1. What is the initial pH of
the solution in the Erlenmeyer flask?
2. What does this
pH tell you about the “type” of solution we
are beginning with (hint: is it an acid or base?)?
3. What ions are
present in the Erlenmeyer flask initially?
4. What ions are
present in the buret initially?
5. Draw a diagram
of the lab set-up in your notebook and label the solutions
6. Begin your virtual
7. Add 5.00 mL
8. Does the pH
change? Explain what is happening to the ions in the Erlenmeyer
9. Now add 15.00
mL of NaOH
10. What is the
“new” pH? What is happening to the solution
in the Erlenmeyer flask?
11. Now add, 10.00
mL more of NaOH to the flask, what happens to the pH? Why
do you think there is such a change?
12. Explain why
accuracy and precision are so important when performing
13. What is the
total volume of solution in the Erlenmeyer flask now?
14. At pH=7.00,
what ions/molecules are present in the Erlenmeyer flask?
15. Now add 5.00
mL more of NaOH.
16. What happens
to the pH?
17. Add 5.00 mL
of NaOH again. Does the pH change?
18. Make a sketch
of the titration curve, labeling the axes, with pH as the
dependant variable and volume of NaOH as the independent