| 1. | Safety |
| 2. |
Objectives/Overview |
| 3. |
Procedures |
| 4. | Observations |
|
5. |
Equipment |
| 6. | View
Techniques: |
| 7. | Sample Calculations |
| 8. | |
| 9. | Calculations/Set-ups |
| 10. | Conclusions |
| 11. | Grading Scale |
|
12. |
Review Prelab Questions |
| 13. | Review Postlab Questions |
- Experiment
5
Standardization
of NaOH by Titration
PRELAB QUESTIONS
References:
Brown, LeMay, and Bursten, "Chemistry: The Central Science", 8th ed.,
pp. 112-113, 117-118 (net ionic equations), pp. 114-118 (neutralization
reactions), pp. 126-136 (calculations involving solutions).
Learning Center:
ECU Lesson 44A (molarity); ECU Lesson 46 (titration);
WEN Module 12 (problems 8, 11) (molarity );
WEN Module 17 (problems 3, 8, 9) (titration);
Answers to pre and post-lab questions on file.
SHOW SET-UP FOR ALL PROBLEMS (see Set-ups)
1. Calculate the volume of 7.0 M NaOH required to prepare 500. mL of 0.30 M NaOH. Record the calculated volume in the appropriate space in your experimental procedure on page 5A.4.
2. A 25.00 mL sample of 0.5000 M H2SO4 solution requires 19.26 mL of NaOH solution to titrate to a phenolphthalein end point. Balance the following unbalanced molecular equation and then write the corresponding balanced net ionic equation, NIE. Use the stoichiometric ratio from the NIE to calculate the moles of NaOH consumed in the titration.
_____H2SO4(aq) + _____NaOH(aq) ---> _____Na2SO4(aq) + _____H2O
NIE:
3. Use the moles of NaOH calculated in #2 above to calculate the molarity of the NaOH solution.
