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Define solution, solute, solvent and solubility.
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Describe the driving force for solution formation.
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Explain the effect of intermolecular forces on solution formation.
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Describe the overall process of solution formation and the enthalpy changes associated with it. Define heat of hydration.
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Explain dynamic equilibrium with respect to solution formation.
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Define: saturated, unsaturated and supersaturated solutions.
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Describe the temperature dependence of the solubility of solids.
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Describe the factors affecting the solubility of gases in water.
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Solve gas solubility problems using Henry’s Law.
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Define and perform calculations using common units to express solution concentrations including: molarity (M), molality (m), mole fraction (X), mole percent (mol %), percent by mass or volume (%). Convert from one concentration unit to another.
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Define: parts per million (ppm) and parts per billion (ppb) by mass or volume.
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Describe the effect on the vapor pressure of the solvent upon the addition of either a nonvolatile, nonelectrolyte solute or a nonvolatile, electrolyte solute.
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Calculate the vapor pressure of solutions containing non-volatile solutes using Raoult’s law.
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Calculate the vapor pressure of solutions containing volatile solutes using Raoult’s law.
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Explain the difference between an ideal and a non-ideal solution.
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Explain why the lower vapor pressure for a solution containing a nonvolatile solute also results in a higher boiling point and a lower melting point compared to the pure solvent.
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Define colligative properties, osmosis and osmotic pressure.
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Perform calculations involving freezing point depression, boiling point elevation, and osmotic pressure.
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Explain the role and meaning of the van’t Hoff factor in determining the colligative properties of solutions containing strong electrolytes.
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Describe the difference between a colloidal dispersion (colloid) and a solution.
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Describe the Tyndall effect and how it can be used to identify colloids.
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