1. Acids, Bases, and Salts
All ionic compounds can be classified as one of these three.
All are types of electrolytes (conduct electricity in aqueous solutions)
Acids and bases are found many places in everyday life:
Acids:
lemon juice, car batteries, vinegar, orange juice
Bases:
ammonia, lye, blood

2. Acids Taste sour Begin with H Found in many foods and drinks
Turn blue litmus paper red
pH 0-6.9
Corrosive
react with metals to generate H2(g)
react with metal oxides and hydroxides to form salts and water
Forms H+ (or H30+)ions in solutions
Hydrogen
Hydronium

3. Bases Bitter Normally end in OH Turn red litmus paper blue pH 7.1-14
Found in many cleaning products
Slippery
Corrosive
react with acids to form salts and water
Forms OH- ions in solution
Hydroxide

4. Acids and Bases Neutral: H+ = OH- Acidic: H+ > OH-
Basic: H+ < OH-
↑H+ = ↓OH- = more acidic = ↓ pH ac
idic
↓H+ = ↑OH- = more basic = ↑ pH

5. Water = Neutral H2O = HOH HOH → H+ + OH- Free Hydrogen ion bonds
with water molecule to
form Hydronium ion
H+ and H3O+ used
interchangeably

6. Hydronium Ion = Hydrogen Ion
Self ionization - two water molecules react to form a hydronium ion (H3O+) and hydroxide ion.
H20 → H OH-

7. pH scale Shows the strength of acid or base on a scale of 0-14.
Numbers below 7 = acids…the lower the number, the more acidic
Numbers above 7 – bases…the higher the number the more basic.

9. pH and pOH
Formula: pH + pOH = 14
Ex. 1) If the pH = 2, what is pOH?

10. pH and pOH Formula: pH + pOH = 14 Ex. 1) If the pH = 2, what is pOH?

11. pH and pOH Formula: pH + pOH = 14 Ex. 1) If the pH = 2, what is pOH?

12. pH and pOH Formula: pH + pOH = 14
Ex. 2) If the pH = 4, what is the pOH?

13. pH and pOH Formula: pH + pOH = 14
Ex. 2) If the pH = 4, what is the pOH?
4 + pOH = 14
pOH = 14 – 4
pOH = 10

14. pH and pOH Formula: pH + pOH = 14
Ex. 3) If the pOH = 7, what is the pH?

15. pH and pOH Formula: pH + pOH = 14
Ex. 3) If the pOH = 7, what is the pH?
pH + 7 = 14
pH = 14 – 7
pH = 7

16. Calculating pH Formula: pH = -log [ H+ ] OR pH = -log [ H3O+ ]
You can calculate pH by finding the negative logarithm of the concentration of hydrogen ions.

17. Calculating pH
Ex. 4) A solution contains 1.0 x mol/L of H+ ions, what is the pH of this solution?
Formula: pH= -log [H+]

18. Calculating pH
Ex. 4) A solution contains 1.0 x mol/L of H+ ions, what is the pH of this solution?
Formula: pH= -log [H+]
pH = -log (1.0 x 10-8)
In calculator pH = -log (1.0 E -8)

19. Calculating pH
Ex. 4) A solution contains 1.0 x mol/L of H+ ions, what is the pH of this solution?
Formula: pH= -log [H+]
pH = -log (1.0 x 10-8)
In calculator pH = -log (1.0 E -8)
pH = =

20. Calculating pH
Ex. 4) A solution contains 1.0 x mol/L of H+ ions, what is the pH of this solution?
Formula: pH= -log [H+]
pH = -log (1.0 x 10-8)
In calculator pH = -log (1.0 E -8)
pH = = Base

21. Calculating pH
Ex. 5) A solution contains 3.5 x 10-5 M of H+ ions, what is the pH of the solution?
Formula: pH= -log [H+]

22. Calculating pH
Ex. 5) A solution contains 3.5 x 10-5 M of H+ ions, what is the pH of the solution?
Formula: pH= -log [H+]
pH= -log (3.5 x 10-5)
In calculator pH= -log (3.5 E -5)

23. Calculating pH
Ex. 5) A solution contains 3.5 x 10-5 M of H+ ions, what is the pH of the solution?
Formula: pH= -log [H+]
pH= -log ( 3.5 x 10-5)
In calculator pH= -log ( 3.5 E -5)
pH = =

24. Calculating pH
Ex. 5) A solution contains 3.5 x 10-5 M of H+ ions, what is the pH of the solution?
Formula: pH= -log [H+]
pH= -log ( 3.5 x 10-5)
In calculator pH= -log ( 3.5 E -5)
pH = = acid

25. pH and Water
Water is amphoteric; it can act as both an acid and a base in an aqueous solution.
Water contains an equal number of H+ and OH- ions.
H2O H+
+ OH-

26. Ion Product Constant of Water
Kw is the ion product constant for water.
Represents the equilibrium for the self ionization of water.
Formula:
Kw = [H+][ OH-]

27. Ex. 6) What is the Kw if [H+] = 1.0 x 10-7 and [ OH-]= 1.0 x 10-7?

28. Ex. 6) What is the Kw if [H+] = 1.0 x 10-7 and [ OH-]= 1.0 x 10-7?
Kw = [H+][ OH-]

29. Ex. 6) What is the Kw if [H+] = 1.0 x 10-7 and [ OH-]= 1.0 x 10-7?
Kw = [H+][ OH-]
Kw= (1.0 x 10-7) x (1.0 x 10-7)

30. Ex. 6) What is the Kw if [H+] = 1.0 x 10-7 and [ OH-]= 1.0 x 10-7?
Kw= (1.0 x 10-7) x (1.0 x 10-7)
Kw= 1.0 x 10-14

31. Ex. 6) What is the Kw if [H+] = 1.0 x 10-7 and [ OH-]= 1.0 x 10-7?
Kw= (1.0 x 10-7) x (1.0 x 10-7)
Kw= 1.0 x 10-14
This is a constant!
Kw always equals 1.0 x 10-14

32. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?

33. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
Kw= [H+][OH-]

34. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
Kw= [H+][OH-]
1.0 x = [H+][ 2.4 x 10-4]

35. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
Kw= [H+][OH-]
1.0 x = [H+][ 2.4 x 10-4]
[H+] = 1.0 x 10-14/ 2.4 x 10-4

36. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
Kw= [H+][OH-]
1.0 x = [H+][ 2.4 x 10-4]
[H+] = 1.0 x 10-14/ 2.4 x 10-4
[H+] = 4.2 x M

37. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
[H+] = 4.2 x 10-11
pH = -log(4.2 x 10-11)
= 10.38
= Basic solution

38. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
[H+] vs [OH-]
4.2 x 10-11M vs x 10-4 M

39. Ex. 7) The OH- concentration of an unknown solution is 2. 4 x 10-4
Ex. 7) The OH- concentration of an unknown solution is 2.4 x What is the H+ concentration of the solution? Is the unknown solution acidic, basic, or neutral?
[H+] vs [OH-]
4.2 x 10-11M vs x 10-4 M
[OH-] is larger so the solution is Basic

40. Finding [H3O+] You can use pH to find the [H3O+]
[H3O+] = 10^-pH OR [H+] = 10^-pH
Ex. 8) Find [H3O+] if pH = 4.720

41. Finding [H3O+]
Ex. 8) Find [H3O+] if pH = [H3O+] = 10^-pH [H3O+] = 10^-4.720

42. Finding [H3O+]
Ex. 8) Find [H3O+] if pH = [H3O+] = 10^-pH [H3O+] = 10^ [H3O+] = 1.91 x 10-5 M

43. Solving for OH- You can also substitute OH- in the place of H3O+.
pOH = -log[OH-] or [OH-] = 10^-pOH
Ex. 9) Find the pOH when [OH-] = x 10-8M

44. Solving for OH-
Ex. 9) Find the pOH when [OH-] = x 10-8M pOH = -log[OH-] pOH = -log (2.700 x 10-8)

45. Solving for OH-
Ex. 9) Find the pOH when [OH-] = x 10-8M pOH = -log[OH-] pOH = -log (2.700 x 10-8) pOH =

46. Ex. 10) Find [OH-] if pOH = 5.77

47. Ex. 10) Find [OH-] if pOH = 5.77
[OH-] = 10^-pOH
[OH-] = 10^-5.77

48. Ex. 10) Find [OH-] if pOH = 5.77
[OH-] = 10^-pOH
[OH-] = 10^-5.77
[OH-] = 1.7 x 10-6 M

49. Formulas To find either pH or pOH when given the other one
pH + pOH = 14
To find pH given hydrogen ion concentration pH= -log [H+] (or pH= -log [H3O+])
To find hydrogen ion or hydroxide ion concentration when given the other one
Kw = [H+][ OH-] Kw= 1.0 x 10-14
To find hydrogen ion concentration when given pH
[H3O+] = 10^-pH
To find pOH when given hydroxide concentration
pOH = -log[OH-]
To find hydroxide ion concentration when given pOH
[OH-] = 10^-pOH

50. Using Google, Define and give examples
Acids:
Bases:

51. Acid Base Reactions HA + BOH → HOH + B+A-
Acid + Base = neutralization reaction
Acid + Base → water + salt (usually)
Salt = (+) ion from base & (-) ion from acid
Positive ions are always listed first

52. Arrhenius
Swedish Chemist Svante Arrhenius created a model for acids and bases in 1883.
acids are anything that generate H+ in aqueous solutions, while bases produce OH- in aqueous solutions

53. Arrhenius Model- Acid H+ (aq) + Cl- (aq) HCl (g)
Acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution.

54. Arrhenius Model- Base NaOH (s) Na+(aq) + OH- (aq)
Base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution.
NaOH (s)
Na+(aq) + OH- (aq)

55. Bronsted- Lowry Model
Danish chemist Bronsted and English chemist Lowry proposed a model that focuses on the Hydrogen Ion
An Acid is a hydrogen-ion donor
A Base is a hydrogen-ion acceptor

56. Bronsted-Lowry Acid-Base Theory
weak acids have strong conjugate bases
weak bases have strong conjugate acids
primary reason they are weak acids or bases: strong conjugates recombine to form the original species
Water can be either an acid or base in Bronsted-Lowry theory
It is both amphiprotic and amphoteric
amphiprotic ~ can donate or accept a proton
amphoteric ~ a substance that can be either an acid or a base. 12 13

57. Ionization
The Bronsted-Lowry Model also shows if and acid or base is strong based on ionization.
Strong acid- completely ionized
Weak acid- partial ionization
aqueous solutions of strong acids, weak acids, strong bases, and weak bases conduct electricity

58. Differences between Arrhenius & Bronsted-Lowry theories
Reaction does not have to occur in an aqueous solution
bases do not have to be hydroxides ~ ammonia is not a hydroxide

59. Strength and Concentration
Strength – how completely it ionizes
Strong – ionizes completely or almost completely
Weak – ionizes partly
Concentration
Concentrated - a lot of acid/base in water.
Dilute – a little acid/base in water.

60. 12 M HCl is a strong acid with a high concentration
Adding 6L of water to this solution would do what to the solution: strong acid, dilute solution
Vinegar has acetic acid, which is weak, in low concentration = dilute
12 M acetic acid would still be weak, because it only partially ionizes, but it would be a concentrated solution, because there is a lot of acid dissolved in a little water.

61. List of Strong Acids and Bases
strong acids - ionize 100% in water
HCl, HBr, HI, H2SO4, HNO3, HClO4, HClO3
strong bases - ionize 100% in water
LiOH, NaOH, KOH, RbOH, CsOH, (all Group 1A)
Ca(OH)2, Sr(OH)2, Ba(OH)2, Ra(OH)2 (some from Group 2A)

62. Strong Acids
Since strong acids are completely ionized they produce the maximum number of ions.
Strong acids are good conductors
Reaction only moves in one direction, represented with an arrow in one direction.

63. HCl H Cl-
HBr H Br –
H2SO4 H HSO4 -

64. Weak Acids An acid that ionizes partially in dilute aqueous solutions
Produce fewer ions, so they are poor conductors
Reactions move both directions until equilibrium is reached, represented by an arrow in both directions

65. HF H+ + F-
H2S H+ + HS-
H2CO3 H+ + HCO3-

66. Conjugate Acid Conjugate Base
The species produced when a base accepts a hydrogen ion to form an acid
Conjugate Base
The species that results when an acid donates a hydrogen ion to form a base.

67. Conjugate acid – base pairs
2 compounds with the same chemical formula, but the acid of the pair will have
1 more H
NH3 & NH4 +
H2SO4 & HSO4-
H2O & H3O+

68. NH3 + H2O NH4+ + OH- Bronsted-Lowry Model Conjugate aCID aCID bASE

69. Identify the acid, base, conj. acid & conj. base.
Ex. 11) HNO3 + H2O  NO H3O+
Ex. 12) NH3 + HBr ↔ Br NH4+

70. Identify the acid, base, conj. acid & conj. base.
Ex. 11) HNO3 + H2O  NO H3O+
Acid Base CB CA
Ex. 12) NH3 + HBr ↔ Br NH4+

71. Identify the Acid, Base, Conj. Acid & Conj. Base
Ex. 11) HNO3 + H2O  NO H3O+
Acid Base CB CA
Ex. 12) NH3 + HBr ↔ Br NH4+
Base Acid CB CA

72. Titration
Use known solution (standard solution) to find the concentration of an unknown solution
Drop by drop process
Endpoint – point of color change of indicator
When neutralized
Equivalence point: where the 2 solutions in a titration are present in chemically equivalent amounts

73. Think back to the Indicator lab…which one would you consider the best indictor of acids and bases?

74. Universal Indicator
Changes colors at almost every pH!

75. Steps to solving titration problems
1st Write a balanced equation 2nd Write down all given information, including what you are looking for 3rd Plug data into the Titration equation and then solve for the unknown MAVA = MBVB nA nB M = Molarity V= Volume n = number of moles from the mole ratios in the balanced equation. A = acid B = base

76. Ex. 13) In a titration, L of M barium hydroxide is added to L of hydrochloric acid. What is the molarity of the acid?
Ex. 14) By titration, a M sulfuric acid solution is neutralized by 27.4 mL of M lithium hydroxide solution. What volume of sulfuric acid did you begin with?

77. Buffers Resist changes or swings in pH Blood pH approx 7.4
Fatal if fall or rise more than 0.3 pH units
Buffers in your blood prevent big changes when, for example, you eat a orange (citric acid)

78. Precipitate Reactions
When two compounds come together to form an aqueous compound and a solid compound. (Double replacement rxns)
2NaOH(aq) +CuCl2(aq) 2NaCl(aq) +Cu(OH)2(s)
KI(aq) + AgNO3(aq)KNO3(aq) + AgI(s)
Use your dissociation table to check solubility
If insoluble – compound will precipitate or settle out of solution as a solid

79. Oxidation-Reduction Reaction
A reaction in which electrons are transferred from one atom to another
(All single replacement, combustion, synthesis, and decomposition rxns)
2KBr(aq) + Cl2(aq)  2KCl(aq) + Br2(aq)
The chlorine on the left steals electrons from the bromine in KBr to become KCl and Br2 on the right.

80. Oxidation- Reductions Reaction

81. Remember Acid-Base Reaction
Form SALT + WATER
(Double replacement rxns)
Mg(OH)2 + 2HCl  MgCl2 + H20
base acid  salt water
Salt = any ionic compound made up of a cation (+) from a base and an anion (-) from an acid

82. Identify the following reaction: as 1) precipitation, 2) oxidation-reduction, or 3)acid-base
2K + Br2  2KBr
H3N + 3CsOH  Cs3N + 3H2O
MgCl2 + Li2CO3  MgCO3 + 2LiCl
Look on dissociation table to see if either compound is insoluble

83. Identify the following reaction: as 1) precipitation, 2) oxidation-reduction, or 3)acid-base
2K + Br2  2KBr
(oxidation-reduction)
H3N + 3CsOH  Cs3N + 3H2O
(acid-base)
MgCl2 + Li2CO3  MgCO3 (s)+ 2LiCl(aq)
(Precipitation)
Look on dissociation table to see if either compound is insoluble