Unit 9: Acid/Base Study Guide
Topics to review:
1. Arrhenius definition of an acid/base
2. Brønsted-Lowry definition of an acid/base
3. Lewis definition of an acid/base
4. Solute
5. Solvent
6. Dilute vs. concentrated
7. Molarity
8. Formula for dilutions: M1V1 = M2V2
9. pH vs. pOH
10. pH scale vs. pOH scale
11. How to use your calculator for log/antilog
12. The flow chart of pH to pOH to [H+] to [OH-]
13. Hydronium vs. Hydroxide ions
14. Indicators, pH meters
15. titrations
16. burette
17. the proper technique to make a specific M solution
18. titrant
19. saturated/unsaturated
20. titrant
21. volumetric flask
Practice Problems:
1. What is the formula for molarity?
2. What is the formula for dilutions?
3. What is the formula for going from pH to pOH?
4. What is the formula for going from pH to [H+]? pOH to [OH-]?
5. What is the formula for going from [H+] to [OH-]?.
***************************** memorize all those formulas above this point!*************************
6. A saline solution contains 0.059 g of NaCl per 10mL of solution. What is the molarity of the solution?
7. How many grams of solute are present in 1.5L of 0.98M CaSO4?
Unit 9: Acid/Base Study Guide
Topics to review:
22. Arrhenius definition of an acid/base
23. Brønsted-Lowry definition of an acid/base
24. Lewis definition of an acid/base
25. Solute
26. Solvent
27. Dilute vs. concentrated
28. Molarity
29. Formula for dilutions: M1V1 = M2V2
30. pH vs. pOH
31. pH scale vs. pOH scale
32. How to use your calculator for log/antilog
33. The flow chart of pH to pOH to [H+] to [OH-]
34. Hydronium vs. Hydroxide ions
35. Indicators, pH meters
36. titrations
37. burette
38. the proper technique to make a specific M solution
39. titrant
40. saturated/unsaturated
41. titrant
42. volumetric flask
Practice Problems:
1. What is the formula for molarity?
2. What is the formula for dilutions?
3. What is the formula for going from pH to pOH?
4. What is the formula for going from pH to [H+]? pOH to [OH-]?
5. What is the formula for going from [H+] to [OH-]?.
***************************** memorize all those formulas above this point!*************************
6. A saline solution contains 0.059 g of NaCl per 10mL of solution. What is the molarity of the solution?
7. How many grams of solute are present in 1.5L of 0.98M CaSO4?
8. I need to prepare a 3.2 M NaCl solution, but all I have in my lab cabinet is 1L of a 10M NaCl solution. How much 3.2 M solution can I make?
9. If I leave 800 mL of a .75 M sodium chloride solution uncovered on a windowsill, and 45 mL of the solvent evaporates, what will the new concentration of the sodium hydroxide solution be?
10. For the following, find pH, pOH, [H+] and [OH-], then tell if it’s an acid or a base:
§ [H+] = 1.0 x 10-5
§ [OH-] = 1.0 x 10-7
§ pH = 8.3
§ [H+] = 5.4 x 10-5
§ pH = 5.2
§ pOH =10.5
11. Write out the formula for the self-ionization of water and label the hydronium ion and the hydroxide ion.
12. Acids have a higher ______ion concentration than the ______ion concentration.
13. What is the molarity of 100. mL calcium hydroxide solution that was titrated with 5.2 mL of a 0.10M hydrocyanic acid solution?
14. What is the pH of the calcium hydroxide solution above?
15. Describe with as much accuracy as possible how to make 500.0 mL of 6.10M sodium perchlorate solution.
16. Why is Arrhenius’s definition of a base inappropriate for ammonia (NH3)?
17. Show the balanced reaction of ammonia with water.
18. If it takes 50.0 mL of a 0.50M KOH solution to completely neutralize 125 mL of sulfuric acid solution, what is the concentration of the acid?
19. How many moles of lithium hydroxide are needed to exactly neutralize 2.00 moles of sulfuric acid?
20. How many mL of a 2.00M sulfuric acid solution are required to neutralize 30.0 mL of a 1.00M sodium hydroxide solution?
8. I need to prepare a 3.2 M NaCl solution, but all I have in my lab cabinet is 1L of a 10M NaCl solution. How much 3.2 M solution can I make?
9. If I leave 800 mL of a .75 M sodium chloride solution uncovered on a windowsill, and 45 mL of the solvent evaporates, what will the new concentration of the sodium hydroxide solution be?
10. For the following, find pH, pOH, [H+] and [OH-], then tell if it’s an acid or a base:
§ [H+] = 1.0 x 10-5
§ [OH-] = 1.0 x 10-7
§ pH = 8.3
§ [H+] = 5.4 x 10-5
§ pH = 5.2
§ pOH =10.5
11. Write out the formula for the self-ionization of water and label the hydronium ion and the hydroxide ion.
12. Acids have a higher ______ion concentration than the ______ion concentration.
13. What is the molarity of 100. mL calcium hydroxide solution that was titrated with 5.2 mL of a 0.10M hydrocyanic acid solution?
14. What is the pH of the calcium hydroxide solution above?
15. Describe with as much accuracy as possible how to make 500.0 mL of 6.10M sodium perchlorate solution.
16. Why is Arrhenius’s definition of a base inappropriate for ammonia (NH3)?
17. Show the balanced reaction of ammonia with water.
18. If it takes 50.0 mL of a 0.50M KOH solution to completely neutralize 125 mL of sulfuric acid solution, what is the concentration of the acid?
19. How many moles of lithium hydroxide are needed to exactly neutralize 2.00 moles of sulfuric acid?
20. How many mL of a 2.00M sulfuric acid solution are required to neutralize 30.0 mL of a 1.00M sodium hydroxide solution?