1. Before the Bell Rings
HW check will be at end of class.

2. ETD 63 2019 What is the pH of a 0.012 M HCl solution?
What is the pH of a solution if [OH-] is 1.0 x 10-3 M?
How many grams of HNO3 are needed to give a pH of 3.65 in a 11.5L tank? (Molar mass for HNO3 is 63.1g/mol)

3. ETD 63Ans
What is the pH of a M HCl solution?

4. ETD 63Ans 2019 What is the pH of a solution if [OH-] is 1.0 x 10-3 M?
What is the pH of a M HCl solution?
What is the pH of a solution if [OH-] is 1.0 x 10-3 M?

5. ETD
How many grams of HNO3 are needed to give a pH of 3.65 in a 11.5L tank? (Molar mass for HNO3 is 63.1g/mol)
What is the pH of a solution if [OH-] is 1.0 x 10-3 M?
What is the pH of a M HCl solution?

6. Learning Targets
I can explain how to do a titration and what the equivalence point represents.

7. Tests Come finish/take missing tests.
Corrections for all tests can be done.
June 14th- Last day for corrections or late work to be done

8. Notebook Check Our final notebook check will be due next class.
Grade yourself, checking ETDs #46-63
1 point for ETD#
1 point for question
1 point for answer
This is optional for seniors.

9. Homework Review

10. Titration Notes

11. Titration Knowledge Background:
When an acid and base are mixed, they form water and a salt (neutralization reaction)
NaOH + HCl  H2O + NaCl
We can determine how much base is needed to neutralize an acid using a titration

12. Titration Curves
Delivery measured volume of a solution of known concentration (titrant) to analyze an unknown solution (analyte)
Titrant = the thing being added (base in buret)
Analyte = solution that’s being added to (acid in Beaker)
Titrant added to the analyte until the solution has reached the
Equivalence Point!

13. Equivalence point =
Point where moles of acid = moles of base (reaction to completion)
Not always pH of 7!!!!!
Middle, near vertical part of the curve

15. Why is the pH not always 7 at Equiv. Pt.?
Equivalence Point is where moles of acid = moles of base
(NOT where [H+] = [OH-])
Strong Acid vs. Strong Base
HCl gives off 100% of it’s H+; NaOH gives off 100% of it’s [OH-]
0.5M of HCl gives off [H+] of 0.5
0.5M NaOH gives off [OH-] of 0.5
[H+] = [OH-] = pH of 7

16. Why is the pH not always 7? Strong Acid vs. Weak Base:
HCl gives off 100% of it’s H+; NH3 results in only 50% [OH-]
0.5M of HCl gives off [H+] of 0.5
0.5M NH3 gives off [OH-] of 0.25
[H+] > [OH-] = pH less than 7 at equivalence pt.

17. Easy way to remember
Whatever is strong, the equivalence pH will be on that side of the scale.
For example, a strong acid with a weak base will end up on the acidic side of the pH scale (pH<7).
A strong base and a weak acid will end up being basic at equivalence (pH >7).
Strong and strong, weak and weak, will both be an equivalence of about pH=7.

18. Learning Targets
I can explain how to do a titration and what the equivalence point represents.

19. Home work Notebook check #46-#63 Make your notecard for the final
Due next class
Make your notecard for the final
3” x 5” card, front and back.
Work on the semester final review packet