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Solutions Part I: The Solution Process
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Solution:
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Solutions: Solute: Solvent
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Types of Solutions
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The solution process To dissolve a solute in a solvent, the intermolecular attractions between solute and solute must be strong enough to compete with solvent- solvent and solute- solute attractions.
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Solvation
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Hydration
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Dissolving an ionic solid in water The ion-dipole attractions between the salt and the solvent must be strong enough to overcome the lattice energy
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“Steps” of the solution process Step 1
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“Steps” of the solution process Step 1 Step 2
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“Steps” of the solution process Step 1 Step 2 Step 3
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Endothermic vs. exothermic?
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Why do processes occur? Achieve a lower energy state Exothermic processes lead to lower enthalpy
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Why do processes occur? More randomness Greater “entropy” Can more than compensate for increasing enthalpy
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Did it dissolve, or did it react? Just because a substance “disappears” into a solvent doesn’t mean that the substance dissolved!
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Dissolving vs. reaction Dissolving Physical change Can recover the original substance by evaporating the solvent
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Dissolving vs. reaction Dissolving Physical change Can recover the original substance by evaporating the solvent Chemical change New substances form
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Solutions saturated unsaturated
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Supersaturated solutions
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Will this substance dissolve?
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“Like dissolves like” Non-polar substances tend to dissolve in non-polar solvents
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“Like dissolves like” Non-polar substances tend to dissolve in non-polar solvents Polar substances tend to dissolve in polar solvents.
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“Like dissolves like” It comes down to having similar intermolecular attractions.
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Gases in solution Solubility depends on intermolecular attractions
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Gases in solution Solubility depends on intermolecular attractions London forces As molar mass increases, dispersion forces are stronger
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Henry’s Law The solubility of a gas in a liquid is directly dependent on the gas pressure
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Henry’s Law The solubility of a gas in a liquid is directly dependent on the gas pressure Pressure really doesn’t affect solubility of solids and liquids
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Henry’s Law S g = kP g
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Solubility and temperature Usually, solubility of ionic solids increases with temperature
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Gas solubility and temperature Solubility of gases typically decreases with increasing temperature
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