1. Define each of the following:
        a) molar mass
        b) empirical formula

2. What do all chemical formulas tell us?

3. When is a chemical formula a molecular formula?

4. If a compound is 40% carbon by mass, what can we say about the mass of carbon in relation to the mass of the compound?

5. How many atoms of each element are present in one molecule of C₄H₆(OH)₄?

6. What is the mass of one molecule of water?

7. What is the mass of one mole of water?

8. What is the number of ions represented by the formula Ca(OH)₂?

9. What is the relationship between the number of atoms in a mole of fluorine and a mole of oxygen?

10. What is the best description of the magnesium content in the formula MgSO₄?

11. What do you need to determine the percentage composition of a substance?

12. What type of formulas are the formulas for ionic compounds?

13. Determine each of the following to the nearest whole number for the compound Ca(OH)₂:
        a) total number of atoms
        b) number of hydroxide ions
        c) mass of oxygen
        d) number of hydrogen atoms
        e) compound’s formula mass

14. Find the molar mass of each of the following:
        a) P₅
         b) KNO₃
         c) Sn(SO₄)₂

15. How many molecules are in 4 moles of HNO₃?

16. How many atoms are in 4 moles of HNO₃?

17. How many atoms are in 0.47 moles of antimony (Sb)?

18. How many moles of potassium atoms are in 5.92 x 10²⁴ atoms of potassium (K)?

19. What is the mass of 1.98 moles of Sr(ClO₂)₂?

20. How many moles of BaO are in 135.9 grams of BaO?

21. What is the percentage composition of Al(NO₃)₃?

22. What is the empirical formula of a compound that contains 22.32 g of iron (Fe), 12.96 g of sulfur (S), and 19.2 g of oxygen (O)?

23. Determine the molecular formula of a substance that is 51.06% carbon (C), 8.51% hydrogen (H), and 40.4% fluorine (F) if one mole of the substance has a mass of 94 grams?