Acid/Base

1
1A 1B ?? 1C 1DCalculate the equilibrium
concentrations of each species when 150 ml 2.0 M
A is mixed with 100.0 ml 2.0 M B. Kc 0.25
2
Acid/Base
3
Properties of Acids

• Sour taste, Change color of dyes, Conduct
  electricity in solution, React with many metals,
  React with bases to form salts

4
Properties of Bases

• Bitter taste, Feel slippery, Change color of
  dyes, Conduct electricity in solution, React with
  acids to form salts

5
Arrhenius

• Acids release H or H3O in solution
• Bases release OH- in solution

6
Arrhenius

• Acid HA --gt H A-
• HCl --gt H Cl-
• Base MOH --gt M OH-
• NaOH --gtNa OH-

7
Bronsted-Lowry

• Acid Proton donor
• Base Proton
• Acceptor

8
Bronsted-Lowry

• HA H2O --gt H3O A-
• HI H2O --gt H3O I-
• Acid Base CA CB
• NH3 H2O --gt NH4 OH-
• Base Acid CA CB

9
Lewis Acid/Base

• Acid Electron
• Acceptor
• Base Electron Donor

10
Lewis Acid/Base
H3N BF3 --gt H3N-BF3 Base Acid Neutral
11
Drill

• List 3 properties each of both acids bases

12
Common Names

• H Hydrogen ion
• H3O Hydronium ion
• H- Hydride ion
• OH- Hydroxide ion
• NH3 Ammonia
• NH4 Ammonium ion

13
Amphoterism

• Can act like an acid or a base
• Can donate or accept protons

14
Define acids bases by each of the three methods
15
Naming Acids

• All acids are H-anion
• If the anion is
• -ides ? hydro___ic acids
• -ates ? ___ic acids
• -ites ? ___ous acids

16
Naming Bases

• Almost all bases are metal hydroxides
• Name by normal method
• Ammonia (NH3) as well as many amines are bases

17
Strong Acids or Bases

• Strong acids or bases ionize 100 in solution
• Weak acids or bases ionize lt100 in solution

18
Strong Acids

• HClO4 Perchloric acid
• H2SO4 Sulfuric acid
• HNO3 Nitric acid
• HCl Hydrochloric acid
• HBr Hydrobromic acid
• HI Hydroiodic acid

19
Strong Bases

• All column I hydroxides
• Ca(OH)2 Calcium hydroxide
• Sr(OH)2 Strontium hydroxide
• Ba(OH)2 Barium hydroxide

20
Binary Acids

• Acids containing only 2 elements
• HCl Hydrochloric acid
• H2S Hydrosulfuric acid

21
Ternary Acids

• Acids containing 3 elements
• H2SO4 Sulfuric acid
• H2SO3 Sulfurous acid
• HNO3 Nitric acid

22
Drill Name give the formula for at least 4
each of strong acids strong bases
23
Strong Acid/Base

• Ionizes 100 (1 M)
• HA H A-
• 1 M all 1 1

24
Monoprotic Acids

• Acids containing only one ionizable hydrogen
• HBr Hydrobromic acid
• HCN Hydrocyanic acid
• HC2H3O2 Acetic acid

25
Diprotic Acids

• Acids containing 2 ionizable hydrogens
• H2SO4 Sulfuric acid
• H2SO3 Sulfurous acid
• H2CO3 Carbonic acid

26
Triprotic Acids

• Acids containing 3 ionizable hydrogens
• H3PO4 Phosphoric acid
• H3PO3 Phosphorus acid
• H3AsO4 Arsenic acid

27
Polyprotic Acids

• Acids containing more than one ionizable
  hydrogens
• H2SO4 Sulfuric acid
• H4SiO4 Silicic acid
• H2CO2 Carbonous acid

28
Monohydroxic Base

• A base containing only one ionizable hydroxide
• NaOH Sodium hydroxide
• KOH Potassium hydro.
• LiOH Lithium hydroxide

29
AP CHM HW

• Read Chapter 13
• Problems 17 19
• Page 395

30
CHM II HW

• Read Chapter 18
• Problems 3 5
• Page 787

31
Neutralization Rxn

• A reaction between an acid a base making salt
  H2O
• HA(aq) MOH(aq)
• ? MA(aq) H2O(l)

32
Neutralization Rxn

• HCl(aq) NaOH(aq)
• ?
• NaCl(aq) H2O(l)

33
Drill Identify acid, base, CA, CB

• HCO3- H2O
• H2CO3 OH-

34
Titration

• A method of determining the concentration of one
  solution by reacting it with a standard solution
• MAVA MBVB for monoprotics

35
Work problems 1 6 on page 395
36
Standard Solution

• A solution with known concentration

37
Titration

• When titrating acids against bases, the end point
  of the titration is at the equivalence point

38
Equivalence Point

• The point where the H concentration is equal to
  the OH- concentration

39
Titration
No changes will be observed when titrating acids
against bases thus, one must use an indicator to
see changes
40
Indicator

• An organic dye that changes color when the pH
  changes

41
Make Calculations

• Calculate the molarity of 25.0 mL HCl when its
  titrated to its equivalence point with 50.0 mL
  0.200 M NaOH

42
Make Calculations

• Calculate the mL of 12.5 M HCl required to make
  2.5 L of 0.200 M HCl

43
Drill

• Calculate the mL of 16.0 M HNO3 it takes to make
  4.0 L of 0.100 M HNO3

44
Molarity

• Moles of solute per liter of solution (M)

45
Normality

• Number of moles of hydrogen or hydroxide ions per
  liter of solution (N)

46
Titration Formula

• NAVA NBVB
• Elliotts Rule
• HMAVA OHMBVB

47
Make Calculations

• Calculate the molarity of 30.0 mL H2CO3 when its
  titrated to its equivalence point with 75.0 mL
  0.200 M NaOH

48
Make Calculations

• Calculate the molarity of 40.0 mL H3PO4 when its
  titrated to its equivalence point with 30.0 mL
  0.20 M Ba(OH)2

49
Calculate the volume of 0.250 M HCl needed to
titrate 50.00 mL 0.200 M NaOH to its equivalence
point
50
Calculate the molarity 25.0 mL H3PO4 that
neutralizes 50.00 mL 0.200 M Ca(OH)2 to its
equivalence point
51
Drill Calculate the volume of 0.10 M H3PO4 that
neutralizes 50.00 mL 0.200 M Ca(OH)2 to its
equivalence point
52
pH

• The negative log of the hydrogen or hydronium ion
  concentration
• pH -logH
• pOH -logOH-

53
Calculate the pH of each of the following1)
HCl 0.0025 M 2) H 0.040 M3) HBr
0.080 M
54
Calculate the pOH of each of the following 1)
OH- 0.030 M2) KOH 0.0025 M3) NaOH
4.0 x 10-12 M
55
AP CHM HW

• Read Chapter 13
• Problems 7 9
• Page 395

56
CHM II HW

• Read Chapter 18
• Problems 27
• Page 787

57
Drill Calculate the molarity of 25.00 mL of
H3PO4 that was titrated to its equivalence point
with 75.00 mL of0.125 M Ba(OH)2.
58
Titration CurveStrong acid vs strong base
59
(No Transcript)
60
Titration CurveStrong acid vs strong base then
weak acid vs strong base
61
(No Transcript)
62
(No Transcript)
63
Titration CurveStrong base vs strong acid then
weak base vs strong acid
64
(No Transcript)