Name

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Name describe each of the 7 crystal structures
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Solutions
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Solution

• Homogeneous mixture made up of at least one
  solute dissolved in the solvent

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Solute

• Substance being dissolved
• Portion in lesser molar amount

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Solvent

• Substance doing the dissolving
• Portion in greatest molar amount

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Colloid

• Slightly larger particles
• Light passes particles stay suspended

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Suspension

• Even larger particles
• Particles block or reflect light

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Tyndall Effect

• Because light reflects off suspended particles,
  the light ray can be seen from the side

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Size Comparison

• Solution lt Colloid
• Colloid lt Suspension

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Soluble

• When one substance (solute) dissolves in another
  (solvent)

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Solubility

• The amount of one substance (solute) dissolved in
  another (solvent)

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ConcentratedSolution

• A solution with a relatively large amount of
  solute dissolved

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Concentration

• The amount of solute dissolved into solution

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Dilute Solution

• A solution with a relatively small amount of
  solute dissolved

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Saturated Solution

• A solution with the maximum amount of solute
  dissolved in the solution

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Unsaturated Solution

• A solution with less than the maximum amount of
  solute dissolved in solution

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Supersaturated Solution

• A solution with greater than the maximum amount
  of solute dissolved in solution

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Solution Measures

• Concentration
• Molarity
• Molality
• Mole Fraction

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Percent Solution

• Mass of one portion per the total mass, all times
  100
• soln ma/mtotal x 100

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Molarity

• Moles of solute per liter of solution
• M molessolute/Lsoln

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Molality

• Moles of solute per kilogram of solvent
• mo molessolute/kgsolvent

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Mole Fraction

• Moles of one portion per total number of moles in
  the solution
• X molesa/molessoln

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Calculate the molarity of a 250 mL solution
containing 5.0 g NaOH dissolved in water
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Drill Calculate

• mass of NaCl required to make 1.5 L of 2.0 M NaCl

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Calculate the molality of 69 g of C2H5OH
dissolved in 500.0 mL of water
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Calculate the mole fraction of each portion when
92 g of C2H5OH dissolved in 144 mL of water
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Calculate the molality mole fraction of a
solution containing 46 g of C2H5OH dissolved in
1782 mL of water
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Colligative Properties

• Properties dependent only on the concentration of
  particles in solution

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Examples

• Vapor pressure
• Boiling Freezing points
• Osmotic pressure

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Drill

• Calculate the VP of a solution containing 36
  glucose (C6H12O6) in water at 29oC
• (VPwater 30.0 mm Hg)

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Vapor Pressure

• VPsolution (VPsolvent)(Xsolvent)
• X mole fraction
• VP vapor pressure

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Boiling Freezing
DT imoK DT change in BP or FP i ionic
activity K BP or FP constant
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Osmotic Pressure
p iMRT p osmotic pressure i ionic
activity M Molarity
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Calculate the vapor pressure of a solution
containing 150 g C5H10O5 in 162 mL of water at
30oC
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Calculate BP FP of 60.0 g of NaOH in 250 mL
waterKBP 0.512oC/moKFP -1.86oC/mo
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Calculate the osmotic pressure of a solution
containing 12 g of NaOH dissolved in 250 mL
solution at 27oC
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Calculate the vapor pressure of a solution
containing 120 g C3H7OH in 144 mL of water at its
BP.
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Calculate the osmotic pressure of a solution
containing 12 g of C4H8O4 dissolved in 750 mL
solution at 27oC
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Clausius-Claperon Eq
(T2)(T1) P2 (T2 T1) P1
Hv R ln
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VPbenzene Temp (oC) 24.5 27 73.5
127Calculate Hv for benzene
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Drill Calculate BP FP of 88 g of CO2 in 750 mL
waterKBP 0.512oC/moKFP -1.86oC/mo
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Calculate the osmotic pressure of a solution
containing 29.9 g of CoBr3 dissolved in 7500 mL
solution at 27oC
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Calculate the vapor pressure of a solution
containing 12.0 g C3H8O in 14.4 mL of water at
its BP.
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180 g C3H8O was dissolved in 180 mL H2O at 27oC
making a 1.5 g/mL solution. Calculate X, mo, M,
p, VP, BP, FP.
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Drill Calculate the mass of lead(II)nitrate
required to make 250 mL of 0.40 M Pb(NO3)2
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300 g C3H6NF was dissolved in 500 g C6H12O at
27oC making a 0.800 g/mL solution. Calculate X,
mo, M, p, VP, BP, FP.
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Calculate the molality of a solution that is 33.1
by mass Pb(NO3)2
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A 1.2 g/cm3 aqueous solution is 20.0 by mass
NaOH at 27oC. Calculate X, mo, M, p, MP
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Calculate the molecular mass of a covalent
compound dissolved in an aqueous solution to make
it 25 by mass when it boils at 102.048oC