1A + 2B 1C + 1DCalculate the equilibrium
concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. Kc = 2.0 x 10-10
1A + 2B 1C + 1DCalculate the equilibrium
concentrations of each species when a solution is
made with 1.0 M A & 1.0 M B. Kc = 2.0 x 10-12
Exp # [A] [B] [C] Rate1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0
Exp # [A] [B] [C] Rate1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0
([A4]/[A1])a = rate4/rate1
3a = 9; thus, a = 2
Exp # [A] [B] [C] Rate1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0
([B3]/[B2])b = rate3/rate2
2b = 8; thus b = 3
Exp # [A] [B] [C] Rate1) 27 C 0.10 0.10 0.10 4.0 2) 27 C 0.10 0.10 0.20 8.0 3) 27 C 0.10 0.20 0.20 64 4) 27 C 0.30 0.10 0.10 36 5)127 C 0.10 0.10 0.10 400.0
([C2]/[C1])c = rate2/rate1
2c = 2; thus c = 1
Rate = k[A]2[B]3[C]
Rate[A]2[B]3[C]k =
__N2 +__CO2 +__O2 __NO2 +__CO
__NO2 __N2O4
__N2O4 + __CO __NO +__CO2
__ NO + __ CO2 __ N2O5 + __ C
__N2O5 + __C __C2N2O5
__N2 +__CO2 +__O2 __NO2 +__CO
__NO2 __N2O4
__N2O4 + __CO __NO +__CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
__N2 +__CO2 +__O2 __NO2 +__CO
__NO2 __N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
__N2 +__CO2 +__O2 __NO2 +__CO
__NO2 __N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
__N2 +__CO2 +__O2 __NO2 +__CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
__N2 +__CO2 +__O2 __NO2 +__CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
2 N2 + 4 CO2 + 2 O2 4 NO2 + 4 CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
__N2O5 + __C __C2N2O5
2 N2 + 4 CO2 + 2 O2 4 NO2 + 4 CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C __N2O5 + __C __C2N2O5
2 N2 + 4 CO2 + 2 O2 4 NO2 + 4 CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C 2 N2O5 + 4 C 2 C2N2O5
2 N2 + 4 CO2 + 2 O2 4 NO2 + 4 CO
4 NO2 2 N2O4
2 N2O4 + 4 CO 4 NO +4 CO2
4 NO + 3 CO2 2 N2O5 + 3 C
2 N2 + 3 CO2 + 2 O2 2 N2O5 + 3 C 2 N2O5 + 1 4 C 2 C2N2O5
Acid/Base
Properties of Acids·Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts
Properties of Bases·Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts
Arrhenius·Acids: release H+ or H3O+ in solution
·Bases: release OH- in solution
Arrhenius·Acid: HA --> H+ + A- ·HCl --> H+ + Cl-
·Base: MOH --> M+ + OH-
·NaOH -->Na+ + OH-
Bronsted-Lowry·Acid: Proton donor ·Base: Proton Acceptor
Bronsted-Lowry· HA + H2O --> H3O+ + A-
· HI + H2O --> H3O+ + I- · Acid Base CA CB· NH3 + H2O --> NH4
+ + OH-
· Base Acid CA CB
Lewis Acid/Base·Acid: Electron Acceptor ·Base: Electron Donor
Lewis Acid/BaseH3N: + BF3 --> H3N-BF3
Base Acid Neutral
Drill:•List 3 properties
each of both acids & bases
Common Names· H+ Hydrogen ion· H3O+ Hydronium ion· H- Hydride ion· OH- Hydroxide ion· NH3 Ammonia
· NH4+ Ammonium ion
Amphoterism·Can act like an acid or a base
·Can donate or accept protons
Define acids & bases by each of
the three methods
Naming Acids· All acids are H-anion· If the anion is:· -ides hydro___ic acids· -ates ___ic acids· -ites ___ous acids
Naming Bases·Almost all bases are metal hydroxides
·Name by normal method·Ammonia (NH3) as well as many amines are bases
Drill: Name each of the following:
NaOH HIBa(OH)2 H2SO4
HMnO4 H3PO3
Strong Acids or Bases·Strong acids or bases ionize 100 % in solution
·Weak acids or bases ionize <100 % in solution
Strong Acids· HClO4 Perchloric acid
· H2SO4 Sulfuric acid
· HNO3 Nitric acid· HCl Hydrochloric acid· HBr Hydrobromic acid· HI Hydroiodic acid
Strong Bases· All column I hydroxides· Ca(OH)2 Calcium hydroxide
· Sr(OH)2 Strontium hydroxide
· Ba(OH)2 Barium hydroxide
Binary Acids·Acids containing only 2 elements
·HCl Hydrochloric acid·H2S Hydrosulfuric acid
Ternary Acids· Acids containing 3 elements
·H2SO4 Sulfuric acid
·H2SO3 Sulfurous acid
·HNO3 Nitric acid
Drill: Name & give the formula for at
least 4 each of strong acids & strong bases
Strong Acid/BaseIonizes 100 % (1 M) HA H+ + A-
1 M – all 1 1
Monoprotic Acids·Acids containing only one ionizable hydrogen
·HBr Hydrobromic acid·HCN Hydrocyanic acid·HC2H3O2 Acetic acid
Diprotic Acids·Acids containing 2 ionizable hydrogens
·H2SO4 Sulfuric acid
·H2SO3 Sulfurous acid
·H2CO3 Carbonic acid
Triprotic Acids·Acids containing 3 ionizable hydrogens
·H3PO4 Phosphoric acid
·H3PO3 Phosphorus acid
·H3AsO4 Arsenic acid
Polyprotic Acids· Acids containing more than one ionizable hydrogens
·H2SO4 Sulfuric acid
·H4SiO4 Silicic acid
·H2CO2 Carbonous acid
Monohydroxic Base·A base containing only one ionizable hydroxide
·NaOH Sodium hydroxide·KOH Potassium hydro.·LiOHLithium hydroxide
AP CHM HW•Read: Chapter 13•Problems: 1 - 3•Page: 395
CHM II HW•Read: Chapter 18•Problems: 3 & 5•Page: 787
Neutralization Rxn· A reaction between an acid
& a base making salt & H2O
·HA(aq) + MOH(aq) MA(aq) + H2O(l)
Neutralization Rxn
HCl(aq) + NaOH(aq)
NaCl(aq) + H2O(l)
Drill: Identify: acid, base, CA, & CB HCO3
- + H2O
H2CO3 + OH-
pH·The negative log of the hydrogen or hydronium ion concentration
·pH = -log[H+]·pOH = -log[OH-]
Calculate the pH of each of the following:1) [H+] = 0.040 M2) [HCl] = 0.0025 M 3) [HBr] = 0.080 M
Calculate the pOH of each of the following:
1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-12 M
AP CHM HW•Read Chapter 13•Work problems 17 & 19 on page 395
Standard Solution
·A solution with known
concentration
Titration· A method of determining the
concentration of one solution by reacting it with a standard solution
· MAVA = MBVB for monoprotics
Titration·When titrating acids against bases, the end point of the titration is at the equivalence point
Equivalence Point·The point where the H+
concentration is equal to the OH-
concentration
Titration No changes will be observed when titrating acids against bases; thus, one must use an indicator to see changes
Indicator·An organic dye that changes color when the pH changes
Drill:·Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH
Dilution Formula
M1V1 = M2V2
·Calculate the mL of 16.0 M HNO3 it takes
to make 4.0 L of 0.100 M HNO3
Make Calculations·Calculate the mL of 12.5 M HCl required
to make 2.5 L of 0.200 M HCl
Molarity·Moles of solute per
liter of solution (M)
Normality·Number of moles of hydrogen or hydroxide ions per liter of solution (N)
Titration Formula·NAVA = NBVB ·Elliott’s Rule:·#HMAVA = #OHMBVB
Make Calculations·Calculate the molarity of 30.0 mL H2CO3 when it’s titrated to its equivalence point with 75.0 mL 0.200 M NaOH
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
Calculate the volume of 0.250 M HCl
needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point
Calculate the molarity 25.0 mL H3PO4 that
neutralizes 50.00 mL 0.200 M Ca(OH)2 to its equivalence point
Drill: Calculate the volume of 0.10 M
H3PO4 that neutralizes 50.00 mL 0.200 M
Ca(OH)2 to its equivalence point
AP CHM HW•Read: Chapter 13•Problems: 7 & 9•Page: 395
CHM II HW•Read: Chapter 18•Problems: 27•Page: 787
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.
Drill: 3.2 g HI is dissolved in a
125 mL aqueous solution.
Calculate its pH.
Titration Curve:Strong acid vs
strong base
Titration Curve:Strong acid vs
strong base; then weak acid vs strong base
Titration Curve:Strong base vs
strong acid; then weak base vs strong acid