution and their Stoichiometry

2. Types of Chemical Reactions:
1. Precipitation Reactions (metathesis reactions) again- Table 4.1 on page 125 is important

3. Ex - Write balanced molecular, ionic, and net ionic equations for any reaction that occurs when the following are mixed:
a. BaCl2 + Na2SO4

4. b. KCl + Na2SO4

5. 2. Acid-Base Reactions - (Neutralization)
When writing acid-base reactions in net ionic form:
strong acids are written as H+
strong bases are written as OH-
Ex - Write the reactions for HClO4 + Ca(OH)2

6. 3. Reduction-Oxidation Reactions (Redox Rxns)
These reactions involve the transfer of electrons.
LEO goes GER
3 CuCl2 + 2 Al  2 AlCl3 + 3 Cu
Cu goes from a +2 to a 0 oxidation state so it is reduced. (the oxidizing agent)
Al goes from a 0 oxidation state to a +3 oxidation state so it is oxidized. (the reducing agent)

7. Rules for assigning oxidation states:
1. Free elements = 0
2. The oxidation state of a monatomic ion = its charge
3. Oxygen = -2, in peroxides such as Na2O2 it is -1
4. H = +1
5. F = -1
6. If the compound is neutral the sum of the oxidation numbers is equal to zero. If it is charged (polyatomic ion) they add to the charge of the ion.

8. Ex - Find the oxidation number of each element in H2SO4.

9. Solution Stoichiometry
Ex - What mass of NaCl is required to precipitate all the silver ions from 25.0 mL of a M solution of AgNO3?

11. Titration - Add a solution of known concentration to a solution of unknown concentration. Stoichiometry can determine the concentration of the unknown.
Ex - What is the molarity of a NaOH solution if 48.0 mL is needed to neutralize 35.0 mL of M H2SO4?

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