Final Exam Study Guide Preview
General Info:
- 2 hr. to complete the exam
- 1 hr. for a lab (approximately 25 pts.)
- 1 hr. for written portion (approx. 25 pts.) [MC / 1 or 2 short answer / 2 short Essays]
What you should study:
- Solutions/Acids/Bases Notes
- Molarity/Molality/Dilution calculation WS
- pH/pOH calculation WS
What you should be able to do:
-
Complete a lab investigation with a group within 1 hour.
Define acids & bases and classify as weak or strong
Calculate pH or pOH
Calculate hydronium or hydroxide concentration
Calculate molarity or molality (or the other variables associated with them)
Describe the solvation process
Define unsaturated, supersaturated, saturated, electrolyte, & nonelectrolyte
Describe the difference between ionic and molecular compounds dissolving
State the general characterizes of acids and bases
Be familiar with the pH scale
Calculate either moles of grams of a compound, given mol or g
Compare and contrast molarity and molality.
Understand and apply the rule of “Like dissolves Like”
State the ways to increase the solubility of a gas or solid
1. Define the following and put an example:
Saturated –
Unsaturated –
Supersaturated –
Electrolyte –
Nonelectrolyte –
Arrhenius Acid –
Arrhenius Base –
Bronsted-Lowry Acid –
Bronsted-Lowry Base –
Lewis Acid –
Lewis Base –
Strong Acids/Bases –
Give several examples of each:
Weak Acids/Bases –
Give several examples of each:
2. Describe the solvation process of an ionic vs. a molecular compound in water. (use scientific terms and be specific)
3. Describe how soap/detergent helps to get a nonpolar-based stain out of a piece of clothing:
4. What are the characteristic of acids?
5. What are the characteristics of bases?
6. State the ways to increase the solubility of a gas or solid:
7. How many grams of ammonium sulfate are needed to make a 0.35 L solution at a concentration of 6.0 M?
8. How many liters of 2.4 M solution can be made using 78 grams of isopropanol (C3H8O)?
9. What mass of water is required to dissolve 175 g KNO3 to produce a 1.25 m solution?
10. What mass of HC2H3O2 must be dissolved in 700. g H2O to produce a 6.25 m solution?
11. What volume of 12.8M HNO3 is required to make 250 mL of a 5.0M solution?
12. Draw and label the pH scale: include some examples of items and where they fall on the scale.
13. Explain the rule “like dissolves like.”
14. Compare and contrast molarity and molality in terms of preparation, equation, equipment used, ect…
15. What is the pH of a solution that contains 35 grams of hydrochloric acid (HCl) dissolved in 1.5 liters of solution?
16. What is the pH of a solution that contains 1.32 grams of nitric acid (HNO3) dissolved in 850 mL of solution?
17. What is the pH of a solution that contains 1.2 moles of nitric acid (HNO3) and 1.9 moles of hydrochloric acid (HCl)
dissolved in 1000 liters of solution?
18. If a solution has a [H+] concentration of 5.5 x 10-7 M, is this an acidic or basic solution? Explain.
19. An acidic solution has a pH of 5. If I dilute 10 mL of this solution to a final volume of 1000 mL, what is the pH of the
resulting solution?
20. What is a titration and what is it used for?
21.
3.45 x 10-4
2.45 x 10-11
9.278
9.05
22. If I have 25.2g of sodium hydroxide, how many moles do I have?
23. I have 2.5 mol of sodium sulphate, how many grams do I have?