_Although a product of a double displacement reaction may form a precipitate according to the solubility table, concentrations of the ions may be low enough that no precipitate actually forms.  Refer to p.487-490 in the text for help. 
The unit test will be next Wed., Dec.15.
Homework:  p.489 #5, 6; p.493 #10
Review for test:  p.493 #11;  p.522 #1-3, 5, 9, 10-18;  p.523-5 #5, 10, 13, 14, 15ac, 16-18;  p.640 #19

_A special kind of equilibrium constant is used when an ionic compound dissolves in water by dissociation.  The text reference is p.482-486.
Homework:  Read p.482-483 and answer p.486 #2-4
Unit Test next Wed., Dec.14.

_If you get a cubic equation to solve from an ICE table problem in which K is very small, then you make assumptions to simplify the equation.  Read the examples in the text on p.472-475.
Homework:  p.476 #7, 8; p.481 #4

_Given initial concentrations and the K value, you can calculate equilibrium concentrations of substances in an equilibrium system.  Refer to the examples in the text on p.469-470 and p.476-478 on how to use an ICE table.
Homework:  p.481 #2, 5, 6ab, 7

_At equilibrium, the concentrations of reactants and products are related in a mathematical formula that produces a constant value.  The lesson slideshow is on the unit 4 page.  Consult the text, p.439-448 and p.463-464.
Homework:  p.445 #5, 6; p.449 #3, 4, 8, 9; p.465 #1, 2

We explained the results of yesterday's experiment in groups by using Le Chatelier's Principle and posted them on the wall. 
Homework:  Lab Exercise 7.2.1 on p.514 in the text