CH 1020- Final Exam Guide - Comprehensive Notes for the exam ( 103 pages long!)

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28 Mar 2018
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Clemson U
CH 1020
Final EXAM
STUDY GUIDE
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Ch 11 Properties of solutions (3.5)
Energy changes during dissolving
Vapor pressure: Claussius-Clapeyron Equation
Mixtures of volatile substances
Colligatie properties: Raoult’s La, Molality, Boiling
Point eleation, freezing point depression, an’t Hoff
factor
Osmosis and osmotic pressure
Use colligative pressure to determine molar mass
Add this to your homework: Ch 11 terms to look up
and know
Mixture
Heterogeneous
Homogeneous
Solution
Solute
Solvent
3 types of interactions to form a solution
Like dissolves like
Molarity
Molality
%mass
Mole fraction
Big Ideas
The process of solution formation involves both entropy
and enthalpy changes.
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Like dissolves like.
Colligative properties are entropy driven and therefore
only depend on the number of particles in solution.
Objectives
Distinguish between solutes and solvents.
Explain the phrase "like dissolves like" in terms of the
types of interactions between particles in a solution.
Describe the solvation process of an ionic salt in water.
Explain the stability of a solvated ion.
Explain why the entropy of solution formation is positive
for most substances.
Explain why the enthalpy of solution formation may be
positive or negative in terms of the energy changes
associated with breaking and making intermolecular
attractions.
Express solution concentrations in terms of molarity,
molality, mole fraction, mass percent and related units.
Be able to convert between these units. Perform
calculations involving these units.
Know when and why each of these units is used.
Explain the effects of temperature and pressure on the
solubility of solids, liquids and gases.
Relate Henry’s La to the solubility of gases. (Section
10.10)
Explain the differences in vapor pressure in pure
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