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