1. Unit 5 Review
Notes #18-21

2. Groups Group 1: Sophia, Evan, Mac Group 2: Brandon, Hunter, Harrison
Group 3: Haley, Chase, Nick
Group 4: Brooks, Austin, Nathan
Group 5: Amanda, Blake, Patrick
Group 6: Parker, Matt, Drew, Madison
Groups

3. Directions Every group participates in every question.
Each question is timed.
You can “re-do” your answer as long as it fits into the time limit.
Your answer must be written on a piece of paper.
Winning group gets extra credit on test.
Directions

4. 1 Point 1 Extra Define Acid and Base using Arrhenius’ definition.
Extra: Give one example of an Arrhenius acid and one example of a Arrhenius base.
1 Point 1 Extra

5. 2 Points Define acids and bases using 1) Bronsted Lowry definition and
2)Lewis definition
2 Points

6. For the following reaction, identify the acid and base using bronsted lowry definition:
HNO3 + H2O  H3O+ + NO3-
2 Points

7. For the following reaction, identify the conjugate acid and base using the standard notation. (Connecting using lines)
HNO3 + H2O  H3O+ + NO3-
2 Points

8. What does Kw mean?
1 point

9. What are the concentrations of [H+] and [OH-] of pure water (At room temp)?
HINT: Why is water neutral?
1 Point

10. T/F
If the [H+] is greater than 1.0 x 10-7, the solution is basic.
YOU NEED TO MEMORIZE THESE
1 point

11. [H+] < 1.0 x = basic
[H+] > 1.0 x = acidic
MEMORIZE

12. Is this solution acidic or basic?
[OH-] = 3.5 x 10-10
2 Points

13. What is the hydrogen ion concentration of a solution with the pH of 5
2 points

14. What is the hydroxide ion concentration of a solution with a pH of 9.5?
3 Points

15. Why do weak acids have a small Ka compared to strong acids
Why do weak acids have a small Ka compared to strong acids. Use the equation to explain your answer.
1 Point

16. When a 1.5M solution of benzoic acid partially ionizes , the concentration of hydrogen ions at equilibrium is [H+] = 4.6 x 10-2 M. What is the Ka for this weak acid?
3 Points

17. Predict the products of this neutralization reaction and balance it:
H2SO4 + LiOH 
H+1 , SO4-2 , Li+1 , OH-1
2 Points

18. 3 Points Using the previous equation… H2SO4 + LiOH 
What is the molarity of lithium hydroxide if 15 mL of lithium hydroxide is neutralized by 17.6 mL of 2M sulfuric acid?
3 Points

19. 3 Points Using Bronsted Lowry Definition:
1) What is the conjugate base of H2SO4?
2) What is the conjugate acid of H2O?
3) What is the conjugate acid of NO3-?
3 Points

20. When dealing with acid base reactions, why is water unlike any other acid or base?
1 Point

21. Calculate the pH of a solution with a hydrogen ion concentration of
[H+] = 2.2 x 10-4.
2 Points

22. Calculate the pH of a solution that contains a hydroxide ion concentration of
[OH-] = 1 x 10-4
2 Points

23. What is a buffer?
1 Point

24. How could you create a buffer solution?
1 Point

25. T/F
Buffers are always neutral (pH=7).
Explain why or why not
1 Point

26. Describe one application of acid base chemistry in the real world (outside of the classroom).
2 Points