Concept Presentation: Solutions and Solubility Chemistry 11 U
Chemistry-Ch10_Solutions and solubility
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Transcript of Chemistry-Ch10_Solutions and solubility
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1010 Solutions Solutions and solubilityand solubility
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10.1 Introduction to solutions 10.1 Introduction to solutions and solubilityand solubility
• Solution– Homogeneous mixture of two or more
pure substance – May be gaseous, liquid or solid
• Solvent– Liquid of a liquid solution
• Solute– Dissolved substance in liquid solution
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10.1 Introduction to solutions 10.1 Introduction to solutions and solubilityand solubility
• Solubility– Maximum amount of solute that dissolves
completely in a given amount of solvent at a particular temperature, T
• Saturated solution– Solution in which no more solute will
dissolve
• Dissolution– Process of dissolving a solute in a solvent to
give a homogeneous solution
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10.2 Gaseous solutions10.2 Gaseous solutions
• All gases mix completely with all other gases in all proportions
• Gases mix spontaneously hence ΔG for mixing process negative
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10.2 Gaseous solutions10.2 Gaseous solutions
• Enthalpy change when two gases are mixed is usually small
• Large positive ΔmixS term ensures ΔmixG negative
• Intermolecular forces between individual gas molecules are tiny, and gas molecules are far apart
• No impediment to the mixing of gases
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10.2 Gaseous solutions10.2 Gaseous solutions
• The magnitude of interatomic and intermolecular attractions in the condensed phase can determine whether or not two substances can mix
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10.3 Liquid solutions10.3 Liquid solutions
• Gas–liquid solutions
– For a gas to dissolve in a liquid, the gas molecules must be able to disperse themselves evenly throughout the solvent
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10.3 Liquid solutions10.3 Liquid solutions
• Gas–liquid solutions
– Intramolecular forces between the solvent molecules are not negligible
– Neither therefore is the value of ΔsolH, the enthalpy of solution
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10.3 Liquid solutions10.3 Liquid solutions
• Gas–liquid solutions
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• Gas–liquid solutions– Solubility of gases vary significantly with
temperature– Solubility of gases vary significantly with
pressure
10.3 Liquid solutions10.3 Liquid solutions
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10.3 Liquid solutions10.3 Liquid solutions
• Gas–liquid solutions– For gases that do not react with the solvent,
Henry’s law gives the relationship between gas pressure and gas solubility
– cgas is the concentration of the gas
– pgas is the partial pressure of the gas above the solution
– kH is called the Henry’s law constant and is unique to each gas
Tpkc constantgasHgas
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10.3 Liquid solutions10.3 Liquid solutions
• Gas–liquid solutions– Equation is only true at low
concentrations and pressures– An alternative expression of Henry’s law
is:
– c1 and p1 refer to initial conditions
– c2 and p2 refer to final conditions
2
2
1
1pc
pc
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10.3 Liquid solutions10.3 Liquid solutions
• Liquid–liquid solutions
– Formation of a liquid–liquid solution requires that the attractive forces present between the molecules of the two pure liquids is overcome
– Two substances are MISCIBLE when they mix completely in all proportions
– Two substances are IMMISCIBLE when they form two layers upon the addition of one to the other
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10.3 Liquid solutions10.3 Liquid solutions
• Liquid–liquid solutions
C C O
H
HH
H
H H
Like–dissolves–like
Ethanol Benzenehydrogen bond
C
CC
C
CC
H
H
H
HH
H
H O
H
H O
C2H5
H
OC2H5
H O
H
O
H
H
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10.3 Liquid solutions10.3 Liquid solutions
• Liquid–solid solutions– Basic principles remain
the same– Solvation is when a solute
molecule is surrounded by solvent molecules
– Hydration occurs when solutes become surrounded by water molecules
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• Liquid–solid solutions– Like-dissolves-like– When intermolecular attractive forces within
solute and solvent are sufficiently different,the two do not form a solution
10.3 Liquid solutions10.3 Liquid solutions
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• Liquid–solid solutions
10.3 Liquid solutions10.3 Liquid solutions
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• Liquid–solid solutions
10.3 Liquid solutions10.3 Liquid solutions
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• Liquid–solid solutions– Temperature can
have a significant effect on the solubility of a solid solute in a liquid
10.3 Liquid solutions10.3 Liquid solutions
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproduct• Ionic salts are generally classified as
being either soluble or insoluble in waterAgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
AgCl(s) Ag+(aq) + Cl–(aq)
Ksp = [Ag+][Cl–]
• Ksp is called the solubility product
MaXb(s) aMc+(aq) + bXd–(aq)
Ksp = [Mc+]a[Xd–]b
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproduct• The relationship between Ksp and
solubility
– Molar solubility (s)molar concentration of a salt in its saturated solution
– Molar solubility can be used to calculate Ksp, assuming that all of the salt that dissolves is 100% dissociated into its ions
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproductThe solubility of AgBr in water is 1.3 × 10–4 g L–1 at 25 °C. Calculate Ksp for AgBr at this temperature
AgBr(s) Ag+(aq) + Br–(aq)
Ksp = [Ag+][Br–]
[Ag+] = [Br–] = 6.9 × 10–7 mol L–1
Ksp = [Ag+][Br–] = (6.9 × 10–7 mol L–1)(6.9 × 10–7 mol L–1)
Ksp = 4.8 × 10–13 at 25 °C
mol109.6gmol77.187
g103.1 71
4
Mm
n
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproductCalculate the molar solubility of lead iodide, PbI2, given that Ksp(PbI2) = 7.9 × 10–9
PbI2(s) Pb2+(aq) + 2I–(aq)
Ksp = [Pb2+][I–]2
Define the molar solubility of PbI2(s) as s mol L–1
[Pb2+] = s mol L–1
[I–] = 2s mol L–1
Ksp = (s)(2s)2 = (s)(4s2) = 4s3 = 7.9 × 10–9
s = 1.3 × 10–3
The molar solubility of PbI2(s) in water at 25 °C is 1.3 × 10–3 mol L–1
4109.7 9
3s
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproduct• The common ion effect
– Any ionic salt is less soluble in the presence of a common ion, an ion that is in the salt
PbCl2(s) Pb2+(aq) + 2Cl–(aq)
Ksp = [Pb2+][Cl–]2
Add Pb(NO3)2(aq) to saturated solution of PbCl2 instantaneously increases [Pb2+] and therefore Qsp (ionic product).
Qsp > Ksp
PbCl2 is precipitated
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproductWhat is the molar solubility of PbI2 in a 0.10 M NaI solution?
PbCl2(s) Pb2+(aq) + 2Cl–(aq)
Ksp = [Pb2+][Cl–]2 = 7.9 × 10–9
Ksp = s(0.10 + 2s)2 = 7.9 × 10–9
Ksp = s(0.10)2 = 7.9 × 10–9
Molar solubility of PbI2 in 0.10 M NaI solution is 7.9 × 10–7 M (s)
PbI2(s) Pb2+(aq) + 2I–(aq)
Initial concentration (M) 0 0.10
Change in concentration (M) +s +2s
Equilibrium concentration (M) s 0.10 + 2s
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10.4 Quantification of 10.4 Quantification of solubility: the solubility solubility: the solubility
productproduct• Prediction of precipitation
– Qsp > Ksp precipitate will form
– Qsp < Ksp no precipitate will form
AgCl(s) Ag+(aq) + Cl–(aq)
Ksp = [Ag+][Cl–] = 1.8 × 10–10
[Ag+] = 5.0 × 10–7 mol L–1
[Cl–] = 5.0 × 10–5 mol L–1
Qsp = 2.5 × 10–11
Qsp < Ksp no precipitate will form
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Nonvolatile solutes– Solutes that can’t evaporate from solution– Vapour pressure of a solution of
nonvolatile solutes is lower than the pure solvent
• Colligative properties– Depend on number of solute particles in
solution rather than chemical identities
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Molarity– Amount of substance in a particular
volume of solution
– Solutions (usually) increase in volume with increasing temperature
– The molarity of a solution changes as the temperature changes
amount of solute (mol)
molarity ( )volume of solution (L)
c
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Molality– Preferred method of expressing solution
composition when colligative properties involved
– Amount of solute per kilogram of solvent
– Temperature independent
amount of solute (mol)
molality ( )mass of solvent (kg)
b
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Mole fraction– The number of moles of a particular
component divided by the total number of moles of material in the solution
– The mole fraction of A, XA, in a solution containing substances A, B and C
– Temperature independent
AA
A B C
nX
n n n
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Raoult’s law
– Boiling point of a solution containing a nonvolatile solute is higher than that of the pure solvent
– Boiling point of a solvent is the temperature at which the vapour pressure of the solvent is equal to the atmospheric pressure
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Raoult’s lawpsolution = Xsolvent p*
solvent
– psolution – vapour pressure of the solution
– Xsolvent – mole fraction or solvent in the solution
– p*solvent – vapour pressure of pure solvent
– For a simple two component system– Provided the solution is sufficiently dilute
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10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
• Raoult’s law psolution = Xsolvent p*
solvent
Xsolvent = 1 – Xsolute
psolution = (1 – Xsolute)p*solvent
psolution = p*solvent – Xsolutep*
solvent
Δp = Xsolutep*solvent
Δp = p*solvent – psolution
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• Raoult’s law– A solution that obeys Raoult’s law is called an ideal
solution– These solutions
are generally dilute and have only small interactions between their constituent molecules
10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
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• Solutions containing more than one volatile component– For component A
pA = XAp*A
– For component BpB = XBp*
B
– Total pressureptotal = XAp*
A + XBp*B
10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
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• Boiling point elevation and freezing point depression– boiling point elevation
ΔTb
ΔTb = Kbb
– freezing point depression
ΔTf
ΔTf = Kfb
10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Boiling point elevation and freezing point depression– Molal boiling point elevation constant
• Kb
• Units – K mol–1 kg
– Molal freezing point depression constant• Kf
• Units – K mol–1 kg
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Boiling point elevation and freezing point depression– Molality of the solution
• b
• Units – mol kg–1
– Kbb and Kf b are properties of the solvent only and independent of the identity of the solute
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Osmosis and osmotic pressure– A membrane keeps mixtures and solutions
organised and separated.– Semipermeable membranes allow selective
substances to pass through– Dialysis occurs when a dialysing membrane
allows both water and small solute particles through
– Osmosis is a net shift of only solvent through an osmotic membrane
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10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
• Osmosis and osmotic pressure
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Osmosis and osmotic pressure– Osmotic pressure
• Π
– In dilute aqueous solution
Π = cRT
ΠV = nRT
– This is the van’t Hoff equation for osmotic pressure
Vn
c
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• Osmosis and osmotic pressure
Osmometer
Isotonic HypotonicHypertonic
10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Measurement of solute dissociation– Molal freezing point depression constant
for water is 1.86 K mol–1
– 1.00 mol kg–1 NaCl freezes at about –3.37 °C
– NaCl(s) Na+(aq) + Cl–(aq)– Solution has a a total molality of dissolved
solute particles of 2 mol kg–1
– Theoretically, a 1.00 mol kg–1 NaCl solution should freeze at –3.72 °C
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Measurement of solute dissociation– With increasing dilution solutes behave
more and more as if they were 100 % dissociated
– Compare degrees of dissociation by quantity called the van’t Hoff factor (i)
f
f
Ti
Tmeasured
calculatedasnonelectrolyte
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• Measurement of solute dissociation
10.5 Colligative properties 10.5 Colligative properties of solutionsof solutions
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Measurement of solute dissociationCH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO–(aq)
– 1.00 mol kg–1 aqueous acetic acid solution freezes at –1.90 °C
– Only a little lower than expected if no ionisation occurred
1
1
kgmol02.1
kgmolK86.1
K90.1
b
KT
bf
f
%2ionisation%
%10000.102.0
ionisation%
100%availableacidofmol
ionisedofmolionisation%
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10.5 Colligative properties of 10.5 Colligative properties of solutionssolutions
• Measurement of solute dissociation– Some molecular solutes produce smaller
colligative effects than their molal concentrations would lead us to predict
– Often evidence of solute molecules clustering or undergoing association in solution
C6H5 C O HO
C6H5 CO H
OC6H5C
OH
O2
benzoic acid benzoic acid dimer
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