Transcript 18-Solutions

Drill: Draw
LDDs for:
BF3
NH3
C3H6 C3H7NO
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
Colloid
•Slightly larger particles
•Light passes &
particles stay
suspended
Suspension
•Even larger
particles
•Particles block or
reflect light
Tyndall Effect
•Because light reflects
off suspended particles,
the light ray can be
seen from the side
Size Comparison
•Solution < Colloid
•Colloid < Suspension
Soluble
•When one
substance (solute)
dissolves in
another (solvent)
Solubility
•The max amount of
one substance
(solute) dissolved
in another (solvent)
Concentration
•The amount of
solute dissolved
into solution
Concentrated
Solution
•A solution with a
relatively large
amount of solute
dissolved
Dilute Solution
•A solution with a
relatively small amount
of solute dissolved
Saturated Solution
•A solution with the
maximum amount of
solute dissolved in
the solution
Unsaturated Solution
•A solution with less
than the maximum
amount of solute
dissolved in solution
Supersaturated Solution
•A solution with greater
than the maximum
amount of solute
dissolved in solution
Drill:
C4 H 8
Draw
HNO3
LDDs
C4 H 6 O
for:
Solution
Chemistry
Solution Measures
•Concentration: % soln
–Molarity
–Molality
–Mole Fraction
Percent Solution
•Mass of one portion per
the total mass, all times
100 %
•%soln = ma/mtotal x 100 %
Molarity
•Moles of solute per
liter of solution
•M = molessolute/Lsoln
Molality
•Moles of solute per
kilogram of solvent
•mo =
molessolute/kgsolvent
Mole Fraction
•Moles of one portion
per total number of
moles in the solution
•X = molesa/molessoln
Calculate the molarity
of a 250 mL solution
containing 5.0 g
NaOH dissolved in
water
Calculate the
molality of 69 g of
C2H5OH dissolved
in 500.0 mL of
water
Calculate the mole
fraction of each
portion when 92 g of
C2H5OH dissolved in
144 mL of water
Calculate the molality
& mole fraction of a
solution containing 46
g of C2H5OH
dissolved in 1782 mL
of water
Drill:
•Calculate the mass
of KI required to
make 250 mL of
0.500 M KI.
Colligative Properties
•Properties dependent
only on the
concentration of
particles in solution
Examples
•Vapor pressure
•Boiling & Freezing
points
•Osmotic pressure
Vapor Pressure
•VPsolution =
(VPsolvent)(Xsolvent)
•X = mole fraction
•VP = vapor pressure
Boiling & Freezing
DT = imoK
DT = change in BP or FP
i = ionic activity
K = BP or FP constant
Osmotic Pressure
p = iMRT
p = osmotic pressure
i = ionic activity
M = Molarity
Calculate the vapor
pressure of a solution
containing 150 g
C5H10O5 in 162 mL of
o
water at 30 C
Calculate BP & FP of
60.0 g of NaOH in
250 mL water
o
KBP = 0.512 C/mo
o
KFP = -1.86 C/mo
Calculate the osmotic
pressure of a solution
containing 12 g of
NaOH dissolved in
250 mL solution at
o
27 C
Drill:
•Calculate the VP of a
solution containing 36 %
m/m glucose (C6H12O6)
o
in water at 29 C:
•(VPwater = 30.0 mm Hg)
Drill: Draw
LDDs for:
BF3
NH3
C3H6 C3H7NO
Are there any
questions on
previous
material?
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
Colloid
•Slightly larger particles
•Light passes &
particles stay
suspended
Suspension
•Even larger
particles
•Particles block or
reflect light
Tyndall Effect
•Because light reflects
off suspended particles,
the light ray can be
seen from the side
Size Comparison
•Solution < Colloid
•Colloid < Suspension
Soluble
•When one
substance (solute)
dissolves in
another (solvent)
Solubility
•The max amount of
one substance
(solute) dissolved
in another (solvent)
Concentration
•The amount of
solute dissolved
into solution
Concentrated
Solution
•A solution with a
relatively large
amount of solute
dissolved
Dilute Solution
•A solution with a
relatively small amount
of solute dissolved
Saturated Solution
•A solution with the
maximum amount of
solute dissolved in
the solution
Unsaturated Solution
•A solution with less
than the maximum
amount of solute
dissolved in solution
Supersaturated Solution
•A solution with greater
than the maximum
amount of solute
dissolved in solution
Drill:
C4 H 8
Draw
HNO3
LDDs
C4 H 6 O
for:
Solution
Chemistry
Solution Measures
•Concentration: % soln
–Molarity
–Molality
–Mole Fraction
Percent Solution
•Mass of one portion per
the total mass, all times
100 %
•%soln = ma/mtotal x 100 %
Molarity
•Moles of solute per
liter of solution
•M = molessolute/Lsoln
Molality
•Moles of solute per
kilogram of solvent
•mo =
molessolute/kgsolvent
Mole Fraction
•Moles of one portion
per total number of
moles in the solution
•X = molesa/molessoln
Calculate the molarity
of a 250 mL solution
containing 5.0 g
NaOH dissolved in
water
Calculate the
molality of 69 g of
C2H5OH dissolved
in 500.0 mL of
water
Calculate the mole
fraction of each
portion when 92 g of
C2H5OH dissolved in
144 mL of water
Calculate the molality
& mole fraction of a
solution containing 46
g of C2H5OH
dissolved in 1782 mL
of water
Drill:
•Calculate the mass
of KI required to
make 250 mL of
0.500 M KI.
Are there any
questions on
previous
material?
Colligative Properties
•Properties dependent
only on the
concentration of
particles in solution
Examples
•Vapor pressure
•Boiling & Freezing
points
•Osmotic pressure
Vapor Pressure
•VPsolution =
(VPsolvent)(Xsolvent)
•X = mole fraction
•VP = vapor pressure
Boiling & Freezing
DT = imoK
DT = change in BP or FP
i = ionic activity
K = BP or FP constant
Osmotic Pressure
p = iMRT
p = osmotic pressure
i = ionic activity
M = Molarity
Calculate the vapor
pressure of a solution
containing 150 g
C5H10O5 in 162 mL of
o
water at 30 C
Calculate BP & FP of
60.0 g of NaOH in
250 mL water
o
KBP = 0.512 C/mo
o
KFP = -1.86 C/mo
Calculate the osmotic
pressure of a solution
containing 12 g of
NaOH dissolved in
250 mL solution at
o
27 C
Drill:
• Calculate the VP of a
solution containing 36.0 %
m/m glucose (C6H12O6) in
o
water at 29 C:
• (VPwater = 30.0 mm Hg)
Test
Review
Classify the type of
Bonding:
Fe-Cl
C-Cl
S-O
Fe-Cr
H-Br
K-I
Classify the type of
IM Force:
H2 & Cl2
HF & HF
H2 & HBr
HBr & HI
CH4 & C2H6
Draw LDDs for:
BH3 NCl3
CF4 C3H6
-2
IF3 CO3
Calculate the BP of a
solution containing 120
g C3H7OH in 250 mL of
water at its BP.
o
KBP = 0.512 C/mo
o
KFP = -1.86 C/mo
Calculate the osmotic
pressure of a solution
containing 12 g
of NaOH dissolved in
o
50.0 mL solution at 27 C
Calculate the vapor
pressure of a solution
containing 12.0 g
C3H8O in 14.4 mL of
water at its BP.
VPsolvent = 120 kPa
Calculate the
molarity of 33.1 g of
Pb(NO3)2 dissolved
in 250 mL of
solution.
Draw LDDs for:
PCl3
C3H7NO
-1
NO3
Calculate the mass of
lead(II)nitrate
required to make 250
mL of 0.40 M
Pb(NO3)2
Calculate the BP of a
solution containing
29.9 g of CoBr3
dissolved in 75 mL of
water.
o
KBP = +0.512 C/mo
Calculate the
molality of a
solution that is 33.1
% by mass Pb(NO3)2
in water
Drill: Calculate
the osmotic
pressure of 0.88 g
of CO2 in 750 mL
o
of soln at 27 C
30.0 g C3H6NF was
dissolved in 50.0 g
C6H12O (VP = 20.0 kPa)
o
at 27 C making a 0.800
g/mL solution. Calculate:
X, mo, M, p, & VP.
180 g C3H8O was
dissolved in 180 mL
o
H2O at 27 C making a
1.5 g/mL solution.
Calculate X, mo, M,
p, VP, BP, & FP.
3
g/cm
A 1.2
aqueous
solution is 20.0 % by
o
mass NaOH at 27 C.
Calculate: X, mo, M,
p, & MP
Calculate the molecular
mass of a covalent
compound dissolved in an
aqueous solution to make
it 25 % by mass when it
o
boils at 102.048 C
Are there any
questions on
previous
material?
Test
Review
Classify the type of
Bonding:
Fe-Cl
C-Cl
S-O
Fe-Cr
H-Br
K-I
Classify the type of
IM Force:
H2 & Cl2
HF & HF
H2 & HCl
HBr & HI
CH4 & C2H6
Draw LDDs for:
BH3 NCl3
CF4 C3H6
-2
IF3 CO3
Calculate the FP & BP
of a solution containing
120 g C3H7OH in 250
mL of water at its BP.
o
KBP = 0.512 C/mo
o
KFP = -1.86 C/mo
Drill: Calculate the
molarity of 33.1 g of
Pb(NO3)2 dissolved
in 250 mL of
solution.
Calculate the BP of a
solution containing
29.9 g of CoBr3
dissolved in 75 mL of
water.
o
KBP = +0.512 C/mo
Calculate the
molality of a
solution that is 33.1
% by mass Pb(NO3)2
in water
Drill: Calculate
the osmotic
pressure of 0.88 g
of CO2 in 750 mL
o
of soln at 27 C
30.0 g C3H6NF was
dissolved in 50.0 g
C6H12O (VP = 20.0 kPa)
o
at 27 C making a 0.800
g/mL solution. Calculate:
X, mo, M, p, & VP.
180 g C3H8O was
dissolved in 180 mL
o
H2O at 27 C making a
1.5 g/mL solution.
Calculate X, mo, M,
p, VP, BP, & FP.
3
g/cm
A 1.2
aqueous
solution is 20.0 % by
o
mass NaOH at 27 C.
Calculate: X, mo, M,
p, & MP
Calculate the molecular
mass of a covalent
compound dissolved in an
aqueous solution to make
it 25 % by mass when it
o
boils at 102.048 C