|
|
|
|
In this lesson we continue our discussion of acids and bases. We'll be concerned with the relative strength of various acids and bases, how that is expressed, and how it relates to the position of equilibrium in an acid-base reaction. We'll also be concerned with a reaction called hydrolysis, in which an ion reacts with water to create an acidic or basic solution, and with the chemistry of buffer solutions, which have the ability to keep the pH of a solution roughly constant. You'll find answers to selected exercises and problems from the workbook on the Answer page, located in the Wrap-up.
You will have completed this lesson when you can: 1. Describe equilibrium in terms of reversible reactions. 2. Describe acid strength and base strength in terms of reversible reactions and equilibrium. 3. Recognize and distingush between strong and weak acids and bases given their formulas. 4. Relate the strength of an acid to the strength of its conjugate base. 5. Write equilibrium constant expressions for acids and bases. 6. Relate the strengths of acids and bases to values for Ka and Kb. 7. Perform calculations relating Ka, Kb, acid concentration, hydronium ion concentration, and pH. 8. Define hydrolysis. 9. Recognize substances that will undergo hydrolysis. 10. Identify neutral, acidic, and basic salts from their formulas. 11. Predict whether and explain why hydrolysis will result in an acidic or basic solution. 12. State and recognize Le Chatelier's Principle. 13. Apply Le Chatelier's Principle to predict and explain the effects that changes in concentration and pH have on acid-base systems at equilibrium. 14. Describe or recognize examples of what chemicals are needed for a buffer. 15. Describe how buffers work.
Assignments: Reading in Text: find the chapter and sections in your text that deal with the
following topics and read them. Practice Problems in Text: To be turned in:
|
|
|
