name & describe each of the 7 crystal structures
DESCRIPTION
Name & describe each of the 7 crystal structures. Solutions. Solution. Homogeneous mixture made up of at least one solute dissolved in the solvent. Solute. Substance being dissolved Portion in lesser molar amount. Solvent. Substance doing the dissolving Portion in greatest molar amount. - PowerPoint PPT PresentationTRANSCRIPT
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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 < Colloid
•Colloid < 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
T = imoKT = change in BP or FP
i = ionic activity
K = BP or FP constant
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Osmotic Pressure = iMRT
= 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
Hv= R ln(T2)(T1) P2
(T2 – T1) P1
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VPbenzene Temp (oC) 24.5 2773.5 127
Calculate 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, , 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, ,
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,
, & 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