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 solids

dissolved in liquids In other types

Solute is substance in _____________ amountSolute is the substance that was a different _____ than

the resulting solution

Similar MixturesColloids

____________ appearance____________ particle size

Particles will not settle Particles will disperse light

(tyndall effect)For example: Foam, fog,

milkSuspensions

__________ appearance________ particle size

Particles 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 liquid-liquid and

solid-liquid 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 immiscible

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 SolutionElectrolytes

Compound broken into _____ when dissolves

Solution can carry electrical current

NonelectrolytesIMF’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 covalently bonded compound into ionsIons spread throughout solutions

DissociationBreaks 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 i = ____

C12H22O12 (s) C12H22O12 (aq) * 1 particle i = ___

Electrolytes i = # of ions created from ionization or dissociationNaCl (s) Na+

(aq) + Cl-(aq) * 2 particles i = ___

MgCl2 (s) Mg+2(aq) + 2 Cl-(aq) * 3 particles i

= ___

SolvationProcess of ___________Also called hydration when solvent is

_________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 increasing temperature increases 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

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 lower

than vapor pressure of 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