Properties of Solutions - 2018 Filled in Chem 1048
Properties of Solutions - 2018 Filled in Chem 1048
Properties of Solutions - 2018 Filled in Chem 1048
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pure substances
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Solute
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3B&6,+B6,3$3B)$888888888888$CD&)").3$/.$
Solvent
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Solvent Solute
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Natural tendency of Substances to mix
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intermolecular interactions
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solute-Solute
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"6@,3)$D'&3/(@)"$3B&6,+B$3B)$"6@K).3#$
%" #############$/.3)&'(3/6."$-)32)).$"6@K).3$
Solvent-Solvent
D'&3/(@)"$7,"3$-)$6K)&(67)$36$7'U)$&667$
>6&$3B)$"6@,3)$D'&3/(@)"$/.$3B)$"6@K).3#$
&" #################$/.3)&'(3/6."$-)32)).$3B)$
Solvent-Solute
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D'&3/(@)"$7/=#$$
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solutions ;'&0)
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condensed $01(%(J) '.&%"9#,%4-,1") *#"4%()
K%4#9%)88888888888888887)
re-arranged
:0%) 888888888888888)
intermolecular *#"4%() K%&;%%.) (#,-&%)
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strong
&#) 8888888888)
compete ;'&0) &0#(%) K%&;%%.) (#,-&%)
$1"&'4,%()1.B)&0#(%)K%&;%%.)(#,=%.&)$1"&'4,%(7)
W$
:0%)+#,-&'#.)!"#4%(()
The water H-bonds have to be
interrupted,
NaCl dissociates into Na+ Cl-,
______________
ion dipoles forces form:
As a solution forms, the solvent pulls the solute particles apart and
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surrounds or solvates them
:D$%()#*)+#,-&'#.()
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encourages crystillization
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cool
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interactions
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Temperature
M# <<<<<<<<<<<<<<<<<<<<<<<<<<$
Pressure ( for gases)
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more similar
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more likely
(-K(&1.4%)'()&#)K%)888888888888)'.)1.#&0%"7)
soluble
>?19$,%() >?19$,%()
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nonpolar
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water C@/U)$<<<<<<E#$
fats
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not
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like dissolves like
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-)33)&$/3$F/""6@K)"$/.$'$D6@'&$"6@K).3#$
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F/""6@K)"$/.$'$.6._D6@'&$"6@K).3#$
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Exercise)
Predict whether each of the following substances is
more likely to dissolve in carbon tetrachloride (CCl4)
or water (H2O)? C7H16, Na2SO4, HCl, I2.$
Step 1: Analyze the given molecules wether non-polar or polar
Polar Solvent: h2o (H-bond predominate)
Non-polar solvent: CCl4 (london dispersion)
Polar solutes: NaSO4 (ionic interaction predominate) and
HCl (dipole-dipole interaction predominate)
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!"%((-"%)>**%4&()
?.$+).)&'@A$3B)$
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increases
2/3B$<<<<<<<<<<<<<<$
increasing mass
<<<<<<<<<<<#$
Q'&+)&$76@)(,@)"$
B'K)$<<<<<<<<<<<<$
stronger
<<<<<<<<<<<<<<<<<<<<#$
dispersion forces
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How Soluble could CO2 be in comparsion to CO?
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liquids
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F6)"$.63$(B'.+)$888888888$2/3B$D&)"",&)#$
appreciably
$
IB)$"6@,-/@/3G$6>$'$8888888/.$'$@/R,/F$/"$
gas
88888888888888888888888888$36$/3"$D&)"",&)#$
directly proportional
$
IB)$888888888$3B)$888888888$A$3B)$9#"%$
higher pressure
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'.F$3B)$E"%1&%"$3B)$401.4%$6>$'$E1($
76@)(,@)$(&"'G'.E$3B)$(-"*14%$'.F$%.&%"'.E$
3B)$(#,-&'#.#$
IB)&)>6&)A$3B)$888888888$3B)$888888888$A$3B)$
higher pressure
greater
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IB)$888888888$3B)$888888888$A$3B)$>)2)&$
lower pressure
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:0%)(#,-K','&D)#*)1)E1()'.)1)
,'A-'B)(#,=%.&)'.4"%1(%()'.)
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$1"&'1,)$"%((-"%)#*)&0%)E1()
1K#=%)&0%)(#,-&'#.7)
Sg = kPg
Carbonated beverages are bottled with a
Where,
partial pressure of CO2 >1 atm.
Sg is the solubility of the gas; As bottle is is opened the partial pressure
k LVWKH+HQU\¶VODZFRQVWDQW of CO2 decreases the solubility of CO2
for that gas in that solvent; decreases.
Pg is the partial pressure of the Therefore the bubbles of CO2 escape from
gas above the liquid. Solutiom
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Example)
Calculate the concentration of carbon dioxide in a soft
drink that is bottled with a partial pressure of CO2 of
0.41Mpa over the liquid at 25o&7KH+HQU\¶VODZ
constant for CO2 in water at this temperature is 3.4 x 10-4
mol/m3Pa-1.
¾Generally, the
solubility of
_____________
solid solutes
in liquid solvents
increases with
increasing
temperature.
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$ n= C. V = 1.0 mol/L x 0.250 L = 0.250 mol
m= n. Mr= 0.250 mol x 159.61 g/mol = 39.9 g
There foe the weigh out 39.9g of CuSO4 and add 250ml of
H2O to make a 1 M solution of CuSO4
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-)$+/K).$6&$.))F"$ a liquid.
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Stock Solution.
;R,)6,"$"6@,3/6."$6>$@62)&$(6.().3&'3/6.$('.$
3B).$-)$6-3'/.)F$-G$'FF/.+$2'3)&A$'$D&6()""$
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Dilution.
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(6.().3&'3)F$6.)g$
XYH)50%.)1)(#,=%.&)'()1BB%B)&#)1)(#,-&'#.J)&0%)
.-9K%")#*)9#,%()#*)(#,-&%)"%91'.()-.401.E%B)
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"6@,3/6.$-G$F/@,3/.+$'$0#99!$8,NL:$"36(U$"6@,3/6.#$
Moles of Solute before = moles of solute after solution
Known formation: volume (250.0ml) and concentration
(0.100mol/L) of th dilute solution.
Therefore from the 1.00M CuSo4 stock solution, we would
withdraw, 25,00mL into a 250,0mL flask with water.
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qualtative
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qualitative
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Mass % Na Cl = 1.50g x100 = 2.91%
(1.50g+50.0g)
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A solution contains 5.0 g of toluene (C7H8) and 225 g of benzene and has a
density of 0.876 g/ml. Calculate the molarity and molality of the solution.
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A solution containing equal masses of glycerol (C3H8O3)
and water has a density of 1.10 g/ml.
Calculate (a) the molality of glycerol (b) the mole fraction of
glycerol (c) molarity of glycerol
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1. A commercial bleach solution contains 3.62% by mass
of NaOCl in water. Calculate (a) the mole fraction and (b)
the molality of NaOCl in the solution.
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A Colligative Property ± is a physical property of a solution
that depends on _________________________________
the number of solute particles present
regardless of the nature of the solute.
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Definition: quantitfies the extent to which non-volatile
solute lowers the vapor pressure of the solvent.
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Ideal solution: one that obeys 5DRXOW¶V law.
5DRXOW¶V law breaks down when the solvent-solvent and solute-solute
intermolecular forces are greater than solute-solvent intermolecular forces.
NOTE: This is one of those times when you want to make sure you have the
vapor pressure of the solvent.
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Kf
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constant of the solvent.
deltaTf is subtracted from the normal freezing point of
¾______
the solvent.
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depression by definition
When a solution freezes, almost pure solvent is formed
first.
± Therefore, the sublimation curve for the pure solvent is
the same as for the solution.
± Therefore, the triple point occurs at a lower temperature
because of the lower vapor pressure for the solution.
The melting-point (freezing-point) curve is a vertical line
from the triple point.
The solution freezes at a lower temperature (ǻTf) than the
pure solvent.
Decrease in freezing point (ǻTf) is directly proportional to
molality (Kf is the molal freezing-point-depression
constant) V:$
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The number of fragments that a solute breaks up into for
a particular solvent.
i= delta Tf (measured)
delta Tf (non-electrolyte)
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ǻT does not depend on ǻTb = Kb x m
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but only on
how many particles are ǻTf = Kf x m
dissolved.
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Calculate the freezing point of a solution containing 0.600 kg of CHCl3
and 42.0 g of eucalyptol (C10H18O), a fragrant substance found in the
leaves of eucalyptus leaves. Use Table 13.4 in text book to get Kf.
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Estimate the freezing point of a 0.010 m aqueous
solution of aluminium sulphate, Al2(SO4)3. Assume the
value of i based on the formula of the compound.
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Which of the following solutes will produce the largest increase
in boiling point upon addition of 1 kg of water: 1 mol of Co
(NO3)2, 2 mol of KCl, 3 mol of ethylene glycol (C2H6O2)?
Remember: colligative properties depend on quantity of solute molecules
(E.g. freezing point depression, melting point elevation and vapour pressure).
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¾ Some substances form semi-permeable membranes,
allowing some smaller particles to pass through, but
blocking other larger particles.
¾ In biological systems, most semi-permeable membranes
allow water to pass through, but not solutes.
Definition: In osmosis,
there is net movement
of solvent from the
area of higher solvent
concentration (lower
solute concentration) to
the are of lower
solvent concentration
(higher solute
concentration).
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¾ The pressure required to stop osmosis, known as
osmotic pressure, ʌ, is
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‒Cucumber placed in NaCl solution loses water to
shrivel up and become a pickle.
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The osmotic pressure of an aqueous solution of a certain
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mass. The solution contained 3.50mg of protein dissolved
in sufficient water to form 5.00mL of solution. The osmotic
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mass. WV$
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Step 1: Write the known/given values & do conversions
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Step 3: Determine the moles.
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125 mg of an alkaline earth metal chloride (XCl2) dissolved in
enough water to make 50.0 mL of solution at 298Û&KDVDQ
osmotic pressure of 1.16 atm. Identify the alkaline earth metal.
Step1:
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Describe the Solution Process.
Distinguish among solvent, solute, solution.
Explain the meaning of saturated solutions and solubility.
Describe the factors affecting solubility, including solute-
solvent interactions, pressure and temperature effects.
Express concentrations in mass percent (m/m %), m/v
%, ppm and ppb, mole fraction, molarity, molality and
osmolality and convert between them.
Explain what is meant by standard solution.
Calculate how to prepare a specified volume of solution
having a specified concentration starting with either a
solid solute or a solution ofX0$known concentration.
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Define the composition of a mixture in terms of its
osmolarity.
Explain the phenomena of colligative properties
including vapor pressure lowering, boiling point
elevation, freezing point depression and osmotic
pressure, and do calculations including molar mass
determinations.
Explain gas solubility. State and apply Henry s Law.
Calculate partial pressure of gases in solution.
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