1. Acids and Bases

2. Properties of Acids Acids taste sour Acids effect indicators
Blue litmus turns red
Methyl orange turns red
Acids have a pH lower than 7
Acids are proton (hydrogen ion, H+) donors
Acids react with active metals, produce H2
Ex: Reactions lab
Acids react with carbonates to produce CO2
Acids neutralize bases

3. Blue litmus paper turns red in contact with an acid.
Acids Effect Indicators
Acid
Base
Blue litmus paper turns red in contact with an acid.

4. Acids Neutralize Bases

5. Effects of Acid Rain on Marble (calcium carbonate)
George Washington:
BEFORE
George Washington:
AFTER

6. Acids React with Active Metals
Magnesium
Acids react with active metals to form salts and hydrogen gas.
Mg + 2HCl  MgCl2 + H2(g)

7. Acids Taste Sour.

9. Dilutions of Acids ALWAYS ADD ACID TO WATER This reduces the chance that it will blow up in your face due to the heat of reaction making steam rapidly. The denser acid will sink and disperse more evenly.

10. An acid that contains hydrogen and one other element.
Binary Acids
An acid that contains hydrogen and one other element.

11. Naming Binary Acids
The proper method to use when naming binary acids is to begin with the hydro- prefix, use the root of the nonmetal, and add the –ic suffix.

12. Oxyacids
An oxyacid is a compound of hydrogen, oxygen, and a third element, usually a nonmetal.

13. Method for Naming Oxyacids
If the acid consists of one more oxygen than the polyatomic ion with the -ate suffix, use the per- prefix, the root of the polyatomic ion and the –ic suffix.
Example HClO4 = perchloric acid
If the acid consists of a polyatomic ion with the -ate suffix, use the root of the polyatomic ion and add –ic.
Example HClO3 = chloric acid
If the acid consists of hydrogen and a polyatomic ion with the -ite suffix, use the root of the polyatomic ion and add –ous.
Example HClO2 = chlorous acid
If an acid consists of one less oxygen than the polyatomic ion ending in –ite, use the hypo prefix, the root of the polyatomic ion and the –ous suffix.
Example HClO = hypochlorouc acid

14. Naming Acids Anion Acid _________ ide (chloride, Cl1-)
Hydro____ ic acid
(hydrochloric acid, HCl)
add H+
ions
_________ic acid
(chloric acid, HClO3)
(perchloric acid, HClO4)
_________ ate
(chlorate, ClO3-)
(perchlorate, ClO4-)
add H+
ions
_________ite
(chlorite, ClO2-)
(hypochlorite, ClO-)
______ous acid
(chlorous acid, HClO2)
(hypochlorous acid, HClO)
add H+
ions

15. Name the Acid

17. Acids you must know: Strong Acids Sulfuric acid, H2SO4
Hydrochloric acid, HCl
Nitric acid, HNO3
Weak Acids
Phosphoric acid, H3PO4
Acetic acid, CH3COOH

18. Sulfuric Acid Highest volume production of any chemical in the U.S.
Used in the production of paper
Used in production of fertilizers
Used in petroleum refining

19. Nitric Acid Used in the production of fertilizers
Used in the production of explosives
Nitric acid is a volatile acid – its reactive components evaporate easily
Stains proteins (including skin!)

20. Hydrochloric Acid Used in the pickling of steel
Used to purify magnesium from sea water
Part of gastric juice, it aids in the digestion of protein
Sold commercially as “Muriatic acid”

21. Useful for cleaning concrete
Muriatic Acid (HCl)
Sold commercially
Useful for cleaning concrete
Buyer beware

22. Phosphoric Acid A flavoring agent in sodas
Used in the manufacture of detergents
Used in the manufacture of fertilizers
Not a common laboratory reagent

23. Acetic Acid Used in the manufacture of plastics
Used in making pharmaceuticals
Acetic acid is the acid present in vinegar

24. Strength of Acids Acids are proton (hydrogen ion, H+) donors
Strong acids are assumed to be 100% ionized in solution (good proton donors).
Weak acids are usually less than 5% ionized in solution (poor proton donors).

25. Acids are Proton Donors
Monoprotic acids
Diprotic acids
Triprotic acids
HCl
HC2H3O2
HNO3
H2SO4
H2CO3
H3PO4

26. Comparison of a Monoprotic Acid to a Diprotic Acid

27. Strong acids such as HCl ionize almost completrly in solution, forming hydronium ions, H3O+
H2O + HCl 
H3O+ + Cl-
Proton
acceptor
Proton
donor

28. Weak acids favor reverse reactions and enter chemical equilibrium before many hydronium ions, H3O+ form.

29. Organic Acids
Organic acids all contain the “carboxyl” group, sometimes several of them.
The carboxyl group is a poor proton donor, so ALL organic acids are weak acids.

30. Examples of Organic Acids
Citric acid in citrus fruit
Malic acid in sour apples
Deoxyribonucleic acid, DNA
Amino acids, the building blocks of protein
Lactic acid in sour milk and sore muscles
Butyric acid in rancid butter

31. The pH scale is used to measure the strength of an acid or base
The pH scale is used to measure the strength of an acid or base. A pH of less than 7 indicates an acid. The lower the pH, the stronger the acid.

32. pH of Many Common Substances

33. Properties of Bases Bases taste bitter Bases effect indicators
Red litmus turns blue
Phenolphthalein turns purple
Bases have a pH greater than 7
Bases are proton (hydrogen ion,H+)
acceptors
Solutions of bases feel slippery
Bases neutralize acids

34. Bases Effect Indicators
Red litmus paper turns blue in contact with a base.
Phenolphthalein turns purple in a base.

35. Bases Have a pH of greater than 7
Bases Have a pH of greater than 7. The greater the pH, the stronger the base.

36. Bases Feel Slippery and Taste Bitter

37. Bases Neutralize Acids
Milk of Magnesia contains magnesium hydroxide, Mg(OH)2, which neutralizes stomach acid, HCl.
2 HCl + Mg(OH)2
MgCl2 + 2 H2O

38. Examples of Bases Sodium hydroxide (lye, Drano), NaOH
Potassium hydroxide, (Caustic Potash) KOH
Magnesium hydroxide, (milk of magnesia) Mg(OH)2
Calcium hydroxide (lime), Ca(OH)2

39. Different Acid-Base Definitions

40. Svante Arrhenius first defined acids to be proton (H+) donors and bases to be hydroxide ion (OH-) donors in aqueous solution.

41. The Arrhenius model of acids and bases is summarized by the following two reactions:

42. Bronsted-Lowry Definition of an Acid and Base
Bronsted-Lowry Acid- a molecule or ion that is a proton donor.
Bronsted-Lowry Base- a molecule or ion that is a proton acceptor.

43. Conjugate Acid-Base Pairs
The conjugate base of a Bronsted acid is the species that remains after an acid has donated a proton.
The conjugate acid of a Bronsted base is the species that is formed after the base has accepted the proton.

45. Bronsted Conjugate Acid-Base Pairs

46. The conjugate of a strong acid is a weak base
The conjugate of a strong acid is a weak base. The conjugate of a strong base is a weak acid.

47. Example of a Weak Acid Hydrofluoric Acid, HF (Hydrogen atom- Red) (Fluorine atom- Blue)

48. Lewis Acids and Bases
Lewis Acid- a molecule or ion that is an electron pair acceptor.
Lewis Base- a molecule or ion that is an electron pair donor.

49. Examples of How Bases Form Bronsted Base = Proton Acceptor Lewis Base = Electron Pair Donor

50. Bases Neutralize Acids
Evergreen shrub + concrete  dead bush
Orange juice + milk  bad taste
Under a pine tree + fertilizer  white powder
Acid + Base  Salt + Water
HCl + NaOH  NaCl + HOH

51. Products of Neutralization
HCl + NaOH 
NaCl + H2O
H2SO4 + Ca(OH)2 
CaSO H2O
HNO3 + KOH 
KNO3 + H2O
The products of neutralization are always a ______ and _______.
salt
water

52. Amphoteric
When a substance acts like an acid under one set of conditions and as a base under another set of conditions.

55. The pH scale is a way of expressing the strength of acids and bases
The pH scale is a way of expressing the strength of acids and bases. Instead of using very small numbers, we just use the NEGATIVE power of 10 on the Molarity of the H+ (or OH-) ion. Under 7 = acid 7 = neutral Over 7 = base

56. (Remember that the [ ] mean Molarity)
Calculating the pH
pH = - log [H+]
(Remember that the [ ] mean Molarity)
Example: If [H+] = 1 X pH = - log 1 X 10-10
pH = - (- 10)
pH = 10
Example: If [H+] = 1.8 X 10-5 pH = - log 1.8 X 10-5
pH = - (- 4.74)
pH = 4.74

57. Calculating [OH-] from pH
What is the [OH-] of a solution with pH = 4.95?
First find [H3O+]
4.95 = -log [H3O+]
[H3O+] =
[H3O+] = 1.12 x 10-5
Now solve for [OH-]
[OH-] = 1 x = 1.0 x 10-9
1.12 x 10-5
pH = -log[H3O+]
8.2 pH: A Measurement Scale for Acids and Bases
1 x = [H3O+][OH-]

58. Try These! pH = - log [H+] pH = - log 0.15 pH = - (- 0.82) pH = 0.82
pH = - log 3 X 10-7
pH = - (- 6.52)
pH = 6.52
Find the pH of these:
A 0.15 M solution of Hydrochloric acid
2) A 3.00 X 10-7 M solution of Nitric acid

59. pH calculations – Solving for H+
If the pH of Coke is 3.12, [H+] = ???
Because pH = - log [H+] then
- pH = log [H+]
Take antilog (10x) of both sides and get
10-pH = [H+]
[H+] = = 7.6 x 10-4 M
*** to find antilog on your calculator, look for “Shift” or “2nd function” and then the log button

60. PROBLEM: You have 50. 0 mL of 3. 0 M NaOH and you want 0. 50 M NaOH
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
Add water to the 3.0 M solution to lower its concentration to 0.50 M
Dilute the solution!

61. But how much water do we add?
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
But how much water
do we add?

62. The important point is that --->
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
How much water is added?
The important point is that --->
moles of NaOH in ORIGINAL solution =
moles of NaOH in FINAL solution

63. Amount of NaOH in original solution = M • V =
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
Amount of NaOH in original solution =
M • V =
(3.0 mol/L)(0.050 L) = mol NaOH
Amount of NaOH in final solution must also = 0.15 mol NaOH
Volume of final solution =
(0.15 mol NaOH)(1 L/0.50 mol) = 0.30 L
or mL

64. PROBLEM: You have 50. 0 mL of 3. 0 M NaOH and you want 0. 50 M NaOH
PROBLEM: You have 50.0 mL of 3.0 M NaOH and you want 0.50 M NaOH. What do you do?
Conclusion:
add 250 mL of water to 50.0 mL of 3.0 M NaOH to make 300 mL of 0.50 M NaOH.

65. Preparing Solutions by Dilution
A shortcut
M1 • V1 = M2 • V2

66. THE
END