1. SOLUTIONS

2. SOLUTION a. HOMOGENEOUS MIXTURE
Even distribution of solute particles throughout the solvent
b. Solute: substance being dissolved
c. Solvent: substance that DOES the dissolving
d TYPES
(s) in (l) = Salt water
(g) in (l) = Soda
(l) in (l) = vinegar
(g) in (g) = air
(s) in (s) = alloy
(l) in (s) = Hg in Ag
e. CHARACTERISTICS
1. Transparent (if liquid)
2. Solute particles small (Ions, atoms, small molecules  1 nm)

3. 3. Does not settle out on standing
4. Cannot be separated by filtering
5. Does NOT show the Tyndall effect
SUSPENSIONS - Dirt in water
1. Heterogeneous
2. Settle out on standing
3. CAN be separated by filtering
4. Do show the Tyndall effect
COLLOIDS
Ex. Dust in air, jello, fog, mayonnaise, glue)
Definition: Suspension of very fine particles ( 1nm  1000 nm)
1. Do not settle out on standing
2. Cannot be separated by filtering
3. DO show the Tyndall effect
4. Colloidal particles CANNOT pass through parchment

4. TERMS TINCTURE: MISCIBLE: IMMISCIBLE: CONCENTRATION or
Solution with alcohol as the solvent
Ex. Tincture of iodine
MISCIBLE:
Two liquids which are completely soluble in one another
Ex. Ethanol and water
IMMISCIBLE:
Liquids which do not dissolve in one another
Ex. Oil in water
CONCENTRATION
MASS PERCENT
% = mass solute__ x 100
mass solution
Mass solute = __X__
Mass solution
MOLARITY (M)
Number of moles of solute per liter of solution
Molarity = moles solute
liter solution or
M = mol L

5. 1.Given: 5.0% solution of HCl
How many grams of HCl in 25 g of solution?
What is the mass of water in 150. g solution?
Find the number of grams of solution containing 13.2 g of HCl.

6. 2. A water solution of H2O2 contains 3.0% H2O2 by mass.
a. Find the mass % of water in the solution.
b. How many grams of solution are needed to furnish 1.0 g of H2O2?
c. How many grams of water are present in 1.00 liter of solution, D = 1.01 g/cm3?

7. MOLARITY PROBLEMS
1. What is the molarity of a solution in which moles of C2H5OH is dissolved in 200. ml solution?
2. What mass of sodium hydroxide ( ) is needed to prepare 300. ml of a M solution?

8. 3. Calculate the molarity of a solution containing 68
3. Calculate the molarity of a solution containing 68.0 g of silver nitrate( ) in 150. ml of solution.

9. 4. What volume of 0. 20 M solution can be prepared when 2
4. What volume of 0.20 M solution can be prepared when 2.8 g of KOH ( ) is dissolved in water?

10. MAKING UP A MOLAR SOLUTION
Prepare 500. ml of a 1.50 M solution.

11. SOLVENTS ARE SELECTIVE
The possibility of solvent action is increased by similarity in composition and structure.
“LIKE DISSOLVES LIKE”
SOLVATION SOLUTES IN EQUATIONS
NaCl(s) 
Cl2(g) 
AgNO3(s) 
MgI2(s) 
C6H12O6(s) 

12. SOLVENT SOLUTE
1. Polar (ex. H2O)
1a. Ionic (ex. NaCl)
b. Polar – such as acids (HCl) or
molecules that form H bonds
ex. C2H5OH
2. Nonpolar (ex. C6H6, organic
solvents)
2. Nonpolar (I2, oil, grease)
3. Polar/Nonpolar
(ex. C2H5OH)
3. Polar/nonpolar (CH3OH)
Some polar (H2O), some nonpolar(I2)
SOLUBILITY
Grams solute that can dissolve in 100 g of water at a particular temperature.
SOLUTION EQUILIBRIUM
Saturated solution!
At first: C12H22O11(s)  C12H22O11(aq) Mostly dissolving
Then recrystallizing begins: C12H22O11(aq)  C12H22O11(s)
Eventually, C12H22O11(aq)  C12H22O11(s)
Dynamic Equilibrium

13. Solution Equilibrium Saturated Solution Then, rate of dissolving is
equal to the rate of crystallization
*NO OVERALL CHANGE
At first, rate of dissolving
is greater than
rate of crystallizing
C12H22O11(aq)  C12H22O11(s)
Dynamic Equilibrium

14. EQUILIBRIUM CONCENTRATION DOES DEPEND ON:
1. Temperature
2. Nature of the solute and solvent

15. Solution Classification
Saturated solution
1.Has as much solute as a solvent can hold at a given temperature
2. Add a crystal, it
falls to bottom.
3. Solution equilibrium

16. Unsaturated solution
1. Contains less solute than it could hold at a given temperature
2. Add a crystal – it
dissolves

17. Supersaturated solution
1. Holds more solute than it can normally hold at a given temperature
2. Add a crystal – excess falls out
3. Unstable!

18. Effect of Temperature on Solubility
1. Increasing temperature __________ the solubility of a solid in a liquid.
increases

19. 2. Increasing temperature _________ the solubility of gas in a liquid.
cool warm
decreases

20. Pressure and Solubility
3.Increasing pressure _______________ the solubility of a gas in a liquid .
(Does not affect a solid in a liquid.)
increases

21. g, 80 g
2. supersaturated
= 44 g
g water
5. 72o C
6. NH3
= 17 g
8. 20o C

22. Increasing the rate of dissolving
(How fast, not how much)
1. Stir it
2. Heat it
3. Crush it
The more opportunities for solute and solvent to have contact, the faster solution will occur!

23. PHYSICAL PROPERTIES OF SOLUTIONS
1.ELECTROLYTES
Substances whose solutions conduct electricity
a. Solutes dissolve as _______________.
b. Types of compounds: _______________________________.
c. Examples:
KI(s) 
HCl(g) 
IONS
IONIC COMPOUNDS, ACIDS
K+(aq) + I-(aq)
H+(aq) + Cl-(aq)
d. Why do they conduct?

24. COLLIGATIVE PROPERTIES
NONELECTROLYTES
Substances whose solutions do NOT conduct electricity
a. Solutes dissolve as __________________________.
b. Types of compounds: ___________________________________.
c. Examples:
molecules
covalent, except acids
C12H22O11, C2H5OH, Br2
COLLIGATIVE PROPERTIES
DEFINITION:
Properties which depend on the NUMBER of particles in solution, not the NATURE of the particles

25. a. VAPOR PRESSURE LOWERING
1. Addition of a solute LOWERS the vapor pressure of a solvent
2. The lowering is proportional to the concentration of the solute
VAPOR PRESSURE LOWERING IN WATER SOLUTIONS AT 25oC
Concentration Glucose Sucrose
(mol/L) (mm Hg) (mm Hg)
b. BOILING POINT ELEVATION, FREEZING POINT LOWERING
HIGHER
1. The boiling points of solutions are ______________ than those of pure solvents.

27. 2. The freezing points of solutions are _________________ than those of pure solvents.
3. The amount of elevation or lowering is directly proportional to the concentration of the PARTICLES in solution.
4. ELECTROLYTES have a greater effect on boiling point & freezing point than NONELECTROLYTES.
Dissolving 1 mole: # particles
a. C12H22O11(s) 
b. NaF(s) 
c. MgCl2(s) 
d. Al2(SO4)3(s) 
LOWER
C12H22O11(aq)
1 mole
Na+(aq) + F-(aq)
2 moles
Mg+2(aq) + 2 Cl-(aq)
3 moles
2 Al+3(aq) + 3 SO4-2(aq)
5 moles
Which solute has the MOST effect?
Al2(SO4)3
Which solute has the LEAST effect?
C12H22O11

29. molality (m) Molality (m) = moles solute kg solvent
And ΔTf = (# particles per unit)(m)(1.86 kg0C/mol)
FREEZING PT DEPRESSION CONSTANT FOR H2O
ΔTb = (# particles per unit)(m)(0.52 kg0C/mol)
BOILING PT ELEVATION CONSTANT FOR H2O
1. What is the freezing point of a 2.00 m solution of Ca(NO3)2?

30. 2. What is the freezing point of a 2.00 m solution of C2H5OH?

31. 3. Calculate the boiling point of a 1.5 m NaCl solution.

32. 4. When 1. 56 g of methanol is dissolved in 200
4. When 1.56 g of methanol is dissolved in 200. g of water, the freezing point depression of the solvent is 0.453oC. Find the molecular mass of the solute.

33. SOLUTION DILUTION
Moles solute stock solution = Moles solute prepared solution
Vconc x Mconc = Vdilute x Mdilute
Because L x mol/L = L x mol/L
1. Prepare 100. ml of a 0.50 M HCl solution from a stock 6.0 M HCl solution.
2.What volume of a 12 M HCl solution is needed to prepare 50. ml of a 1.5 M HCl solution?

34. Deliquescence
The process by which a solid picks up water from the air
Ex. Calcium chloride – used in labs as a drying agent