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1A + 1B  1C + 1D Calculate 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.

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Presentation on theme: "1A + 1B  1C + 1D Calculate 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."— Presentation transcript:

1 1A + 1B  1C + 1D Calculate the equilibrium concentrations of each species when 150 ml 2.0 M A is mixed with 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 --> H+ + A- HCl --> H+ + Cl-
Base: MOH --> M+ + OH- NaOH -->Na+ + OH-

7 Bronsted-Lowry Acid: Proton donor Base: Proton Acceptor

8 Bronsted-Lowry HA + H2O --> H3O+ + A- HI + H2O --> H3O+ + I-
Acid Base CA CB NH3 + H2O --> NH4+ + OH- Base Acid CA CB

9 Lewis Acid/Base Acid: Electron Acceptor Base: Electron Donor

10 Lewis Acid/Base H3N: + BF3 --> H3N-BF3 Base Acid Neutral

11 List 3 properties each of both acids & bases
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 <100 % 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 H2SO4 Sulfuric acid H2SO3 Sulfurous acid
Acids containing 3 elements H2SO4 Sulfuric acid H2SO3 Sulfurous acid HNO3 Nitric acid

22 Drill: Name & give the formula for at least 4 strong acids & strong bases

23 Strong Acid/Base Ionizes 100 % (1 M) HA H+ + A- 1 M – all

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 H2SO4 Sulfuric acid H4SiO4 Silicic acid
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 HA(aq) + MOH(aq)  MA(aq) + H2O(l)
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 A solution with known concentration
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 The point where the H+ concentration is equal to the OH- concentration
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 it’s titrated to its equivalence point with 50.0 mL M NaOH

42 Calculate the mL of 12.5 M HCl required to make 2.5 L of 0.200 M HCl
Make Calculations Calculate the mL of 12.5 M HCl required to make 2.5 L of M HCl

43 Calculate the mL of 16.0 M HNO3 it takes to make 4.0 L of 0.100 M HNO3
Drill: Calculate the mL of 16.0 M HNO3 it takes to make 4.0 L of M HNO3

44 Moles of solute per liter of solution (M)
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 Elliott’s Rule: #HMAVA = #OHMBVB

47 Make Calculations Calculate the molarity of 30.0 mL H2CO3 when it’s titrated to its equivalence point with 75.0 mL M NaOH

48 Make Calculations Calculate the molarity of 40.0 mL H3PO4 when it’s 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
Calculate the volume of M HCl needed to titrate mL M NaOH to its equivalence point

50 Calculate the molarity 25. 0 mL H3PO4 that neutralizes 50. 00 mL 0
Calculate the molarity 25.0 mL H3PO4 that neutralizes mL M Ca(OH)2 to its equivalence point

51 Drill: Calculate the volume of 0. 10 M H3PO4 that neutralizes 50
Drill: Calculate the volume of 0.10 M H3PO4 that neutralizes mL M Ca(OH)2 to its equivalence point

52 pH The negative log of the hydrogen or hydronium ion concentration
pH = -log[H+] pOH = -log[OH-]

53 Calculate the pH of each of the following: 1) [HCl] = 0
Calculate the pH of each of the following: 1) [HCl] = M 2) [H+] = M 3) [HBr] = M

54 Calculate the pOH of each of the following:
1) [OH-] = M 2) [KOH] = M 3) [NaOH] = 4.0 x 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
Drill: Calculate the molarity of mL of H3PO4 that was titrated to its equivalence point with mL of M Ba(OH)2.

58 Titration Curve: Strong acid vs strong base

59

60 Titration Curve: Strong acid vs strong base; then weak acid vs strong base

61

62

63 Titration Curve: Strong base vs strong acid; then weak base vs strong acid

64

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