Acids and bases are a type of reversible chemical reaction. Instead of using absorbance to decect changes in concentrations, indicators made up of organic molecules are added to acid/base solutions to produce a color change based upon H+ and OH- concentrations.
Tomorrow, we will complete our discussion of scientific theories. Please be sure to have the reading completed for a lively discussion.
HW: Complete the Chemical Equilibrium Notes in your journal by Wednesday.
1. What is a reversible reaction?
2. How do the rates of the forward and reverse reactions change throughout a reaction?
3. Write the equilibrium constant equation. How does it relate to chemical equilibrium?
4. What can you conclude about the magnitude of Keq?
5. What is the reaction quotient (Q)? How does it relate to equilibrium?
6. State Le Chatlier's principle.
7. Predict the shift in equilibrium for the following reaction if (a) CO is added, (b) As4 is removed, (c) pressure is increased:
As4O6 (s) + 6C (s) ---> As4 (g) + 6CO (g)
8. What is the Haber process? Why is an understanding of chemical equilibrium essential to the industrial production of ammonia?
9. Summarize how changes in concentration, pressure, and temperature affect reversible reactions at equilibrium. Give examples of each.
I will post an additional journal entry for (1) the "Determining the Keq of a Reaction" lab and (2) scientific theories by mid-week which will be due by Friday.
