Agenda:
Homework:
New Element Project
 Warm-up: Explain the solvation process
 Review – terms, importance, “likes dissolve likes”
 Solubility Curves
 What can they tell us about solutions?
 Measuring concentration of solutions
Warm-up: Solvation Process
 Explain what is happening when an ionic compound is
dissolved in water (called solvation or hydration)
 View the video - what are key steps that need?
 How does the water molecules interact with the ionic
compound?
 http://group.chem.iastate.edu/Greenbowe/sections/pro
jectfolder/flashfiles/thermochem/solutionSalt.html
a. Making Solutions: Molecules
(Covalent compounds)
 General Rule: “Likes dissolve likes”
Polar solutes can dissolve in polar solvents.
Examples:
Organic solvents
 Non-polar solute can dissolve in non-
polar solvents
 Examples:
To remove oily stains in dry-cleaning
 Lipids will dissolve in hydrocarbon
 To clean oil based paints
 To manufacture plastics, man-made fibers,
adhesives

Solution process
Solution process
 Animations
 https://www.youtube.com/watch?v=EBfGcTAJF4o
b. Making Solutions: Factors that impact the
solubility of solids in liquids
 Energy is involved – 2 steps
 Endothermic to separate solute & solvent particles
 Exothermics – attraction between solvent & solute particles
Factors affecting solids
dissolving in liquids
General trend to increase
solubility
Chemical components of solute and
solvent
Intermolecular forces
Temperature
Particle size
Agitation (amount of stirring)
High attraction between solute and
solvent particles
c. Measuring Concentration
 Solubility: number of grams of solute in 100 grams of
water at 20℃
 Solubility Curves
 Saturated solutions
 Unsaturated
 Supersaturated


http://www.youtube.com/watch?v=XSGvy2FPfCw
http://www.youtube.com/watch?v=1y3bKIOkcmk&feature=re
lated
Interpreting
solubility curves
Y axis
X axis
Lines
If the amount needed is
more or less than 100 g
of H₂O
1 g H₂0 = 1 mL H₂0
c. Making solutions: Factors that affect the
solubility of gases in liquids
Think about soda (carbonated drinks)
Factors affecting gases
Temperature
Pressure
General trends to increase
solubility
Solubility Rules determined under specified
concentration (often 0.1% molarity)
Except with
these ions
Category
Ions
Soluble cations
Group 1 ions
No exceptions
and ammonium, NH4+
NO3- and
Soluble anions
C2H3O2Usually soluble
anions
Cl-, Br-, and I-
SO42-
Usually
insoluble
anions
CO32-, PO43-, and OH-
No exceptions
Soluble:
Exceptions: Ag+
and Pb2+
Soluble
Exceptions:
Ba2+ and Pb2+
Examples
Na2CO3, LiOH, and
(NH4)2S are soluble.
Bi(NO3)3, and
Co(C2H3O2)2 are soluble.
CuCl2 is water soluble,
but AgCl is insoluble.
FeSO4 is water soluble,
but BaSO4 is insoluble.
CaCO3, Ca3(PO4)2, and
Insoluble:
Mn(OH)2 are insoluble in
Exceptions: group
water, but (NH4)2CO3,
1 elements and
Li3PO4, and CsOH are
NH4+
soluble.
d. Measuring Concentrations
 Molarity (M) by definition =
 Molarity = Moles of solute
1 Liter of solution


Therefore: 2 molar solution = __________________
 Discovery Education video

Standard Deviants School Chemistry: solutions & dilutions
Molarity: moles of solute
liters of solution
Molarity problems M= moles_______
1 Liter solution
 What I s the molarity of a solution in which 58 gram of
NaCl are dissolved in 1.0 L of solution?
 What is the molarity of a solution in which 10.0 grams
of silver I nitrate is dissolved in 500 mL of solution?
 How many grams of potassium nitrate should be used
to prepare a 2.0 L of a 0.5 molar solution?
Steps needed in molarity
calculations
 Moles
For grams:
 Liters of solution
 If less than 1L ? mL = 1L
 Comparison __________ = moles of solute
1 liter of solution
Molarity practice
 To what volume should 5.0 g of KCl be diluted in order
to prepare a 0.25M solution?
 How many grams of copper II sulfate – penta hydrate
are needed to prepare 100 mL of a 0.10M solution?
9g. Dilution of concentrated
solutions:
V₁M₁= V₂M₂
 Molarity by dilution practice problems
 Most reagents are sold & sorted in concentrated
solutions
 How much concentrated 18M sulfuric acid is needed to
prepare 250mL of a 6.0M solution?
 How much concentrated 12M hydrochloric acid is
needed to prepare 100 mL of a 2.0 M solution?
 To what volume should 25 mL of 15 M nitric actid be
diluted to prepare a 3.0 M solution?
 To how much water should 50 mL of 12 M hydrochloric
acid be added to produce a 4.0 M solution?
 To how much water should 100 mL of 18M sulfuric acid be
added to prepare 1.5 M solution?
Colligative Properties
 The properties of the solution that depend on the
number of particles in solution, not the identity of the
solute.
 The solvent properties will be changed.
 NaCl
 CaCl₂
 AlCl₃
 Melting point depression; boiling point elevation;
 Vapor pressure lowering
Resources
 http://www.karentimber
 http://www.chemistryge
lake.com/solution.htm
 http://www.afn.org/~afn
02809/powerpointlist.htm
ek.com/chemistrypower
point/Student%20Ch%2
015%20Solutions.ppt
 http://college.cengage.co
m/chemistry/general/zu
mdahl/world_of_chem/1
e/instructors/ppt/figures
/viewindex.html
Solution process