Definitions:
1. mole                                        10. molarity
2. Avogadro’s number                 11. percent composition
3. molar mass                              12. empirical formula
4. solute                                      13. molecular formula
5. solvent                                    14. precision
6. dilute                                       15. accuracy
7. concentrated                           16. significant digit
8. concentration                          17. exact number
9. ppm

Questions:
1. Why is it necessary to use a term, like mole, which id a large quantity?
2. How is the number of atoms determined?
3. What does the atomic mass on the periodic table tell you?
4. How is the molar mass of a compound determined?
5. Summarize the conversion relationships in Table 4-1 p. 133.
6. State a couple of examples of how the unit ppm is used.
7. Write the formula for molarity.
8. Write the formula for determining percent composition.
9. List the steps necessary to determine an empirical formula.
10. How is an empirical formula related to a molecular formula? How is molecular mass related to empirical formula mass?
11. Write an equation for percent error.
12. List the rules for counting significant figures.
13. List the rules for significant figures when multiplying & dividing and for when adding & subtracting.
14. Do exact numbers limit the number of significant digits?
15. What is the rule for rounding five’s?

Problems:
p. 126  # 1,2                  p. 129  #  3,4
p. 131 # 5,6                   p. 132 # 7,8
p. 135  # 11,13,14,15,16,17,18,19,20,21,22
p. 140 # 24,25
p. 141  # 26,27,29,30,31
p. 144 # 32,33               p. 146  # 34,35
p. 148  # 36,37              p. 150 # 38,39
p. 153  # 41,42,43,44,45,46,47,49,50,51
p.156 through p.159  # 3,4,5,6,7,8,9,10,11,13,14, 15,17,    18,19,20,21,22,23,24,25,26,27,28,29,30,31,32,33, 34,35,36,37,38,39, 40,41,42,43,44