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Transcript of Solutions
Solutions
Solutions_______________ mixturesOccur in each state of matter
Gas mixed in gas (________)Gas mixed in liquid (___________________)Liquid mixed in liquid (_______________)Solid mixed in liquid (______________)Solid mixed in solid (_________________________)
Composed of a solute mixed with solventTerms used most commonly with ______
dissolved in _______In other types
Solute is substance in ___________ amount______ is the substance that was a different phase
than the resulting solution
Similar Mixtures___________
Homogenous appearanceMedium particle size
Particles will not settle Particles will disperse light
(tyndall effect)For example: Foam, fog,
milk____________
Heterogeneous appearance
Large particle sizeParticles will settle over time
For example: Italian salad dressing
Solubility
Ability of a substance to dissolve within another substance Depends on ___________ being usedUsually ______ dissolves ________We often mean the solubility in ___________
solutionsReally only in question for ___________ and
____________ solutionsReally a question of _______________
dissolves
Gas-Gas Solutions
Mix freely with each other
Each gas acts on its own
Gas-Liquid SolutionsSolubility ______________ with higher partial
pressures of the gas over a liquidSolubility _____________ with increasing
temperature
Liquid-Liquid SolutionsSome liquids are
______________Insoluble in each otherDue to polarity of liquids
(usually non-polar with polar)Miscible liquids
Usually like with likePolar with polarNon-polar with non-polar
Solid-Solid SolutionsAlloys
ALLOY COMPONENT METALSBronze copper, tinBrass copper, zincSteel iron, carbon, (various other
metals)Sterling Silver silver, nickel, copper14K Gold gold, copper, antimonyPewter tin, copper, antimonySolder tin, lead
Solid-Liquid Solution_________________
Compound broken into ions when dissolves
Solution can carry electrical current
_________________IMF’s (but not
molecules) are broken when dissolves
No electrical current can be carried
Dissolving NonelectrolytesNon-polar molecules
Soluble in non-polar solventsInsoluble in polar solvents
Polar molecules (or molecules with polar sections)Soluble in polar solventsInsoluble in non-polar
solventsDo not break apart
______ mole of solid solute creates _____ mole of particles in solution
Dissolving ElectrolytesIonization
Breaks a _______ bonded compound into ionsIons spread throughout solutions
______________Breaks ions in ionic bond apartIons spread throughout solution
Both processes create more particles in solution than were present in the solid solute
V’ant Hoff FactorRepresented by ____Equals the number of particles created from
each solute when dissolvedNonelectrolytes ________
C12H22O12 (s) C12H22O12 (aq) * _______________
Electrolytes ________________ from ionization or dissociationNaCl (s) Na+
(aq) + Cl-(aq) * _________________MgCl2 (s) Mg+2
(aq) + Cl-(aq) * _________________
SolvationProcess of ____________Also called hydration when solvent in
_________Bonds or IMF’s between particles must be
brokenEnergy is absorbed
Solvent particles surround the solute particles and form new bonds or IMF’s Energy is released
SaturationAn amount of solvent can only hold a certain amount of
soluteAmount depends on ______________Amount also depends on ________________
Usually ____________ temperature _____________ solubility
________________ solutionAmount of solute is below the amount that the solvent can
hold_________________ solution
Amount of solute is at the amount that the solvent can hold_______________ solution
Amount of solute is above the amount that the solvent can hold
Not common, made by carefully cooling a saturated solution
Solubility CurvesGraph depicting the solubility of substances
at different temperatures
Concentrations of SolutionsComparison of amount of solute in a solvent_______________
Dilute- small amount of solute compared to solvent
Concentrated- large amount of solute ____________
MolarityMolalityppm, ppb, pptMole fractionMass %
MolarityMole/Volume
EquationMolarity (M) = moles of solute / liters of
solution (not solvent)* Amount must be in _____________* Volume must be in _____________
Changes with temperature
MolalityMole/Mass
EquationMolality (m) = moles of solute / mass of
solvent* Amount must be in ____________* Mass must be in ____________
Does not change with temperature
ppm, ppb, and pptMass/VolumeUsed for very __________ solutions
ppm = parts per million one part solute in a million parts solutionRoughly equal to one person in a large city
ppb = parts per billion one part solute in a billion parts solutionRoughly equal to one person in India
ppt = parts per trillionOne part solute in a trillion parts solution
Not exact terms but we will useppm = 1 mg/Lppb = 1 g/Lppt = 1 ng/L
Mole FractionMol/Mol
EquationMole Fraction () = moles of component /
moles of all componentsNo unitsAll of the mole fractions of a solution add up to
________
Mass PercentMass/Mass
EquationMass Percent = (mass of solute/ mass of
solution) x 100
Colligative PropertiesProperties of solutions that depend on the
__________ of solute particles not the __________ of the solute
Shift in PointsFreezing point _____________- solution freezes
at a lower temperature than the pure solventBoiling point ___________- solution boils at a
higher temperaure than the pure solventVapor PressureOsmotic Pressure
Vapor PressureVapor pressure of solvent in solution is _______
than vapor pressure of pure solventEquation
Psolv = solv P°solv
Psolv = pressure of solvent vapor over solutionsolv = mole fraction of solvent in solutionP°solv = pressure of solvent vapor over pure solvent
Variables in Point Shiftsm- Molality of solutioni- V’ant Hoff factorConstants
Kf
Specific to solvent Shows the affect of solute on that solvent’s freezing
pointKf for water is 1.86 °C kg/mol
Kb
Specific to solvent Shows the affect of solute on that solvent’s boiling pointKb for water is 0.512 °C kg/mol
Freezing Point DepressionEquation
ΔTf = iKf m
Gives change in freezing pointMust subtract from pure solvent’s freezing
point to find solution’s freezing point
Boiling Point ElevationEquation
ΔTb = iKb m
Gives change in boiling pointMust add to pure solvent’s boiling point to
find solution’s boiling point
Osmotic PressurePressure that must be applied in order to
stop __________
OsmosisMovement of water from an area of
____________ concentration to an area of ______________ concentration
Occurs across semipermeable membranes (cell membranes)
Calculating Osmotic Pressure = iMRT
= osmotic pressure (will have pressure units)
i = V’ant Hoff factor M = Molarity of solutionR = gas constant (0.08206 atm L mol-1 K-1)T = temperature in K