_If you try to dissolve some calcium carbonate into a solution of sodium carbonate, even less than usual will dissolve, because there is already carbonate ion present.  This shifts the dissociation equilibrium of calcium carbonate towards the solid so less dissolves.  Refer to text p.490-492.
Homework:  p.492 #8, 9, 11, 12

_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

We performed the experiment "Testing Le Chatelier's Principle" from p.514-517 in the text. 
Homework:  p.459 #2, 3, 5, 6, 8a, 10

Fritz Haber applied Le Chatelier's Principle to develop a process to make ammonia.  The text reference is p.461-462.
Homework:  Use p.515 and Table 2 on p.517 to make predictions for each part of the experiment "Testing Le Chatelier's Principle" by writing down the eqbm. eqn., with the colour of reactant or product underneath.  Then state the result of each change on the equilibrium:  will the shift be toward reactants or products, and what colour change will occur?

_Read the text p.450-456.  Answer p.457 #1, 2, 4-7.