Chemistry 19.1 Study Guide 4-25-12
Page 587 in book
1. Give 4 common examples of acids
2. Give 3 general characteristics of acids.
3. Explain what it means that acids can be weak electrolytes.
4. What happens when acids react with compounds containing hydroxides?
5. Give 3 common examples of bases.
6. Give 4 general characteristics of bases.
7. What did Arrhenius say about acids and when?
8. Write the formula for the hydrogen ion.
9. What did Arrhenius say about bases and when?
10. Write the formula for the hydroxide ion.
11. Explain what a monoprotic acid is and give an example of one.
12. Explain what a diprotic acid is and give an example of one.
13. Explain what a triprotic acid is and give an example of one.
14. Are all compounds that contain hydrogen acids? Explain
15. Will all the hydrogens in an acid be released as hydrogen ions? Explain
16. Which hydrogens will get released as hydrogen ions?
17. Explain why this happens.
18. Explain what happens to the hydrogen in hydrochloric acid and why.
19. Write the equation for this process.
20. Explain what happens to the hydrogen in methane and why.
21. Explain what happens to ethoic acid and how this is unique from both
hydrochloric acid and methane.
22. What base are you most familiar with and what is it used for?
23. What happens to sodium hydroxide in solution? Write the equation for this
process.
24. Explain what the word caustic means and how it applies to sodium hydroxide.
25. What happens to potassium hydroxide in solution? Write the equation for this
process.
26. What is unique about the group I metals in solution?
27. Write the equation for the reaction of sodium in water.
28. Explain what it means that sodium and potassium hydroxide are soluble in water
and what that means in terms of safely handling these solutions.
29. Explain what it means that calcium and magnesium hydroxide are not very
soluble in water.
30. Explain how these substances are used in health care.
31. Explain why the Arrhenius definition of acids and bases is not very
comprehensive.
32. Give an example of this.
33. Give the Bronsted-Lowry definition of an acid and when that was formed by these
scientists.
34. Explain what happens to ammonia when it dissolves in water and write the
equation for this process.
35. Explain what the B/L base is in this reaction and why.
36. Explain what the B/L acid is in this reaction and why.
37. What happens to the hydrogen ions in this reaction?
38. What happens to the hydroxide ion concentration in this solution compared to
pure water?
39. Write the equation for the formation of ammonium ion from ammonia and water
and label it with acid/base/conjugate acid and conjugate base.
40. Explain what a conjugate acid is.
41. Explain what a conjugate base is.
42. Explain what a conjugate acid-base pair consists of.
43. Give the 2 conjugate acid base pairs in this reaction.
44. Write the equation for the reaction between hydrochloric acid and water. Label it
with acid/base/conjugate acid and conjugate base
45. Explain what a hydronium ion is, how it is formed and its charge.
46. Explain why the hydronium ion is the conjugate acid of the base water.
47. Write the complete reaction equation for the reaction between sulfuric acid and
water.
48. Identify the base/acid/conjugate acid and conjugate base in this reaction
49. Explain what is meant by amphoteric. Give an example of an amphoteric
substance.
50. Explain the theory of acids proposed by Lewis and what year.
51. How is this different from the previous 2 theories?
52. Explain what a Lewis acid is.
53. Explain what a Lewis base is.