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23 Cards in this Set
- Front
- Back
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Solute
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Stuff being dissolved
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Solvent
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Stuff doing the dissolving
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Saturation
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No more solute will dissolve into solvent
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Solubility
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Amount of solute that will saturate a particular solvent
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Molarity
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M, [x]
Moles Solute/Liters Solution Varies with temperature |
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Phase Solubility Rules
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(1) Solubility of solids in liquids increases with temperature
(2) Solubility of gases in liquids decreases with temperature (3) Solubility of gases in liquids increases with pressure |
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Molality
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m
moles solute/kg solvent Does not vary with temperature |
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Normality
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N
(# H ions that can participate in a reaction) * Molarity Does vary with temperature |
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Parts per million
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ppm
Mass solute/Mass solution * 10^6 |
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Van Hoff Factor
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i
Number of ions in solution i can NEVER be zero. |
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Electrolytes
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- Conduct electricity
- Can either be non, strong, or weak - Strongest electrolyte has the highest van-hoff factor |
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1 Liter is equal to x kg?
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1 kg or 1000g
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Solubility Rules
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(1) All Group I (Li, Na, K, Rb, Cs) and ammonium (NH₄) salts are soluable
(2) All Nitrate (NO₃), Perchlorate (ClO₄) and acetate (C₂H₃O₂) are soluble (3) Silver (Ag) Lead (Pb) and Mercury (Hg) salts are insoluble, EXCEPT for their nitrates, perchlorates, and acetates |
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What are Colligative Properties and what do they depend on? (4)
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NUMBER of molecules is important
- Vapor Pressure Depression - Boiling Point Elevation - Freezing Point Depression - Osmotic Pressure |
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Vapor Pressure
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- Pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid
- Had enough KE to escape liquid and go to gas - Think of IMF. Stronger IMF is harder to break, so lower VP |
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Volatile
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- Easily vaporized liquids
- Liquids with HIGH vapor pressure - Tend to have weaker IMF |
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Raoult's Law
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- Partial pressure of a subject equal to mole fraction in solution times the vapor pressure of pure subject
- Pa = X * Pure A |
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Vapor-Pressure Depression
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ΔVP = - Xb * Pa Pure
Change in VP is equal to the mole fraction of B times the partial pressure of the pure solvent |
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Boiling Point Elevation
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- When we add solute to solvent, we increase the boiling point, b/c tons of interaction between the solute + solvent, "anchoring" it.
- ΔT = k * i * m Where m is moLaLity. |
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Freezing Point Depression
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- Adding solute to a solvent disrupts the solid lattice.. makes it harder to freeze because of interaction
- ΔT = -k * i * m |
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Osmotic Pressure
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- Pressure to STOP osmosis from happening... resist it!
- π = MiRT So it's a pressure... units are what: atm, L, K, mol! R is 0.08! |
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Osmosis
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- Net movement of water across semipermeable membrane to areas of high [solute]
- Generally opposes diffusion |
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Diffusion
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- Movement of solute from high to low
- Generally opposes osmosis |
