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AP Chemistry. Chapter 13 Solutions. 13.1. Solvation- solvent part surround solute part. Hydration- when solvent is water Process in which the NRG content ↑ tend to occur spontaneously. Process in which the disorder of the system increases tend to occur spontaneously. 13.2.
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AP Chemistry Chapter 13 Solutions
13.1 Solvation- solvent part surround solute part. Hydration- when solvent is water Process in which the NRG content ↑ tend to occur spontaneously. Process in which the disorder of the system increases tend to occur spontaneously.
13.2 Solute+solventcrystallizedissolvesolution Saturated Unsaturated Supersaturated Solubility = grams dissolved per 100g H2O
13.3 Factors Affecting Solubility • Temp solids ↑ temp. ↑sol. gas ↑ temp. ↓sol. 1. Miscible- mutually sol. 2. Immiscible- insol. B. Type of solvent P/NP C. Stirring D. Pressure (gas only)
…Continue 13.3 1. Henry’s Law sol. & pressure (directly proportional) Cg = kP(g) E. Particle Size (surface area)
13.4 Ways to Express Conc. • Mass % = mass x 100 mass total B. ppm- parts per million C. ppb- parts per billion D. Molarity= M=moles of solute liters of solution E. Molality= m= mole of solute Kg of solvent F. Mole fraction= X= moles total moles
13.5 Colligative Properties Colligative Properties- depend on amount of solute, not what kind. • Vapor Pressure- lowered 1. Raoult’s Law= PA=XAPA˚ 2. Ideal solution – obeys Raoult’s Law B. Boiling Point ↑ 1. ∆T = Kb x m Kb = molal boiling pt. Elevation constant. = .52˚C/m = .512˚/m
…Continue 13.5 C. Freezing Point ↓ 1.) ∆T = Kf x m Kf = molal freezing pt. Depression constant = 1.86˚C/m Sample 13.8, 13.4 Van’t Hoff factor. 2.) NaCl Na+ + Cl- x 2 CaCl2 Ca+2 + 2Cl- x 3 AlCl3 Al+3 + 3Cl- x 4
Jacobus Henricus van 't Hoff Won Nobel Prize in 1901 Van’t Hoff factor
…Continue 13.5 D. Osmotic pressure- π 1. π= MRT = (mol/L)RT PV= nRT 2. Osmosis- diffusion through a semipermeable membrane 3. Net movement of solvent is always toward the soln. w/ higher solute conc. 4. Isotonic - =conc. 5. Hypotonic – lower ost. Pressure 6. Hypertonic – more conc. Soln.
…Continue 13.5 II. Calculate Molecular Weight **N.B. Sample 13.11 pg. 494 ∆ T = Kbm .357˚ = (5.02˚/m) m m= .0711m MW= g1 1000 = (.250g)(1000)= 88.0 g/mol g2 m (40.0g)(.0711) g1= solute g2= solvent m= molality
3.6 Colloids 1. Hydrophilic (water loving) 2. Hydrophobic (water fearing)