chemistry 102(01) spring 2012
DESCRIPTION
Chemistry 102(01) Spring 2012. CTH 328 9:30-10:45 am Instructor : Dr. Upali Siriwardane e-mail : [email protected] Office : CTH 311 Phone 257-4941 Office Hours : M,W 8:00-9:00 & 11:00-12:00 am; Tu,Th,F 8:00 - 10:00 am.. Exams: 9 :30-10:45 am, CTH 328. - PowerPoint PPT PresentationTRANSCRIPT
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15-1CHEM 102, Spring 2012 LA TECH
CTH 328 9:30-10:45 am
Instructor: Dr. Upali Siriwardane
e-mail: [email protected]
Office: CTH 311 Phone 257-4941
Office Hours: M,W 8:00-9:00 & 11:00-12:00 am;
Tu,Th,F 8:00 - 10:00 am..
Exams: 9:30-10:45 am, CTH 328.
March 26 , 2012 (Test 1): Chapter 13
April 18 , 2012 (Test 2): Chapter 14 &15
May 14 , 2012 (Test 3): Chapter 16 &18
Optional Comprehensive Final Exam: May 17, 2012 :
Chapters 13, 14, 15, 16, 17, and 18
Chemistry 102(01) Spring 2012
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15-2CHEM 102, Spring 2012 LA TECH
Chapter 15. The Chemistry of Solutes and Solutions 15.1 Solubility and Intermolecular Forces 15.2 Enthalpy, Entropy, and Dissolving Solids 15.3 Solubility and Equilibrium 15.4 Temperature and Solubility 15.5 Pressure and Dissolving Gases in Liquids:
Henry's Law15.6 Solution Concentration: Keeping Track of Units15.7 Vapor Pressures, Boiling Points, and Freezing Points
of Solutions15.8 Osmotic Pressure of Solutions15.9 Colloids 15.10 Surfactants15.11 Water: Natural, Clean, and Otherwise
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15-3CHEM 102, Spring 2012 LA TECH
Solution TerminologySoluteone or more substance(s) dispersed in the solution
Solventmajority substance in a solutionThe solubility of a solid in a solvent is typically given in
g/100 ml.
Types of solutionsMixture of GasesLiquid solutions (L+S,L+L,L+G)Solid solutions (S+S, alloys)Aerosols (L+G)Foam (S+G)
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15-4CHEM 102, Spring 2012 LA TECH
Miscible vs. Immiscible
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15-5CHEM 102, Spring 2012 LA TECH
“Likes Dissolve Likes”Materials with similar polarity are soluble in
each other. Dissimilar ones are not.Polar substances with similar forces are likely
to be soluble in each otherNon-polar solutes dissolve in non-polar
solventsstronger solute-solvent attractions favor
solubility, stronger solute-solute or solvent-solvent attractions reduce solubility
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15-6CHEM 102, Spring 2012 LA TECH
Solubility of Ionic Compounds and Temperature
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15-7CHEM 102, Spring 2012 LA TECH
Solution Terminology
Miscible - liquids that dissolve in each otherImmiscible - liquids that do not dissolve in each
other due to differences types of interactionsSaturated solutionA solution that contains as much it can hold Unsaturated solutionA solution that contains less than maximum
amountSupersaturated solution A solution that contains more than maximum
amount
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15-8CHEM 102, Spring 2012 LA TECH
Types of Solutions (Diluted, Saturated, and Supersaturated)
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15-9CHEM 102, Spring 2012 LA TECH
Supersaturated Solution
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15-10CHEM 102, Spring 2012 LA TECH
Solute - Solvent Interactions
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15-11CHEM 102, Spring 2012 LA TECH
The Solution Making Exopthermic Process
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15-12CHEM 102, Spring 2012 LA TECH
The Solution Making Endothermic Process
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15-13CHEM 102, Spring 2012 LA TECH
Thermodynamic Factors Affecting Solubility
1. Energy: Enthalpy (DH) Lower energy – DH
2. Order: Entropy (DS) Disorder + DS
Exothermic –DH favors solubility: product favored
Mixing (+DS disorder favors solubility: product favored
Gibbs Free Energy: (Chapter 18)
DGsoln = DHsoln -TDSsoln,
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15-14CHEM 102, Spring 2012 LA TECH
Types of Solute - Solvent Interactions
All interactions are electrostatic force
~ Coulombic: proprotional to charge and séparation)
1. London Dispersion Forces: (O2 dissolved in Liq. N2)
2. Ion-Ion Interaction: (Ionic liquids in batteries)
3. Ion-Dipole Interaction (hydrated ions Na+
(aq))
4. Dipole-Dipole Interaction (CCl4 in benzene (C6H6)
5. Hydrogen Bonding. (water and éthanol)
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15-15CHEM 102, Spring 2012 LA TECH
1) What are the main factors affecting a solubility of a solute in a solvent?
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15-16CHEM 102, Spring 2012 LA TECH
The Solution Making Exopthermic Process
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15-17CHEM 102, Spring 2012 LA TECH
The Solution Making Endothermic Process
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15-18CHEM 102, Spring 2012 LA TECH
2) Arrange the following inter-particles forces in liquids and solids in the order of increasing strength:
• ion-ion, • ion-dipole, • hydrogen bond, • dipole-dipole and • London dispersion
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15-19CHEM 102, Spring 2012 LA TECH
3) Identify the most important type of inter-particle force for each of the following compounds:
a) NaCl(s) or NaCl(l) b) N2(l) or N2(s) c) N2(g) d) Na(s) and Na(l)
e) H2O(l) or H2O(s) f) CH3CH2OH(l) or CH3CH2OH(s)
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15-20CHEM 102, Spring 2012 LA TECH
4) Which of the above inter-particle force could be named as intermolecular force?
a) NaCl(s) or NaCl(l) b) N2(l) or N2(s) c) N2(g) d) Na(s) and Na(l)
e) H2O(l) or H2O(s) f) CH3CH2OH(l) or CH3CH2OH(s)
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15-21CHEM 102, Spring 2012 LA TECH
Acetic acid
HC2H3O2
CH3COOH
Hexanol
C6H13OHHexane
C6H14
Propanoic acid
C2H5COOH
“Like Dissolves Like”
Identify Hydrogen Bonding, Polar and Non-polar groups in Covalent Molecules
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15-22CHEM 102, Spring 2012 LA TECH
5) What types of inter-particle forces solute-solute:DH1, solvent-solvent: DH2, solvent-solute:DH3) are involved when a) CH3CH2OH(l): dissolved in water,H2O:DH1 = ; DH2 = ; DH3= For covalent compounds: DHsoln= DH1+ DH2+ DH3
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15-23CHEM 102, Spring 2012 LA TECH
Water Dissolving An Ionic Solute
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15-24CHEM 102, Spring 2012 LA TECH
Solution Process of Ionic Compounds
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15-25CHEM 102, Spring 2012 LA TECH
Hydration of a Sodium Ion
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15-26CHEM 102, Spring 2012 LA TECH
Heats of Solution
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15-27CHEM 102, Spring 2012 LA TECH
4) b) Na2SO4(s) dissolved in water:DH1 = ; DH2 = ; DH3 = Ion-ion inter-particle forces in solids are called
Lattice Energy. ( this is related to DH1)Ion-water inter-particle forces are called Hydration
Energy (this is related to DH2 and DH3) For ionic compounds; DHsoln = DHlattice + DHhyd
Qualitatively speaking which of the above a) or b) would have a more exothermic DHsoln?
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15-28CHEM 102, Spring 2012 LA TECH
4) What factors make it more exothermic? a) CH3CH2OH in H2O DH1 = ; DH2 = ; DH3=
b) Na2SO4(s) dissolved in water: (DH1 = DHsoln)+ (Hhyd= DH2+ DH3)
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15-29CHEM 102, Spring 2012 LA TECH
5) Assign the entropy (most +, medium + or least +) for i) S1 –solute: ii) S2-solvent:iii) S3, solution (solvent-solute):
For the following: (Indicate which one is highest, intermediate and lowest order) For
a) CH3CH2OH(l): dissolved in water: S1 = ; S2 = ;S3= Na2SO4(s) dissolved in water: S1 = ; S2 = ;S3 =
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15-30CHEM 102, Spring 2012 LA TECH
5) Qualitatively speaking which of the above a) or b) would have a more positive DSsoln?
a) CH3CH2OH(l): dissolved in water: S1 = ; S2 = ;S3= b) For Na2SO4(s) dissolved in water: S1 = ; S2 = ;S3 =
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15-31CHEM 102, Spring 2012 LA TECH
6) Calculate the DHsoln for dissolving CaCl2(s) in water given the Lattice-Energy CaCl2(s) = +2258 kJ/mole), and Hydration energy for CaCl2 = - 2205 kJ/mole (DHsoln = DHlattice + DHhyd =?)
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15-32CHEM 102, Spring 2012 LA TECH
7) DHsoln value thermodynamically product favored?
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15-33CHEM 102, Spring 2012 LA TECH
8) For dissolving CaCl2(s) in water, which of the following entropy represent the highest order? Explain.a) S for CaCl2(s): +104.6 J/mole
b) S for H2O(l): +69.91 J/mole
c) S for solution CaCl2(aq): +815 J/mole
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15-34CHEM 102, Spring 2012 LA TECH
9) Calculate the DSsoln for dissolving CaCl2(s) in water given the entropies of Lattice- CaCl2(s) (S1= +104.6 J/mole), H2O(l)(S2 = +69.91 J/mole); CaCl2(aq)(S3 = +815 J/mole).
DSsoln= Sfinal-Sinitial =S3 - ( S1+ S2)?
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15-35CHEM 102, Spring 2012 LA TECH
10) Calculate the DSsoln for dissolving CaCl2(s) in water given the entropies of Lattice- CaCl2(s) (S1= +104.6 J/mole), H2O(l)(S2 = +69.91 J/mole); CaCl2(aq)(S3 = +815 J/mole).
DSsoln= Sfinal-Sinitial =S3 - ( S1+ S2)?
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15-36CHEM 102, Spring 2012 LA TECH
11) DSsoln value thermodynamically product favored?
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15-37CHEM 102, Spring 2012 LA TECH
12) Based on DGsoln, determine if CaCl2 is soluble at 25C, given,
DGsoln = DHsoln -TDSsoln, and DHsoln and DSsoln calculated above.
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15-38CHEM 102, Spring 2012 LA TECH
13) Why sand is insoluble in both polar and nonpolar solvents?
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15-39CHEM 102, Spring 2012 LA TECH
14) How does temperature and pressure affect the solubility of following?
a) NH4NO3(solid) in water with +(positive) DHsoln:
b) CO2 gas in water:
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15-40CHEM 102, Spring 2012 LA TECH
Solubility of Oxygen in Water
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15-41CHEM 102, Spring 2012 LA TECH
Henry’s Law
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Henry’s LawSolubility of Gases in SolventsSg = kHPg
where Sg solubilitykH Henry’s Law constantPg partial pressure of gas
Increasing the pressure of a gas above a liquid increases its solubility
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15) Deep sea divers may experience a condition called the "bends" if they do not readjust slowly to the lower pressure at the surface. Using the diagram on pressure dependence solubility of gases on water explain this phenomenon.