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