316 E3

ndifranco94's version from 2015-09-03 19:36


Question Answer
True solutiona mixture of two or more components that form homogeneous molecular dispersion, or one phase system
Coarse dispersionsuspension of particles LARGER than 100 nm
Collodal dispersionsuspension of particles w/ size b/n true solution and coarse dispersion
Nonelectrolytessubstances that do not yield ions when dissolved in water; do not conduct electric current through the solution
Glucose electrolyte?nonelectrolyte
Aspirin electrolyte?weak electrolyte (acid)
Oxymetazoline hydrochlorine electrolyte?strong electrolyte (salt)
Molaritymol solute/Liter solution
Molalitymol solute/1000 g solvent
Why use Molality instead of Molarity?volume can change w/ tem, but MASS DOESNT
Ideal soln propertiesno changes in component props when solution is made, Enthalpy=0, no delV mixing, vapor pressure obeys Raoult's Law
Enthalpy of ideal soln?0
Volume of mixing of ideal soln?no change
Real solutionprops change when components are mixed, Ex. sulfuric acid + H2O
Raoult's Lawp = p*X
If mixture molecules interact more strongly than ideal soln?negative deviation, lower vapor pressure
If mixture molecules interact less strongly than ideal soln?positive deviation, higher vapor pressure
Colligative propsonly depend on the QUANTITY of solute molecules present, not chem nature or size
Colligative props listvapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure
Colligative props can only be used to measure MW inLOW CONCENTRATION solutions, bc they resemble ideal solns
Osmosismovement of solvent molecules through a membrane permeable only to the solvent molecule into a solution w/ higher solute conc
Osmotic pressurethe pressure that is applied to prevent the new flow of solvent molecules of a low solute conc soln through a membrane to a soln w/ higher solute conc
Osmotic pumps for drug delivery, push layer (high salt conc) and drug layer

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