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Drill: Name & describe each of the 7 crystal structures. Drill: Draw LDDs for:. BF 3 NH 3 BeCl 3 C 3 H 6 H 3 PO 4 H 2 CO 3. Drill: Draw LDDs for:. C 6 H 8. Drill: Draw LDD for:. C 3 H 5 NO. CHM II. Test Friday. CHM II HW. Read: Chapter 14 Work Problems 25 & 29 on page 585.
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Drill: Draw LDDs for: BF3 NH3 BeCl3 C3H6 H3PO4 H2CO3
Drill: Draw LDD for: C3H5NO
CHM II • Test Friday
CHM II HW • Read: Chapter 14 • Work Problems 25 & 29 on page 585
Solution • Homogeneous mixture made up of at least one solute dissolved in the solvent
Solute • Substance being dissolved • Portion in lesser molar amount
Solvent • Substance doing the dissolving • Portion in greatest molar amount
Colloid • Slightly larger particles • Light passes & particles stay suspended
Suspension • Even larger particles • Particles block or reflect light
Tyndall Effect • Because light reflects off suspended particles, the light ray can be seen from the side
Size Comparison • Solution < Colloid • Colloid < Suspension
Soluble • When one substance (solute) dissolves in another (solvent)
Solubility • The amount of one substance (solute) dissolved in another (solvent)
Concentration • The amount of solute dissolved into solution
ConcentratedSolution • A solution with a relatively large amount of solute dissolved
Dilute Solution • A solution with a relatively small amount of solute dissolved
Saturated Solution • A solution with the maximum amount of solute dissolved in the solution
Unsaturated Solution • A solution with less than the maximum amount of solute dissolved in solution
Supersaturated Solution • A solution with greater than the maximum amount of solute dissolved in solution
Solution Measures • Concentration • Molarity • Molality • Mole Fraction
Percent Solution • Mass of one portion per the total mass, all times 100 % • %soln = ma/mtotal x 100 %
Drill: • Define & give units for: • Molarity • Molality • Mole Fraction
Molarity • Moles of solute per liter of solution • M = molessolute/Lsoln
Molality • Moles of solute per kilogram of solvent • mo = molessolute/kgsolvent
Mole Fraction • Moles of one portion per total number of moles in the solution • X = molesa/molessoln
Calculate the molarity of a 250 mL solution containing 5.0 g NaOH dissolved in water
Calculate the molality of 69 g of C2H5OH dissolved in 500.0 mL of water
Calculate the mole fraction of each portion when 92 g of C2H5OH dissolved in 144 mL of water
Drill: • Calculate the mass of KI required to make 250 mL of 0.500 M KI.
Calculate the molality & mole fraction of a solution containing 46 g of C2H5OH dissolved in 1782 mL of water
Chm II HW Problems: 31 & 38 Page: 585 & 586
AP Chm HW Problems: 31 & 35 Page: 298
Colligative Properties • Properties dependent only on the concentration of particles in solution
Examples • Vapor pressure • Boiling & Freezing points • Osmotic pressure
Vapor Pressure • VPsolution = (VPsolvent)(Xsolvent) • X = mole fraction • VP = vapor pressure
Boiling & Freezing DT = imoK DT = change in BP or FP i = ionic activity K = BP or FP constant
Osmotic Pressure p = iMRT p = osmotic pressure i = ionic activity M = Molarity
Calculate the vapor pressure of a solution containing 150 g C5H10O5 in 162 mL of water at 30oC
Drill: • Calculate the VP of a solution containing 36 % m/m glucose (C6H12O6) in water at 29oC: • (VPwater = 30.0 mm Hg)
Calculate BP & FP of 60.0 g of NaOH in 250 mL waterKBP = 0.512oC/moKFP = -1.86oC/mo
Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 250 mL solution at 27oC
Chm II Homework: Problems: 47 & 87 Page: 585 - 587
AP Chm HW: Problems: 31, 35, & 39 Page: 298
Calculate the vapor pressure of a solution containing 120 g C3H7OH in 144 mL of water at its BP.