Name _________________________________________________________
Ionic Formulas Lab
1. Write a balanced equation for the reaction between aqueous solutions of iron (III) nitrate and sodium hydroxide.
2. Write an overall ionic equation for the above reaction.
3. Write a net ionic equation for the reaction.
Test Tube
# of drops of
0.1 M
Fe(NO3)3
# of drops of
0.1 M NaOH
Ratio of Fe3+
to OHDraw each
tube,
showing the
relative
amount of
precipitate in
each tube
and label the
color of the
solution
above the
precipitate.
Limiting
reagent
Excess
reagent
#1
4
#2
6
#3
9
#4
12
#5
18
#6
24
#7
27
32
30
27
24
18
12
9
1:8
Fe(NO3)3
NaOH
4. Which test tube actually had the most precipitate?
5. According to the formula for the precipitate, which tube theoretically should have the most precipitate?
6. If there is a difference between the theoretical and the actual, what is a possible reason for the difference?
7. Fe3+ ions in solution impart a rusty-color to the solution. Which tubes have Fe3+ ions in solution?
8. What could you do to show evidence that there are still Fe 3+ ions in solution in test tube #7, but not in test tube #1?
9. List all the ions still in solution in test tube # 4.
10. How many drops of NaOH would be needed to precipitate out all the excess Fe3+ ions still in solution in test tube #5?
11. How many drops of Fe(NO3) would be needed to precipitate out all the excess OH- ions still in solution in test tube #1?