Chemistry Ch 10 Acids and Bases

23. Which type of solution is one with a pH of 8?

Basic

37. Be able to identify the Bronsted-Lowry bases in a given reaction. An example is given.

H2S + H2O H3O+ + HS-base

3. What is the formula for phosphoric acid?

H3PO4

49. What substances are present in a buffer?

Hydrogen ions

42. What products result from a neutralization reaction?

Salt and water

34. Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base?

Water

14. A liter of impure water has 10-4 mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water?

[H3O+] = 1 x 10-10 mol

6. What is the charge on the hydronium ion?

+1

15. What is the concentration of hydronium ions in a neutral solution?

1 x 10-7 M

9. If the hydroxide ion concentration is 10-10M, what is the pH of the solution?

4

45. What measuring instrument is used in a titration?

A buret and Erlenmeyer flask or beaker

26. What is an acid according to Arrhenius?

A compound that increases the number of positively charged ions, H+, when added to water

44. What type of reaction is an acid-base reaction?

A neutralizing reaction

39. Which acid can be concentrated but is always weak?

Acetic acid

18. What is a solution in which the hydroxide-ion concentration is 1 x 10-8M is classified as?

Acidic

7. If the hydrogen ion concentration is 10-10M, is the solution acidic, alkaline, or neutral?

Alkaline

36. What is the term used to describe a substance that can be both an acid and a base?

Amphiprotic

47. Which substance when dissolved in water will produce a solution with a pH greater than 7?

B) NaCl

17. What is a solution in which the hydroxide-ion concentration is 1 x 10-4M classified as?

Basic

54. Be able to identify what is reduced in chemical reaction equation? An example follows. S + Cl2 à SCl2

Chlorine is reduced

46. What is the purpose of a titration

Discover the concentration of an unknown acid or base

33. What is an acid according to Bronsted?

Donation of protons in the form of a hydrogen ion

55. What are transferred in an oxidation-reduction reaction?

Electrons

19. What is the formula of the hydrogen ion is often written as?

H+

21. In a neutral solution, what is concentration of the [H+] and [OH-]?[

H+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M

20. What are the products of self-ionization of water?

Hydronium and hydroxide ion

41. With solutions of "strong" acids and "strong" bases, what does the word "strong" refer to?

It completely ionizes into ions

50. If an atom is reduced in a redox reaction, what must occur to another atom in the system?

It must be oxidized

48. What does a buffer do?

Neutralizing the effects of adding acid or bases

57. In which types of reaction are electrons lost?

Oxidation reactions

51. In the reaction of sodium with oxygen, which atom is reduced?

Oxygen

35. What is transferred between a conjugate acid-base pair?

Proton

4. Which of the following is a property of an acid?

Reacts with metals

56. What is another name for an oxidation-reduction reaction?

Redox reaction

53. Be able to identify the reducing agent in the reaction equation. An example follows. 2Na + Sà Na2S

Reducing agent = Na

1. When an acid reacts with a base what compounds are formed?

Salt and Water

52. In the reaction of sodium with oxygen, which atom is the reducing agent?

Sodium

27. What type of acid is sulfuric acid?

Strong Acid

2. What is the name of H2SO3?

Sulfurous Acid

58. What occurs in the oxidation part of a redox reaction?

The atom increases its oxidation number and loses electrons

5. What is a property of a base?

They taste bitter and feel slippery

28. Which hydrogens can ionize in a compound?

Those bonded to highly electronegative atoms

29. Which hydroxides can ionize in a compound

Those bonded to metal ions

40. What would a solution that ionizes only slightly in a 0.12M solution be termed?

Weak and dilute

25. An indicator is what type of compound?

Weak base or acid

38. According to the Bronsted-Lowry theory, when does water act as a base?

When it accepts a proton

30. What is the basic equation that represents the dissociation of a metal hydroxide in water? (Note: no charges are shown and the reactions are not balanced.)

XOH + A + H

11. If the pH is 6, what is the concentration of hydrogen ion?

[H+] = 1 x 10-6 M

16. For a solution to be classified as acidic, what must the relationship between hydrogen-ion concentration and the hydroxide-ion concentration be?

[H+] = 7 > pH > 1 and [OH-] = 7 < pH < 14

8. If the [H+] in a solution is 1 x 10-1 mol/L, what is the [OH-]?

[OH-] = 1 x 10-13 M

10. If the pH is 9, what is the concentration of hydroxide ion?

[OH-] = 1 x 10-5 M

24. What is the hydroxide- ion concentration of a solution with a pH of 5.0?

[OH-] = 1 x 10-9 M

22. What is the definition of pH

pH = -log[H+]

12. If [OH-] = 1 x 10-4M, what is the pH of the solution?

pH = 10

13. If [H+] = 1 x 10-11M, what is the pH of the solution?

pH = 11