Solutions. SOLUTE + SOLVENT SOLUTION State of Matter homogenous mixture of gases (Air…) Gas:
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Transcript of Solutions. SOLUTE + SOLVENT SOLUTION State of Matter homogenous mixture of gases (Air…) Gas:
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SolutionsSolutions
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SOLUTE + SOLVENT SOLUTION
State of MatterState of Matter
homogenous mixture of gases (Air…)
Gas:Gas:
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solvent: liquid solute: liquid(ethanol in water)
solvent: liquid solute: gassolid
(soda water: CO2/H2O; brine: NaCl/H2O)
Liquid:Liquid:
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solvent: solid solute: liquid(Dental-filling alloy)
solvent: solid solute: solid(gold-silver alloy)
Solid:Solid:
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Dissolve: solute + solvent solution.
Crystallization: solution solute + solvent.
Saturation: crystallization and dissolution are in equilibrium.
Solubility: amount of solute required to form a saturated solution.
Supersaturated: a solution formed when more solute is dissolved than in a saturated solution.
Miscible: two liquids that mix.
Immiscible: two liquids that do not mix.
Terms to Know…
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Like Dissolves Like
“Rule”: polar solvents dissolve
polar solutes. Non-polar solvents
dissolve non-polar solutes. Why?
If ΔHsoln is too endothermic a
solution will not form.
NaCl in octane (C8H18): the ion-
London forces are weak because
octane is non-polar. Therefore,
the ion-London forces do not
compensate for the separation of
ions.
NaCl dissolves nicely in water.
+ –+–
+ –
+ –+–
+ –
NaCl
octane
water
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Terminology:
Solubility: is the maximum amount of the solute that will dissolve in a definite amount of solvent (at a given t°)
g/100 mL
Concentration: ratio of the solute and the solvent
Dilute solutionsConcentrated solutions
Saturated solutions:
solutepure solute dissolved
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Supersaturated solutions:
g/100 mL KNO3
PbCl2
NaCl
Solubility curves t°
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Temperature Effects: Solids
• Experience tells us that sugar dissolves better in warm water than cold.
• As temperature increases, solubility of solids generally increases.
• Sometimes, solubility decreases as temperature increases (e.g. Ce2(SO4)3).
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Properties of Water
Most abundant liquid
Vital to life
Universal solvent
1. High melting and boiling points
M.p.: 0.0°CB.p.: 100.0°C (0.1 MPa)
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Hydrogen Bonding
Special case of dipole-dipole forces.By experiments: boiling points of compounds with H-F, H-O, and H-N bonds are abnormally high.Intermolecular forces are abnormally strong.
-200
-150
-100
-50
0
50
100
150
0 1 2 3 4 5
Period
Bo
ilin
g P
oin
t (d
eg C
)
Group 4
Group 5
Group 6
Group 7
CH4
SnH4
GaH4SiH4
H2O
H2SH2Se
H2Te
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Water Molecule
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Solutions
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Phase Diagram of H2O
The melting point curve slopes to the left because ice is less dense than water.Triple point occurs at 0.0098°C and 4.58 mmHg.Normal melting (freezing) point is 0°C.Normal boiling point is 100°C.Critical point is 374°C and 218 atm.
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2. Density
0.0°C (ice) 0.91680 g/cm3
0.0°C (liquid) 0.99984 g/cm3
3.98°C 0.99997 g/cm3
25.0°C 0.99704 g/cm3
3. Surface tension: high
Bottom of meniscus
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4. High heat of vaporization
40.70 kJ/mol
5. High heat of fusion
6.02 kJ/mol
6. High specific heat
75.20 kJ/mol
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1. Chemically pure water
2. Water of crystallization or hydration
CuSO4 5H2O(s) CuSO4(s) + 5H2O(g)
(CaSO4)2 H2O (plaster of paris)
CaSO4 2H2O (gypsum)
Na2CO3 10H2O
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3. Groundwater
CationsCations AnionsAnions
Ca2+ HCO3-, CO3
2-
Na+ OH-
Mg2+ SO42-
K+ Cl-
Fe2+, Fe3+ NO3-
NH4+ F-, PO4
3-
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Hard water Soft water
Water Softening
Temporary hard water HCO3
- (bicarbonate) Permanent hard water
Boiling Softening agents precipitation
complex formation Distillation Ion-exchange
Mineral waterThermal water