Chapter 13 Solutions. Overview Solution Process energy changes, solution formation, chemical...
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Transcript of Chapter 13 Solutions. Overview Solution Process energy changes, solution formation, chemical...
Chapter 13
SolutionsSolutions
Overview Solution Process
• energy changes, solution formation, chemical reactions
Concentration• mole fraction, molarity, molality, mass
percent, ppm
Saturated Solutions & Solubility Factors Affecting Interactions
• solute-solvent, pressure, temperature
Colligative Properties
• vapor pressure lowering, boiling point elevation, freezing point depression, osmosis
Colloids
Solutions Solution
• mixture of two or more substances • components are the solute and the solvent
Solvent• component of the mixture present in greater
quantity• often retains its physical characteristics
Solute• component of the mixture present in smaller
quantity
Solution Process
Intermolecular Forces• must be overcome in both the solvent & solute
before the mixture can be formed• forces between the solute & solvent must be
similar in nature and strength
hydration• interaction between water (the solvent) &
solute is termed hydration
solvation• interaction between any solvent & the solute
Energy Relationships
Hsolution = H1 + H2 + H3
• H1 = energy required to separate solute particles
• H2 = energy required to separate solvent particles
• H3 = energy produced by interaction of solute/solvent
Hsolution is exothermic only if
• H3 is larger than H1 + H2
Solubility General Rule -- like dissolves like
• polar substances will dissolve other polar substances
• non-polar substances will dissolve other non-polar substances
• polar substances will not dissolve non-polar substances
Polar/Polar solutions• driven by energy relationships -- H3 is larger
than H1 + H2
Cont’d
Polar/Polar solutions• driven by energy relationships -- H3 is larger
than H1 + H2
Non-polar/Non-polar solutions• driven by disorder -- H3 is about the same as
H1 + H2
Cont’d
True Solution• solute particles remain unchanged
– NaCl(s) + H2O(l) Na+(aq) + Cl-(aq)
• no chemical reaction occurs– Ni(s) + 2HCl(aq) NiCl2(aq) + H2(g)
Concentration
Expresses a ratio between solute andsolvent/solution Mass %
• percent mass (%) = g solute x 100 total g solution
ppm -- parts per million• ppm = mass of solute x 106
tot. mass soln
Mole Fraction• Mole Fraction (X) = moles solute
total moles
Molarity• Molarity (M) = moles solute
1L solution
Molality
• Molality (m) = moles solute 1 kg solvent
Saturated Solutions & Solubility
Process
• solute + solvent solution
solution formation
crystallization
Solubility
• quantity of solute necessary to produce a saturated solution
• generally in grams of solute per 100 grams or mL of water
Saturated Solution
• solution is in equilibrium with undissolved solute
• solution contains the maximum amount of solute possible
Unsaturated Solution• solution contains less than the maximum amount of solute• there is no undissolved solute present
Supersaturated Solution• solution contains more than the maximum amount of solute• there is no undissolved solute present• solution is unstable
Factors Affecting Solubility Solute-Solvent Interactions
• types of solute/solvent -- polar or non-polar• like dissolves like• pairs of liquids which are soluble in all proportions are
miscible • pairs which are not soluble are immiscible
Pressure• solubility of gases increase with
– increasing pressure– increasing mass
Henry’s Law• Cg = kPg Cg is solubility of the gas, Pg is partial
pressure of gas, k is a constant
Temperature• generally, solubility of solids increases with
increasing temperature• solubility of gases decreases with increasing
temperature
Colligative Properties
Properties which depend on the quantity of solute:
Vapor Pressure Lowering• addition of a nonvolatile solute lowers the vapor pressure
of the solvent• extent of lowering depends on concentration of solute,
described by Raoult’s Law
Raoult’s Law• Psolvent = XsolventP°solvent
Cont’d Boiling Point Elevation
• Tb = Kb msolute
• Kb is a constant, m is molality
Freezing Point Depression• Tf = Kf msolute
Osmosis• = (n/V) RT = MRT• M is molarity• R is the gas constant (0.0821 L atm/mol K)
Colloids -dispersed particles which are larger than
molecular in size -size from 10 to 2000Å -may be a clump of particles or one large
particle• hemoglobin has a MM = 64,500 amu and 65 x 55 x 50 Å
-appear cloudy or opaque & scatter light -- Tyndall effect