Solutions
Solutions
 ____________ mixtures
 Occur in each state of matter
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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 solvent
 Terms used most commonly with solids dissolved in liquids
 In other types
 Solute is substance in _____________ amount
 Solute is the substance that was a different _____ than the resulting solution
Similar Mixtures
 Colloids
 ____________ appearance
 ____________ particle size
 Particles will not settle
 Particles will disperse light (tyndall
effect)
 For example: Foam, fog, milk
 Suspensions
 __________ 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 used
 Usually ______ dissolves _______
 We often mean the solubility in __________ solutions
 Really only in question for liquid-liquid and solid-liquid
solutions
 Really a question of _____________ dissolves
Gas-Gas Solutions
 Mix freely with each other
 Each gas acts on its own
Gas-Liquid Solutions
 Solubility ___________ with higher partial pressures of the
gas over a liquid
 Solubility ___________ with increasing temperature
Liquid-Liquid Solutions
 Some liquids are immiscible
 Insoluble in each other
 Due to polarity of liquids (usually non-polar
with polar)
 Miscible liquids
 Usually like with like
 Polar with polar
 Non-polar with non-polar
Solid-Solid Solutions
 Alloys
ALLOY
Bronze
Brass
Steel
Sterling Silver
14K Gold
Pewter
Solder
COMPONENT METALS
copper, tin
copper, zinc
iron, carbon, (various other
metals)
silver, nickel, copper
gold, copper, antimony
tin, copper, antimony
tin, lead
Solid-Liquid Solution
 Electrolytes
 Compound broken into _____
when dissolves
 Solution can carry electrical
current
 Nonelectrolytes
 IMF’s (but not molecules) are
broken when dissolves
 No electrical current can be
carried
Dissolving Nonelectrolytes
 Non-polar molecules
 Soluble in non-polar solvents
 Insoluble in polar solvents
 Polar molecules (or molecules
with polar sections)
 Soluble in polar solvents
 Insoluble in non-polar solvents
 Do not break apart
 ____ mole of solid solute creates
____ mole of particles in solution
Dissolving Electrolytes
 Ionization
 Breaks a covalently bonded compound into ions
 Ions spread throughout solutions
 Dissociation
 Breaks ions in ionic bond apart
 Ions spread throughout solution
 Both processes create more particles in solution than were
present in the solid solute
V’ant Hoff Factor
 Represented by ___
 Equals the number of particles created from each solute
when dissolved
 Nonelectrolytes i = ____
 C12H22O12 (s)  C12H22O12 (aq)
* 1 particle i = ___
 Electrolytes i = # of ions created from ionization or
dissociation
 NaCl (s)  Na+(aq) + Cl-(aq)
 MgCl2 (s)  Mg+2(aq) + 2 Cl-(aq)
* 2 particles
* 3 particles
i = ___
i = ___
Solvation
 Process of ___________
 Also called hydration when solvent is _________
 Bonds or IMF’s between particles must be broken
 Energy is absorbed
 Solvent particles surround the solute particles and form new
bonds or IMF’s
 Energy is released
Saturation
 An amount of solvent can only hold a certain amount of solute
 Amount depends on ________
 Amount also depends on _____________
 Usually increasing temperature increases solubility
 ______________ solution
 Amount 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 Curves
 Graph depicting the solubility of substances at different
temperatures
Concentrations of Solutions
 Comparison of amount of solute in a solvent
 _______________
 Dilute- small amount of solute compared to solvent
 Concentrated- large amount of solute
 ___________
 Molarity
 Molality
 ppm, ppb, ppt
 Mole fraction
 Mass %
Molarity
 Mole/Volume
 Equation
 Molarity (M) = moles of solute / liters of solution (not solvent)
* Amount must be in ________
* Volume must be in __________
 Changes with temperature
Molality
 Mole/Mass
 Equation
 Molality (m) = moles of solute / mass of solvent
* Amount must be in __________
* Mass must be in ____________
 Does not change with temperature
Colligative Properties
 Properties of solutions that depend on the ________ of
solute particles not the _________ of the solute
 Shift in Points
 Freezing point _________- solution freezes at a lower
temperature than the pure solvent
 Boiling point ________- solution boils at a higher temperaure
than the pure solvent
 Vapor Pressure
 Osmotic Pressure
Vapor Pressure
 Vapor pressure of solvent in solution is lower than vapor pressure
of pure solvent
Variables in Point Shifts
 m- Molality of solution
 i- V’ant Hoff factor
 Constants
 Kf
 Specific to solvent
 Shows the affect of solute on that solvent’s freezing point
 Kf for water is 1.86 °C kg/mol
 Kb
 Specific to solvent
 Shows the affect of solute on that solvent’s boiling point
 Kb for water is 0.512 °C kg/mol
Freezing Point Depression
 Equation
 ΔTf = iKf m
 Gives change in freezing point
 Must subtract from pure solvent’s freezing point to find
solution’s freezing point
Boiling Point Elevation
 Equation
 ΔTb = iKb m
 Gives change in boiling point
 Must add to pure solvent’s boiling point to find solution’s
boiling point